Acid Base Review 2021

PAP Chemistry – Acids and Bases Review Name: _________________ Per: ____ Properties and Naming 1. Insert the correct sign (<, >, or =). a) In a neutral solution: [H+1] _____ [OH-1] b) In a basic solurion: [H+1] _____ [OH-1] c) In an acidic solution: [H+1] _____ [OH-1] 2. Identify each of the following characteristics as acidic or basic: a) Turns litmus red ______________ b) Turns phenolphthalein pink ______________ c) Tastes bitter ______________ d) Reacts with metals ______________ e) Feels slippery ______________ f) Tastes sour ______________ 3. Name the following acids: ______________ a) HCl ______________ b) H2SO4 ______________ c) HNO2 ______________ d) HF 4. Write formulas for the following acids: a) nitric acid ______________ b) acetic acid ______________ c) hydrobromic acid ______________ d) sulfurous acid ______________

Bronsted-Lowry Theory Label the acids and bases in the following reactions. Connect the conjugate pairs. 5. H2O + HNO3 → H3O+ + NO3- 6. N2H4 + H2O → N2H3- + H3O+ 7. N2H4 + HCl → N2H5+ + Cl- 8. HCN + H3O+ → H2CN+ + H2O 9. OH- + NH4+ → NH3 + H2O 10. HSO4- + H2O → H2SO4 + OH- 11. Circle the acid in each of the conjugate pairs: a) CH3COO-1 ; CH3COOH b) HOCl ; OCl-1 c) NH4+ ; NH3 d) C6H5NH2 ; C6H5NH3+ e) H2PO4-1 ; HPO4-2 12. Give the formula and charge for the conjugate base of each of the following: a) HF c) HCO3-1 b) HC2H3O2 d) H2O 13. Give the formula and charge for the conjugate acid of each of the following: a) NH3 c) NO3-1 b) HSO4-1 d) H2O

pH and pOH Calculations The pH of a solution indicates how acidic or basic that solution is. It is a measure of the hydrogen ion concentration [H+]. H+] x [OH-] = 1 x 10-14 M 1. Calculate the [OH-] in solutions with the following [H+] concentration: a) [H+] = 1 x 10-4M b) [H+] = 2.5 x 10-3 M 2. Calculate the [H+] in solutions with the following [OH-] concentrations: a) [OH-] = 1 x 10-9 M b) [OH-] = 8.3 x 10-11 M pH = -log [H+] 3. Calculate the pH of solutions with the following [H+] concentrations: a) 1 x 10-2 M b) 1 x 10-11 M c) 3.7 x 10-4 M d) 9.6 x 10-7 M pH + pOH = 14 4. Calculate the pH of the following solutions: a) pOH = 8.25 b) pOH = 11.03 5. Calculate the pOH of the following solutions: a) pH = 2.98 b) pH = 9.45

Directions: Fill in the following table. (No calculator needed) [H+] pH [OH-] pOH Acid, Base or Neutral 1. 1 x 10-5 M 5 1 x 10-9 M 2. 7 1 x 10-4 M 9A 3. 4. 1 x 10-2 M 12 1 x 10-5 M 11 5. 6. 6 13 7. 8. 1 x 10-11 M 9. 10. If the base number is not 1, then you’ll need your calculator… Example Calculations: a) Determine the pH for a solution having [H+] = 2.3 x 10-5 M. Solution: pH = -log [H+] = -log (2.3 x 10-5 M) In your calculator, punch the following keys in this order: (-) (log) (2.3) (2nd) (EE) (-) (5) (=) Answer: pH = 4.64 b) Determine [H+] for a solution with pH = 4.64. Solution: [H+] = 10-pH In your calculator, punch the following keys in this order: (2nd) (log) