Tactics of Passing Chemistry

Learning chemistry made easier Stop watch 2 In This stop watch an hour timing is indicated. It is important to note that in an exam it is hard to get timing in hours. When reset it reads 0:00:0000. It is reading; Zero hours, zero minutes, zero seconds and zero centiseconds. When you start and stop immediately and may be it read 0:00:0055, these are 55centiseconds. If it reads 0:00:1025 , these are 10 seconds and 25 centiseconds or 10.25 seconds. If it read 0:01:3638, these are zero hour, 1 minute, 36 seconds and 38 centiseconds. If required to give time in seconds you have to convert the minutes into seconds ie {(1 x 60) + 36} = 60 + 36 = 96.38 seconds. Common mistakes among the students when recording time are • Confusing centiseconds with milliseconds. The Last two digits to the right of the stopwatch is not milliseconds it is 1/100th of a seconds. • Ignoring centiseconds - this may cause errors which are shown mostly when drawing the graph. For instance if stopped at 0:1025 or 0:00:1025 on either of the stop watch the time is 10.25seconds not 10 seconds. (Failure to indicate centiseconds may not be penalized in chemistry) • Wrong interpretation - This is due to lack of understanding how to read the stop watch. For instance if the readings are same as 0:1025 or 0:00:1025 on either of the stop watch the time is 10.25seconds not 0.10 seconds or 0.01025seconds. • Consistency of the decimal places - this is also very important. A correct time is recorded to two decimal places. This recording must be maintained. Sample question 84 You are provided with: • 1M Acidified potassium manganate (VI) solution, U. • 1M Oxalic acid solution, W. 189

Tactics of Chemistry You are required to determine the effect of temperature on the reaction of potassium manganate (VII) with oxalic acid. Procedure • Using a measuring cylinder, place 10 cm3 portions of solution U into five separate test tubes in a test tube rack. • Clean the measuring cylinder and use it to measure 10 cm3 of solution W. Transfer it into a boiling tube. • Place the boiling tube in the water bath provided and heat W to a temperature of 400C. • Add the first portion of solution U to the boiling tube. Shake and at the same time start the stop-watch. • Record the time taken for the purple colour of the mixture to decolourise in the table below. • Repeat the experiment by using 10 cm3 of solution W at temperatures of 500C, 600C, 700C and 800C. Complete the table below. {5 marks} Temperature of solution W(0C) 40 50 60 70 80 Time taken for W to decolourise (t) 55.41 44.75 29.15 17.54 12.03 seconds 1/t (s-1) 0.018 0.022 0.034 0.057 0.083 The 5 marks are distributed as follows 1. Complete Table … 2 ½ mark - Complete column … ½ mark - Accept concentration to at least 3 decimals places otherwise penalize 1mk once for rounding off 2. Decimals….. 1mark -Values recorded to whole numbers or to 1 decimal place which must either be 0 or 5 3. Accuracy…. 1mark -Compare the candidates time at 1st experiment and if within 2 units, award 1 mark, of beyond, award 0mark 190

Learning chemistry made easier 4. Trend …. ½mark -Award ½ mark for continuous rise / increase in temperature, otherwise penalize fully i.e 0 mark a. Plot a graph of temperature against 1/time. (3 marks) 10-2 80 70 x 60 50 (s-1) 40 30 1/ 20 Time 10 0 40 50 60 70 80 Temperature (0C) The three marks are distributed as follows Graph …. 3 marks 191

Tactics of Chemistry 1. Scale … ½ mark • At lease 2/3 of the grid provided • Scale (intervals) must be consistent 2. Labelling of axes …. ½ mark • Both the x – axis and y – axis must be labeled with units. • Penalise fully i.e 0 mark if : • Units are not shown on both or either of the axes • Axes are inter charged. • Wrong units are shown 3. Plotting …… 1mark • 5 points correctly plotted … 1mark • 4 points correctly plotted ….. ½ mark • Below 4 points plotted ………0 mark • Award for plots even if axes are interchanged N/B: not all interchanged axes are marked correct. It depends with the type of a graph. Avoid interchanging the axes. • Award for plots if intervals are consistent but the area of grid covered is less than 2/3 4. Curve ….. 1mk - Accept smooth curve for 1mark otherwise penalize fully b. From the graph, determine the time taken for decolourization of the mixture when the temperature of solution W was 650C.(1 mark) - ½ mark on the graph for working - ½ 1⁄t = 1/4.5 x 10⁻2 s⁻1 t = 22.22 seconds c. How does the rate of reaction of potassium manganate (VII) with oxalic acid vary with temperature. (1 mark) An increase in temperature increases the rate of the reaction. 192

Learning chemistry made easier iii. Volume Volume can be measured from the following instruments. • Volumetric flask • Measuring cylinder • Burette • Pipette The measurement of the instruments Volumetric flasks and the pipette have fixed measurements. Volumetric flask can be 1000ml, 500ml, 250ml, 100, 50ml etc. These volumes are up to the mark as indicated on its neck. Burette can measure a maximum volume of 50cm3 at once while measuring cylinder can measure up 1000cm3. They are of different volumes commonly up to 5cm3, 10cm3, 50cm3 193

Tactics of Chemistry 100cm3, 500cm3, 1000cm3 . Remember that the level considered is at the lower part of the meniscus. Your eyes must be perpendicular to the reading and not at an angle to avoid parallax errors. The accuracy of the instruments. We can consider the burette because it is mostly preferred for measuring volumes with higher accuracy. On this section of a burette between 13 and 14 is divided in to 10 sections. Therefore each division is 1/10 = 0.1cm3. This means the accuracy of the burette is to the nearest 0.1cm3. Readings such as 10.3, 10.4, 20.7, etc are acceptable. Sometimes the reading my lie between two divisions, it is accepted when estimated to the nearest next reading or 0.05 of the reading. The burette reading should have the second decimal place as either 0 or 5. Readings such as 9.20, 10.35, 15.00, 35.55, 40.25... are acceptable. Readings such as 20.11, 30.17, 40.69 are invalid. The consistency of recording the decimal places must also be maintained. Refer the filling titration tables. Measuring cylinder`s use depends on the volume required to be measured. This measuring cylinder This measuring cylinder is suitable for volumes in is suitable for volumes in ranges of tens. ranges of twos 194

Learning chemistry made easier NOTE: Don`t use the solution in the instrument for the part which is not calibrated. A good example is a burette. The solution beyond 50cm3, is not used. Other instruments you may use includes iv. Length Mostly a ruler is used when measuring the lengths of a precipitate in a test tube, length of a magnesium ribbon etc. The accuracy of a ruler is to the nearest 0.1cm or 1mm. Values like 0.5cm, 1.3cm, 10.5cm are expected. In 0.12cm, case of a second decimal 0.16cm are place it has to be 0 not acceptable or 5. Readings because the second such as decimal place cannot be determined from an instrument such as a ruler. The most exact is the first decimal place, when measured to the nearest cm. v. Mass A balance is used when measuring the mass of a substance. The common balances in school laboratory measures in grams. before you use the balance ensure that the reading is set at 0.0g, and the units are in grams. Do not use mass which is beyond the limit of the balance. It may destroy the balance. 195

Tactics of Chemistry UNITS OF MEASUREMENT IN CHEMISTRY In calculation the correct units must be indicated. It is always appropriate to give a quantity in its SI units( International Systems of unit). Chemistry uses small portions of matter and it may not be possible to use full units. It is therefore recommended to indicate the units of any answer. The penalties are in the following area 1. Failure to indicate the units. When indicating the units it can be done in two ways. • Indicating the units at the root of the answer. Eg • Indicating the units after the answer Sample question 85 Calculate the current passed if a mass of copper of 0.234g of copper is deposited in 4 minutes. (1F=96,500C, Cu = 63.5) Units at the root Units after the answer Current in Amperes Cu(s) Cu2+(aq) + 2e- Cu(s) Cu2+(aq) + 2e- To deposit mole To deposit mole = 96,500 x 2 = 96,500 x 2 = 193,000 C = 193,000 C To Deposit 0.234g To Deposit 0.234g = 0.235 x 193, 000 = 0.235 x 193, 000 63.5 63.5 = 711.21C = 711.21C Current in Amperes I = Q/t I = Q/t = 711.21 = 711.21 4 x 60 4 x 60 = 2.96 Amperes or 2.96A = 2.96 2. Giving wrong units. This is another problem student face. Wrong units are also penalized. 196

Learning chemistry made easier The following are the SI units commonly used in some quantities in chemistry. Quantity SI units SI Units Sub-multiple/ Symbol symbol Multiples Mass Kilogram g Energy Joules Kg Grams kJ Kilo joules cm3 Volume Cubic metre J Cubic centimeter l M3 dm3 Length Litres cm Metres m Cubic decimeter mm Time min Current Seconds S centimetres Potential difference Amperes A millimetres Electromotive force V Charge Volts Minutes Pressure Coulombs C Solubility Atmospheres atm Molarity Pascals Pa mmHg mmHg Substance cmHg cmHg Heating value Torr Torr Absolute Mass/100cm3 of g/100cm3 Temperature Temperature water Of H20 Rate of diffusion Moles/ litre Molar, M Mass/litre g/litre Moles mol Joules/gram J/g Kelvin K Degree Celsius 0C Cubic centimeter cm3/s per second 197

Tactics of Chemistry HANDWRITING , GRAMMATICAL ERRORS & SPELLING. A lot of time, students fail due to their poor hand writing. Your hand writing should be legible in all exams. Poor hand writing may contribute to the following. »» Contacts of chemical symbols which may lead to fail. »» Incomplete words which may alter the meaning of your statements. »» Illegible words which may alter the meaning or the understanding of the sentences. Grammatical errors should also be avoided, Your statements and your explanations must show coherency of facts. Spelling mistakes should also be avoided, note that all spelling mistakes are strictly penalized if the meaning intended is completely altered. 198

Learning chemistry made easier Sample KCSE Exams

Tactics of Chemistry Tactical Paper I PAPER 1. [80 marks] 1. The diagram below shows a reaction between carbon (IV) oxide and charcoal to produce gas X. Combustion tube CO gas CO2 gas Heat Charcoal Water KOH(aq) i. Identify gas X ( 1 mark) ii. Write an equation for the reaction between carbon (IV) oxide and charcoal. ( 1 mark) iii. What is the purpose of concentrated potassium hydroxide solution? (1 mark) iv. State two uses of gas X. ( 1 mark) 2. A solution of aluminium chloride in methylbenzene has no effect on litmus, while a solution of aluminium chloride in water turns blue litmus red. Explain. ( 2 marks) 3. John a form 4 student found that the pages of her chemistry note book she used in form one and kept in an open shelf had turned from white to brown while the pages of her new note book were still white. Explain.( 2 marks) 4. The diagram below illustrates an experiment to investigate the effect of an electric current on dilute copper (II) Sulphate solution. A Beaker Carbon electrode X Carbon electrode Y Copper (II) sulphate solution 200

Learning chemistry made easier a. Identify one mistake in the set – up. ( 1 mark). b. Identify carbon electrodes X and Y. ( 1 mark) X………………………… Y…………………………. c. State and explain the observations made on the solution at the end of the experiment after the mistake was rectified. (2 marks) 5. Diamond and graphite are allotropes of carbon. Diamond is hard and used for drilling while graphite is soft and used as a lubricant. ( 2 marks) 6. State two reasons why aluminium is preferred to copper in making overhead electric cables. ( 2 marks) 7. The set – up below shows an experiment set to prepare iron (II) chloride. i. State the name of the method of salt preparation shown in the set – up above. (1 mark) ii. State the property of iron (III) chloride that makes it possible, for it to prepared as shown in the set – up. ( 1 mark) iii. What is the function of the anhydrous calcium chloride in the U - tube. ( 1mark) iv. Explain why iron (III) chloride is formed in this set up and not iron (II) chloride. ( 1 mark) 8. Sodium oxide has a melting point of 11320C while Sulphur (IV) oxide has a melting point of -750C. Explain this observation in terms of structure and bonding. (2 marks) 9. Kamau found a sample of sodium chloride contaminated with glucose and lead (II) chloride. Describe how he separates them so as to obtain a pure dry sample of each. (3 marks) 10. Most apparatus in a chemistry laboratory are made of glass. Give two reasons for this . (2 marks) 201

Tactics of Chemistry 11. The diagram below shows an experiment to demonstrate one property of hydrogen gas. a. Which property is demonstrated above? (1 mark) b. State one observation made in the combustion tube.(1 mark) c. Explain the following i. The combustion tube is in a slanting position.(1mark) ii. The unreacted hydrogen is ignited at the end of the combustion tube. ( 1 mark) 12. Draw the structure of the following compounds i. 2,3 – dimethyl butan – 1 – ol. (1 mark) ii. Hexan –1,6 – dioc acid. ( 1mark) 13. When Concentrated nitric (V) acid was added into a boiling tube containing iron (II) sulphate solution which had been acidified with sulphuric (VI) acid it produces colourless gas A which turn into brown fumes B at the mouth of the boiling tube. i. Identify colourless gas A( 1 mark) ii. Explain how brown fumes B are formed.( 1 mark) iii. Write an equation for the reaction between concentrated nitric (V) acid and iron (II) sulphate in sulphuric (VI) acid. ( 1 mark) iv. State two uses of nitric ( V) acid. ( 1mark) 14. 30 cm3 of dry ammonia gas were mixed with 40 cm3 of dry hydrogen chloride gas in a glass tube as shown below. a. What observations were made when the two gases were mixed. ( 1 mark) 202

Learning chemistry made easier b. Which gas was in excess and by what volume. ( 2 marks) c. Write an equation for the reaction between dry ammonia gas and dry hydrogen chloride gas. ( 1mark) 15. 5 ml of 1M potassium iodide solution completely reacted with 2.5 ml of 1 M lead (II) nitrate solution. a. Use this information to calculate the number of moles of iodide ions that reacted with one mole of lead (II) ion. (3 marks) b. Write an ionic equation for this reaction ( 1 mark) 16. Study the flow chart below and use it to answer the questions below. White precipitate NaCl(aq) Colourless NaOH(aq) White precipitate W Step 1 solution A Step 2 P Excess NaOH(aq) Colourless solution B Aluminium foil Warm Colourless gas turns red litmus blue a. Identify the anion and cation present in solution A. ( 1 mark) Cation …………………….. Anion……………………….. b. Write an ionic equation in i. Step 1 ( 1 mark) ii. Step 2 ( 1 mark) c. Write the formula of the complex ion in solution E. ( 1 mark) 17. Use the reduction potentials below to answer the questions that follow. E0 (v) A 2+ + 2e A(s) -0.76 (aq) B2+ + 2e B(s) -1.92 ( aq) C(s) +0.34 C2+ + 2e (aq) D+ + e D(s) +0.84 (aq) a. Identify the strongest reducing agent. ( 1 mark) 203

Tactics of Chemistry b. Which two half cells if connected will give the least e.m.f. ( 1 mark) c. Calculate the e.m.f of the cell in (b) above. ( 1 mark) d. Draw a cell diagram to represent the cell in (b) above. (1 mark) 18. I) In terms of functional group distinguish between soap and soapless detergent. ( 1 mark) II) Describe how detergents remove grease from fabrics when used with water. ( 2 marks) 19. The graph below shows the volume of carbon (IV) oxide produced when 5g of marble chips react with 50 ml of 1M hydrochloric acid. Volume of CO2 Time ( min) a. Explain the shape of the graph ( 2 mark) b. On the same axis show the graph that would be obtained if marble powder was used in place of marble chips.( 1 mark) 20. Distinguish between nuclear fusion and nuclear fission (2 mark) 21. State two advantages of synthetic polymers over natural polymers.( 2 marks) 22. Bond energies for some bonds are tabulated below:- Bond Bond Energy KJ/mol H – H 436 C = C 610 C - H 410 C - C 345 Use the bond energies to estimate the enthalpy for the reaction. (3 marks) C2H4(g) + H2(g) C2H6(g) 23. a. State the observation made at the end of the experiment when a mixture of 204

Learning chemistry made easier iron powder and sulphur are heated in a test-tube (1 mark) b. Write an equation for the reaction between the product in (a) above and dilute hydrochloric acid. ( 1mark) c. When a mixture of iron powder and sulphur is heated it glows more brightly than that of iron fillings and sulphur. Explain this observation. ( 2marks) 24. a. What is meant by the term solubility of salts? ( 1 mark) b. Calculate the solubility of magnesium chloride given that 15g of the salt can saturate 25cm3 of water at 250C. ( 1 mark). 25. A given drink was analyzed to find out the sugars present in it using chromatography. The diagram below shows the spots after the chromatogram was developed. T U VWX Drink Z Sugars a. Name the sugars present in Z. (1mark) b. Which of the sugars has the lowest density? Explain. (2marks) 26. When excess dilute hydrochloric acid was added to sodium sulphite, 960cm3 of sulphuric (IV) Oxide gas was produced. Calculate the mass of sodium sulphate that was used. ( 3 marks) (Molar gas volume=24.0dm3 and S=32 Na=23, O=16). 27. Name the chief ores from which the following metals are extracted a. Aluminium ……………………………… ( 1 mark) b. Copper ..………………………………………( 1 mark) 205

Tactics of Chemistry PAPER 2 [80 MARKS]. 1. a. Name the following compounds i. CH3CH2CH2CH2CH2OH (1mark) ii. CH3CH (CH3) CH2COOH (1 mark) iii. CH3CH2 COOCH2CH3 (1mark) iv. Study the diagram below and answer the questions that follows Compound C K2Cr2O7(aq)/H+ Propan-1-ol Na Gas A Compoud B Reactant D Bromine Gas Polymer Prop-1-ene F E Step 1 Propane Cracking E Methane b. Identify the product. B..................................... (1 mark) F...................................... ( 1 mark) c. Name the compound. C ...................................... ( 1 mark) E ...................................... ( 1 mark) d. State the conditions for step 1 (1mark) e. Write the equation for the reaction leading to the formation of methane. (1mark) f. State two industrial uses of methane. (2marks) g. Identify the reagent D. (1mark) 2. The diagram below was set-up by a student to investigate one of the chemical properties of ammonia. Use it to answer the questions that follow. 206

Learning chemistry made easier Copper (II) oxide a. State and explain the observation that would be made in the combustion tube. (2marks) b. Write down a well-balanced chemical equation for the reaction taking place in the combustion tube. (1mark) c. Which property of ammonia is investigated above? (½ mark) d. Identify i. Gas R (½ mark) ii. Liquid Q and give its chemical test. ( 1 mark) e. Below is set up of apparatus used to react ammonia gas with iron (II) chloride solution. Use it to answer the questions that follow i. State observation made in the beaker. (1mark) ii. Give a reason for using a funnel to deliver ammonia into the beaker. (1mark) f. The flow chart below shows a network of reactions starting with sodium nitrate and ammonium chloride. Study it and use it to answer the questions that follow 207

Tactics of Chemistry Ammonium Step 6 Salt B, chloride solution Heat Gas W + water Water Sodium Nitrate Step 5 Solid V Heat Step 1 Liquid X Gas K Sodium 50% nitric Step 2 Step 4 hydrogen (V) acid Copper Solution P Substance V sulphate SteCp o3pper Excess Process A NH3(g) + water 70% nitric (V) acid i. State the difference that occurs between Step 2 and Step 3. (1mark) ii. Identify: I. Liquid X (½mark) II. Process A (½ mark) (½mark) III. Gas K (½mark) IV. Gas W iii. State and explain the observation made in Step 4. (2mks) iv. Write the equation for the reaction that take place in step 6: (1mark) 3. a. The following electrochemical cell was set-up at 250C and one atmosphere. Cd2+(aq)+ 2e Cd(s) +0.4v I2(s) + 2e 2I-(aq) +0.54v Br2(l) + 2e 2Br-(aq) +1.09v Ag+(aq) + e Ag(s) +0.84v Cr3+(aq) + 3e Cr(s) -0.74v 208

Learning chemistry made easier Given the above standard electrode potentials, give advice to someone who would like to store a solution of cadmium (Cd) in a container made up of chromium (Cr). Show your workings. (2 marks) i. Calculate the e.m.f for the cell. (1mark) Ag+(aq) + e Ag(s) Cr3+(aq) + 3e Cr(s) ii. Identify I. The strongest oxidizing agent. (½ mark) II. The strongest reducing agent. (½ mark) b. The figure below shows a set-up that was used by a student to electrolyze copper (II) sulphate using copper electrode. Use it to answer the questions that follow. i. State and explain two observations that would be made during the experiment. . (2marks) ii. Write the equation for the reaction that takes place at: I. Anode (1mark) II. Cathode (1mark) c. During electrolysis of aqueous magnesium sulphate solution a current of 0.72 A was passed through the electrolyte for 15 minutes. Calculate the volume of the gas produced at the anode. (1 Faraday 96,500 Coulombs, molar gas volume is 24,000cm3 at room temperature.) (2marks) 4. a. Distinguish between thermal decomposition and thermal dissociation (2 marks) b. The flow diagram below shows a scheme for the decomposition of a salt. 209

Tactics of Chemistry White Heat White solid Q Excess Solution S deliquescent Brown gas R NaOH(aq) Excess Faint white NH3(aq) precipitate salt P i. Suggest how solid P is stored in the laboratory. (1mark) ii. Name the cation in solid P. (½ mark) iii. Write the formula of anion in the colorless solution S. (½ mark) iv. State and explain the observation made when HCl is added to the faint white precipitate. (2marks) v. Write the equation for the decomposition of solid P. (1 mark) c. 3.31 of lead (II) nitrate was strongly heated i. Write the equation for the decomposition that occurred. (1mark) ii. Calculate the mass of the residue formed. (2 marks) (Pb = 207, N = 14, O = 16) d. Starting with lead (II) oxide describe how a sample of lead (II) carbonate can be prepared. (3marks) 5. a. The table below shows the ions of elements W, X, Y and Z and their electron arrangement. The letters do not represent the actual symbols of the elements. Ion Electronic configuration W- 2.8.8 X2+ 2.8.8 Y3+ 2.8 Z2- 2.8 i. Which two elements belong to the same period. Give a reason. (2marks) ii. In which group of the periodic table does Y3+ belong? (½ mark) iii. Write the formula of the compound formed between W and X. (1mark) iv. What type of bond is formed between W and X, Explain? (2marks) b. i. What is a co-ordinate bond. (1mark) 210

Learning chemistry made easier ii. Draw a dot (•) cross (x) diagram to show bonding in the c. Aluminumhycdhrlooxroidneiuamnd, Hs3oOd+iuiomn.c(hHlo-1ri,dOe-1a6re) (2marks) both chlorides of period 3 elements. Use this information to explain the following observations. I. AresdowluhtiiolentohfaAt ol2fCslo6 diniuwmaCtehrloturirdnesdboluees litmus paper not. (1 mark) II. The melting point of sodium chloride (8010C) is higher than that of Al2Cl6 (1800C) (1 mark) 6. a. The flow chart below shows the preparation of carbon (II) oxide and its reactions Oxalic acid Conc. KOH H2C2O4 PbO Concentrated H2SO4 Gas C Solid B i. CWNoahnmacteeintshttrehatetyerpdoeHleo2foSOrfec4a.ocn(t1cioemnntatrarakkt)iendgppoltaacsesbiuemtwheyednrHox2iCd2eO?4 and ii. (l mark) iii. Write an equation for the production of B and C. (1 mark) iv. Give two uses of carbon (II) oxide. (2 marks) v. State one use of sodium carbonate other than softening hard water. (1 mark) b. The diagram below represents a charcoal jiko burning. S R Ash P Air i. Write down the equation for the reaction that occurs in regions P, R and S. (3 marks) Region S Region P Region R 211

Tactics of Chemistry ii. State one by-product that is produced in Solvay process that is not recycled and state its use. (2 marks) The results below awtesrteanodbatardinteedmwpheerantu2r.5egaonfdMpCreOs3swureer.e 7. 2M nitric (V) acid reacted with excess Time (sec) 0 2 4 6 8 10 12 14 16 18 Volume of gas (cm3) 0 165 270 350 410 445 465 480 480 480 a. i. On the grid provided draw the graph of volume of gas against time (x–axis). (3mks) ii. From the graph, find the time the reaction stops. (1mark) iii. What is the maximum volume of the gas evolved? (½ mark) iv. Determine the rate of the reaction at time t = 4 seconds. (1mark) e. i. Write down the equation for the reaction. (1mark) ii. HDeetnecrem, fiinnedtthheemreollaatrivme aastosmoficMmCOas3s. (o2fmMa.r (k2sm) (aCr=k1s2) , O=16) iii. PAPER 3 [40 marks]. 1. You are provided with: • Solution A – 0.1M hydrochloric acid • Solution B – Containing 19.1g/litre of a basic compound B2X.10H2O. You are required to determine the relative atomic mass of metal B in the formula B2X.10H2O. Procedure • Fill the burette with solution A up to the zero mark. • Using a pipette and a pipette filler, place 25cm3 of solution B into a 250cm3 conical flask. • Add three drops of methyl orange indicator and titrate. • Record your results in the table below. • Repeat the procedure two more times and complete table I. Table I Titration I II III 4 marks Final Burette reading (cm3) Initial Burette reading (cm3) Volume of solution A used (cm3) a. Calculate the average volume of solution A used. (1 mark ) b. Given that one mole of B2X.10H2O reacts with 2 moles of hydrochloric acid, calculate the: i. Moles of B2X.10H2O in the volume of solution B used. (2 marks) 212

Learning chemistry made easier ii. Concentration of solution B in moles per litre. (2 marks) iii. mRReeallsaasttiiovvfeeXfaot=ormm15uic6la,mHma=asss1so.0of,fmOBe2=tXa1.l16B0.0Hin2)OB 2.X(2.1m0Ha(2r2Okms()Raerklast)ive iv. formula 2. You are provided with: • 2g of solid C 0–.O5Mxalsioclauctiiodn(oHf 2oCx2aOli4c.2aHc2iOd)(dibasic • Solution D – acid ) • Solution E – Sodium hydroxide solution. You are required to determine a. i. The molar heat of solution of solid C. ii. The enthalpy of neutralization between oxalic acid solution D and sodium hydroxide solution E. b. Calculate the heat of reaction of solid C with aqueous sodium hydroxide by applying Hess’ law. Procedure I: • Place 30cm3 of distilled water into a 100ml plastic beaker. • Measure the initial temperature of the water and record it in table II below. Add all the solid C at once. • Stir the mixture carefully with the thermometer until all the solid dissolves. Do not break the thermometer. • Measure the final temperature reached and record it in table II below. Table II Final temperature (0C) Initial temperature (0C) c. Determine the change in temperature, ΔT1. ( 1 mark ) d. Calculate the: i. Heat change when solid C dissolves in water. (Assume the heat capacity of the solution is 4.2kJkg-1k-1 and density is 1gcm-3) ( 2 marks ) ii. Moles of solid C oxalic acid (H2C2O4.2H2O) used (H = 1.0, C = 12.0, O = 16.0) ( 2 marks ) iii. Molar heat of solution, ΔH1 of solid C (oxalic acid ). (1 mark ) Procedure II: • Place 30cm3 of solution D into a clean 100ml plastic beaker. • Measure its temperature and record it in table III below. • Measure 30cm3 of solution E and measure its temperature; record it in table III below. • Add all the solution E at once to solution D in the beaker. 213

Tactics of Chemistry • Stir the mixture gently with the thermometer. • Measure the final temperature reached and record it in table III below. Table III Temperature of solution D, T1(0C) Temperature of solution E, T2(0C) Initial temperature T1 + T2 (0C) 2 Final temperature of mixture (0C) e. Determine the change in temperature, ΔT2. ( 1 mark ) f. Determine the: i. Heat change for the reaction (Assume heat capacity of solution = 4.2kJkg-1k-1 and density of solution is 1gcm-3) (2 marks) ii. Number of moles of oxalic acid, solution D used. ( 1 mark) iii. Hheyadtrooxf irdeea.c tio n, ΔH2, of one mole of oxalic acid with sodium (1 mark ) iv. Molar enthalpy of neutralization between oxalic acid and sodium hydroxide. ( 1 mark ) g. Given that: ΔM1 is the molar heat of solution of solid oxalic acid; reaction: H2C2O4(s) Water 2H+(aq) + C O 2- 2 4 (aq) ΔhMyd2riosxtihdeeh; reeaatcotfiorneaction of one mole of oxalic acid with sodium 2M+(aq) + 2OH-(aq) 2H2O(l) Calculate ΔH3, for the reaction: H2C2O4(s) + 2OH-(aq) 2H2O(l) + C O 2- (2 marks) 2 4 (aq) 3. You are provided with solid F which is a mixture of two salts. Put all the solid F provided in a boiling tube and add a about 10cm3 of distilled water. Shake to dissolve. Divide the resulting solution into four portions. a. To the first portion, add 5 drops of aqueous sodium hydroxide and heat. 214

Learning chemistry made easier Test for any gases produced using a blue and red litmus papers. Observation Inference (1 mark) (1 mark) b. To the second portion, dip a clean glass rod and vaporize a drop of the solution on a non-luminous flame. Observation Inference (1 mark) (1 mark) c. To the third portion, add 3 drops of acidified potassium manganate (VII) (KMnO4) solution. Inference Observation (1 mark) (1 mark) d. To the fourth portion, add about 5 drops of Barium chloride followed by dilute hydrochloric acid. Observation Inference (1 mark) (1 mark) Confidential for question In addition to the general apparatus in a chemistry laboratory each student is required to have the following. 1. About 100cm3 of solution A. 12. A 50ml measuring cylinder . 2. About 100cm3 of solution B. 13. One thermometer – 100C – 1100C. 3. About 60cm3 of solution D. 14. Four clean test tubes in a rack. 4. About 60cm3 of solution E. 15. One 100ml measuring cylinder. 5. 2g of solid C ( weigh accurately). 16. A 10ml measuring cylinder. 6. About 1.0g of solid F. 17. One boiling tube. 7. One burette – 50.0 ml. 18. Blue an red litmus papers. 19. One test tube holder. 8. One pipette – 25 ml. 20. Glass rod. 9. Three conical flasks. 21. Piece of tissue paper 10. One pipette filler. 11. About 500cm3 of distilled water. 215

Tactics of Chemistry ACCESS TO; 600cm3 of distilled water, warm to increase solubility ) 1. Methyl orange indicator. 2. 2M hydrochloric acid. 3. Solid C is oxalic acid (H2C2O4.2H2O). It 3. should be presented to students in a 4. 2M sodium hydroxide solution. 4. stoppered container. 5. Means of heating. 5. Acidified potassium manganate (VII) Solution D is 0.5M solution of oxalic 6. solution. acid (63g/litre) Acidified potassium manganate (VII) is Aqueous barium chloride solution. NOTES prepared by dissolving 3.16g of solid 1. Solution A 0.1M HCl KMnO4 in 500cm3 of 2MH2SO4 and Is made by dissolving 8.6cm3 of diluting to one litre solution. concentrated. HCl (1.18gcm-3) in 1 litre Solid F is a mixture of solid aNtHa4NraOt3ioanodf of solution. 6. Na2SO3 (sodium sulphite) 2. Solution B 1 : 1. Place the mixture in stoppered Is made of 19.1gl-1 of dissolving sodium containers. tetraborate decahydrate (Dissolve19.1g in Tactical Paper II PAPER 1 1. The following reaction is in equilibrium in a closed container 2SO2(g) + O2(g) ⇌ 2SO3(g) ∆H= -Ve State giving reasons how an increase in temperature would affect the amount of sulphur (VI) oxide gas. (2 marks) 2. State and explain the observation made when excess ammonia gas reacts with chlorine gas. (2 marks) 3. The diagram below is a sketch of the graph of the catalyzed decomposition of hydrogen peroxide. 2H2O2(aq) Z Catalysed Energy (kJ) 2H2O(l) + O2(g) Reaction path a. What does point Z represent. (1 mark) b. Name one suitable catalyst that can be used. (1 mark) 216

Learning chemistry made easier 4. Use the thermochemical equations below to answer the questions that follow. i. Ca(s) + C(s) + 3/2 O2(g) CaCO3(s) ΔH= -1207 kJ/Mol-1 ii. C(s) + O2(g) CO2 (s) ΔH= - 394 kJ/Mol-1 iii. Ca(s) + O2(g) CaO (s) ΔH= -635 kJ/Mol-1 a. Calculate the standard enthalpy of formation of calcium carbonate. (2 marks) b. Draw an energy cycle level diagram for the reaction represented by equation (i) (ii) and (iii). (2 marks) 5. The following are half cell reactions and their reduction potentials. The letter are not the actual symbols of the elements) Eθ(volts) i. Z2+ + 2e- Z (s) - 0.76 (aq) ii. M2+ + 2e - M (s) - 0.13 iii. S+(aq)+ e- S (s) +0.80 iv. T2+ + 2e- T (s) + 0.30 (aq) a. Write the cell representation for the electrochemical cell that would give the highest Eθ . (1mark) b. Calculate the Eθ value for the cell represented in 5(a) above. (2 marks) 6. The table below shows the relative molecular masses and boiling points of propan-l-ol and Ethanoic acid. Relative Molecular Mass Boiling point (0C) Propan –l-ol 60 36 Ethanoic acid 60 118 Explain why the boiling point of ethanoic acid is higher than that of propan –l-ol and yet they have same molecular mass. (2 marks) 7. 6.84g of aluminium sulphate were dissolved in 200cm3 of water. Calculate the Molar concentrations of the sulphate ions in the solution. (Relative formula mass of aluminium sulphate is 342) (3 marks) 8. Samples of urine from three participants M, K, and L at a national police recruitment exercise were spotted onto a chromatography paper alongside Dch1 raonmdaDt2o.gArachmr.omatogram was run using ethanol. The figure two illegal drugs below shows the 217

Tactics of Chemistry D1 D2 M K L Baseline a. Identify the participant who had used an illegal drug. (1 mark) b. Which drug is less soluble in ethanol. (1 mark) 9. Study the flow chart below and answer the questions that follow. Ethanol Step 1 Step 2 Ethene T U Polymerization Steps 3. Tem. of 150o Polymerization Nickel catalyst Nickel catalyst K a. Identify substances: K………………………………………………….. (½ mark) U………………………………..………………… (½ mark) L…………………………………………………. (½ mark) b. State the conditions for the reaction in step 1 to occur. (2 marks) c. Give one disadvantages of continued used of substances such as U. ( ½ mark) 10. The diagram below shows the set-up that was used to prepare and collect sulphur (IV) oxide gas. 218

Learning chemistry made easier Hydrochloric acid Solid P a. Identify solid P (1mark) b. i. Why is it possible to collect sulphur (IV) Oxide as shown? (1mark) ii. What happened to the red flower in the gas jar. 1mark) 11. The set-up show how small pieces of red phosphorous are heated in Nitrogen (I) Oxide. Gas Jar Deflagrating spoon Nitrogen (I) oxide Burning phosphorous a. Write an equation for the reactions which occur in the gas jar. (2marks) b. Give one use of Nitrogen (I) oxide. (1mark) 12. In the industrial extraction of aluminium Metal, the ore is first heated at 1600C with concentrated Sodium hydroxide. The Solid mixture obtained is then filtered and treated with carbon (IV) oxide and diluted with water. State the function of each of the following in this process. (3marks) a. Concentrated Sodium hydroxide. b. Carbon (IV) oxide c. Water. 13. a. What is meant by the term: Half-life (1mark) b. 50g of a radioactive substance was reduced to 6.25g in 36.3years. Calculate that half-life of the substance. (2marks) 219

Tactics of Chemistry 14. Part of the structure of a Polymer is given below. CH CH2 CH CH2 CH i. Identify the Polymer. (1mark) ii. State one disadvantage of continued use of this Polymer. (1mark) 15. a. State the Graham’s law. (1mark) b. In Smart Oxygen Company, it takes 20 seconds for 200cm3 of oxygen gas to diffuse across a porous wall. How long will it take an equal volume of sulphur (IV) oxide to diffuse across the same wall. (2marks) 16. Starting with copper metal, describe how a sample of crystals of copper (II) sulphate is prepared in laboratory. (3marks) 17. The Set up below shows an experiment where hydrogen gas was passed over heated copper (II) Oxide. Dry hydrogen Copper (II) oxide Heat a. State and explain the observations made in the combustion tube during the experiment. (2marks) b. Explain why heat is necessary in this experiment. (2marks) 18. In an experiment to investigate the conductivity of substances, a student used the set-up shown below. Bulb Platimum electrodes PbBr2(s) The student noted that the bulb didn’t light. a. What had been omitted in the set-up (1mark) b. Explain why the bulb lights when the Omission was corrected. (2marks) 220

Learning chemistry made easier 19. The table below gives some information about elements J,K,L,M which are in the same group of the periodic table. Use the formation to answer the question that follow. Element 1st Ionization energy kJmol-1 Atomic radius (nm) J 520 0.15 K 500 0.19 L M 420 0.23 400 0.25 (1mark) a. What is meant by ionization energy. b. State and explain the relationship between the variations in the first ionization energies and the atomic radii. (3marks) 20. Below is a structure of aluminium Chloride. AB Cl Cl Cl Al Al Cl Cl Cl a. Identify the bond labelled A and B A…………………………………………… ( ½ mark) B……………………………………………. ( ½ mark) b. When aluminium chloride is dissolved in water resulting solution has a pH of 3 Explain. (2 marks) 21. A hydrocarbon was found to contain 72% carbon, 6 % hydrogen and the rest is oxygen. If its molecular mass is 78, determine its molecular formula. (C=12, H=1) (3 marks) 22. The structure below belongs to a member of alkanoic acid. HO | || H C CO H | H a. Give the name of the structure. (1mark) b. What is the total number of electrons used for bonding in a molecule of the structured named in 22(a) (2marks) 23. a. State the observation made at the end of the experiment when the mixture 221

Tactics of Chemistry of iron powder and sulphur is heated in a test tube. (1mark) b. State one agricultural used of Sulphur. (1mark) 24. The graph below shows a curve obtained when water at 220C was heated for 10 minutes. Sodium Chloride crystals were added and strongly heated for 15 minutes. 120oC- C 100oC- B Temperature oC A 22oC | | || || 05 10 15 20 25 30 Time (min) a. What happened to water molecular between points A and B? (2 marks) b. Explain why the temperature rise is not steady between points B and C. (2 marks) 25. Use the table below to answer the questions that follow. Substance A BC DE Symbol R-COO-Na+ |CH2OH CH2 – CH2 – n |R-COOCH2 CHOH R- COOCH R-OSO3-Na+ || CH2OH R- COOCH2 a. Which substances is I. A soapless detergent. (½mark) II. An ester (½ mark) b. Give name to substance B (1mark) c. Write an equation for the reaction between the structure of substance D and sodium hydroxide solution. (2marks) 26. In an experiment to determine the solubility of sodium chloride, 5.0cm3 of a saturated solution of sodium chloride weighing 5.35g were placed in a volumetric flask and diluted sodium to a total 250cm3 of the diluted chloride volume reacted with 24.1cm3 of 0.1M silver nitrate solution. 222

Learning chemistry made easier AgNO3(aq) + NaCl (aq) AgCl (s) + NaNO3 (aq) Calculate: I. Number of moles of silver Nitrate in 24.1cm3 of solution. (1mark) II. Number of moles of sodium chloride in 250cm3 of solution. (1mark) III. Solubility of sodium chloride in g/100g of water. (2marks) 27. Both aluminium and sodium have giant metallic structure but different melting points. Explain. (2marks) PAPER 2 [80 MARKS] 1. a. The grid below show part of the periodic table. (The letter do not represent the actual symbols). Use it to answer the questions that follow. T Q S RK AJ Y UL W MB C N P i. Select the most reactive non-metal. (1mark) ii. Select an element that forms a divalent cation. (1mark) iii. Element Z has atomic number 14.Show its position in the grid. (1mark) iv. How do the atomic radii of U and J compare? (2 marks) v. How do electrical conductivity of A and Y compare?(2marks) vi. How does the boiling point of elements K, L and M vary? Explain(2marks) b. The table below gives information on four elements by letters K, L, M and N. Study it and answer the questions that follow. The letters do not represent the actual symbols of the elements. Element Electron arrangement Atomic radius Ionic radius K 0.065 L 2.8.2 0.136 0.181 M 0.133 N 2.8.7 0.099 0.099 2.8.8.1 0.203 2.8.8.2 0.174 223

Tactics of Chemistry a. Which two elements have similar properties? Explain. (2 marks) b. Which element is a non-metal? Explain. (1 mark) c. Which one of the elements is the strongest reducing agent. (1mark) 2. The list of potential differences below was obtained when metals A, B, C, D and E were used in the following electrochemical. Metal/metal ion (aq)||copper (II) ions(aq)/copper(s) Metal Eθvolts A -1.10 B -0.46 C 0.00 D +0.45 E +1.16 a. What is metal C? Explain your choice. (1mark) b. Identify two of the above metals in an electrochemical cell that would produce the largest potential difference. (1mark) c. Determine the potential difference of the cell chosen in (b) above. (2marks) d. Draw a labelled diagram of the electrochemical cell formed in (b) above (3marks) e. Which of the metal above can not be displaced by any of the other metals in the list. Explain.(2marks) f. Explain whether a sulphate solution of D can be kept in a container made of element B. (3marks) 3. a. Brine usually contains soluble calcium and magnesium salt. Explain how sodium carbonate is used to purify brine. (2marks) b. The diagram below represents a diaphragm cell used to electrolysis pure brine. Brine Steel cathode Titanum Porous diaphragm Anode i. Write the equation for the reaction that takes place at; I. Cathode (1mark) II. Anode (1mark) 224

Learning chemistry made easier ii. Name; (1mark) I. Product at U. II. Another material that can be used instead of titanium. (1mark) III. The impurity present in the product at U. (1mark) iii. State two functions of the diaphragm. (2marks) c. Give one industrial use of the product at U. (1mark) 4. a. Petrol is a mixture of several alkane molecules ranging forbotmainpeedntfarnoem(Cc5rHud12e) tooil.d eca ne (C10H22).Na(m1me tahrek)process by which petrol is b. A decane molecule derived from petrol is cracked into hydrocarbon with equal number of carbon atoms in each molecule. i. What is cracking? (1mark) ii. State two conditions necessary for the above process.(2marks) iii. Write an equation for the cracking of decane molecule. (1mark) iv. Draw and name two isomers of molecule with lower molecular mass obtained from cracking of decane as shown in b(iii) above. (2marks) v. How would you distinguish the products formed by cracking as shown in b(iii) in the laboratory. (2marks) c. Name the class to which the following cleansing agents belong. i. R-COONa+ (1mark) ii. R - O -O-SO3Na (1mark) d. Which cleaning agent above is not environmental friendly? Explain. (2marks) 5. a. State two factors which determine the stability of an isotope. (2marks) b. State two differences between chemical and nuclear reactions. (2marks) c. Study the nuclear reaction below and answer the questions that follow. U235 01n 14516Ba x Kr n1 92 y 3 0 i. Determine the value of; (1mark) X……………………………… Y……………………………… (1mark) ii. State one application of this type of reaction. (1mark) d. The activity of a radioactive isotope decreases from 512 counts per minute to 64 counts per minute in 9 minutes. What is the half-life of the radioactive isotope? (2marks) e. Give two uses of radioactive isotopes in medicine. (2marks) 6. In an experiment to determine the heat of combustion of methanol (CH3OH) a student used a set up like the one shown in the diagram below. 225

Tactics of Chemistry Thermometer Beaker Water Lamp Methanol Volume of water = 500cm3 Final temperature of water =27.00C Initial temperature of water =20.00C Final mass of lamp + methanol =22.11g Initial mass of lamp + methanol =22.98g Density of water =1.0g/cm3 a. Write a equation for the combustion of methanol. (1mark) b. Calculate; i. The number of moles of methanol used in this experiment (C=12, H=1 O=16). (2marks) ii. The heat change in this experiment. (1mark) iii. The heat of combustion per mole of methanol (2marks) c. Explain why the value of molar heat of combustion for methanol obtained in this experiment is different from the theoretical value. (1mark) d. On the axis below draw an energy level diagram for combustion of methanol. (2 marks) Energy (kJ) Reaction path 7. a. The diagram below shows the extraction of sulphur by Frasch process. 226

Learning chemistry made easier A Molten sulphur to storage B tanks Sulphur deposits i. Name the substances passed through B. (1mark) ii. State the purpose of passing substance A during the extraction of Sulphur. (1mark) iii. The sulphur obtained is mixed with water. Explain why Sulphur is easily obtained from water. (1mark) b. The equation below shows the oxidation of Sulphur (IV) oxide to Sulphur (VI) oxide in the contact process. 2SO2(g) + O2(g) 2SO3(g) ∆H = -196kJ i. Name one catalyst for this reaction. (1mark) ii. State and explain the effect on the yield of Sulphur (IV) oxide when. I. the temperature increased. (2marks) II. the amount of oxygen is increased. (2marks) iii. Describe how Sulphur (IV) oxide is converted to Sulphuric (IV) acid in the contact process. (2marks) c. State two disadvantages of having sulphur (IV) oxide in the environment. (2marks) 227

Tactics of Chemistry 1. You are provided with; PAPER 3 i. Solution G, which is 0.1M sodium hydroxide ii. Solution H, which is 0.02M potassium Manganate (VII) iii. Solution I, which is a mixture of sodium oxoalate (Na2C2O4) and oxalic acid (H2C2O4), a dibasic acid. You are required to find the percentage of sodium oxalate in the mixture. Procedure I i. Titrate 25cm3 portion of solution I with 0.1M of solution G using 2 drops of phenolphthalein. ii. Record your result as shown in the table below. Volume of pipette used=…………………….cm3 (½mark) Table I Titration I II III Final Burette reading (cm3) 4 marks Initial Burette reading (cm3) Volume of solution I used (cm3) Find the average titre. (1mark) Procedure II i. Use a pipette filler to pipette 25cm3 of solution H into a dry clean conical flask. ii. Heat the content of the conical flask to about 700C. iii. Add 20cm3 of 2M sulphuric (VI) acid and titrate against solution I to a colourless end point. iv. Record your results as shown in the table below. Titration I II III 4 marks Final Burette reading (cm3) Initial Burette reading (cm3) Volume of solution I used (cm3) Find the average titre. (1mark) You are given that an acidified solution of sodium oxalate reacts in the same way with potassium Manganate (VII) as it does with oxalic acid. Thus; 228

Learning chemistry made easier Na2C2O4(aq) 2Na+(aq) + C O 2- 2 4 (aq) and C O 2- + 2H+(aq) H2C2O4(aq) 2 4 (aq) K2SO4(aq) + 2MnSO4(aq)+ 8H2O(l) + 10CO2(g) 2KMnO4(aq)+ 5H2C2O4(aq)+ 3H2SO4(aq) You are required to: a. Write an equation for the reaction between sodium hydroxide and the substance it reacts with in the mixture of solution I. (1mark) b. Calculate the number of moles of: i. Oxalic acid used to neutralize sodium hydroxide in the first titration. (1½ marks) ii. Mass of oxalic acid in one litre of the mixture (H=1.0, C= 12.0, O=16.0) (1½ marks) c. Calculate the number of moles of; i. Oxalate ions that react with acidified potassium Manganate (VII) in the titration. (1½ marks) ii. The number of oxalate ions in sodium oxalate in the 25cm3 of the mixture. (1mark) iii. The mass of sodium Oox=a1l6a.t0e)( Na2C 2O4) in one titre of the mixture. (Na= 23.0, C =12.0, (2marks) d. Use your answer in b(ii) to calculate the percentage of; i. Oxalate acid in the mixture. (1mark) ii. Sodium oxalate in the mixture. (1mark) 2. You are provide with solid P in a test tube. You are required to determine the freezing point of solid P. Procedure i. Place 100cm3 of tap water in a 200ml- glass beaker . ii. Heat the water to near boiling. iii. Use a test-tube holder to immerse the test-tube containing Solid P into the hot water. Ensure that half of the test-tube is immersed. iv. Continue heating the water until the solid starts to melt. v. Insert a thermometer into the liquid being formed in the test-tube. Take down the temperature when all the solid melts. Record the temperature taken as show in the table below. vi. Remove the test-tube from the water and immediately start a stopwatch or the clock. vii. Record the temperature of the contents of the test-tube after every 229

Tactics of Chemistry half-minute and complete the table. viii. Dip the thermometer into the hot bath to clean it then wipe it with some tissue paper. Time (min) 0 ½ 1 1 ½ 2 2 ½ 3 3 ½ 4 4 ½ (5 marks) Temp. (0C) Required a. Plot a graph of temperature against time (3marks) b. Use the graph to; i. Determine the freezing points of solid P. (1mark) ii. Explain whether P is a pure or an impure substance. (2mks) 3. Place solid Q in a boiling tube. Add about 10cm3 of distilled water. Warm and shake the mixture until it dissolves. Divide the solution onto four portion. i. To the first portion, test with a pH paper. Inference Observation (1 mark) (1 mark) ii. To the second portion, add a little solid sodium carbonate and shake. Observation Inference (1 mark) (1 mark) iii. To the third portion, add 3 drops of acidified potassium Mangenate (VII) solution Observation Inference (1 mark) (2 mark) iv. To the fourth portion, add equal volume of ethanol followed by 3 drops of concentrated sulphuric acid and warm the mixture. Observation Inference (2 marks) (1 mark) 230

Learning chemistry made easier Confidential for question In addition to the general apparatus in a chemistry laboratory each student is required to have the following. 1. About 100cm3 of solution G 19. About 10cm3 of ethanol 2. About 100cm3 of solution H 3. About 60cm3 of solution I ACCESS TO: 4. Burette 1. Phenolphthalein 5. Pipette 2. pH chart 6. A pipette filler 3. Acidified KMnO4 supplied with a 7. A conical flask 8. A funnel dropper 9. Solid P 4. Concentrate H2SO4 supplied with a 10. Solid Q dropper 5. Source of heat 11. Thermometer 12. 100cm3 of distilled water in NOTES: a glass beaker 1. Solution G is 0.1M NaOH 13. Test-tube holder 2. SmSooillxuutttuiioorenndIHiississ2o0.l6v.08e2gdMNinaKo2MCn2neOOl4i/4tr5e.0ogfH 2C2O4 3. 14. Six test-tube solution. 15. Stop watch 4. Solid P is 1g naphthalene 16. Tissue paper 5. Solid Q is Aspirin tablets crushed to 17. Universal indicator paper powder form (about 0.5grams) 18. About 0.5grams of sodium carbonate 231

Tactics of Chemistry

Learning chemistry made easier

Tactics of Chemistry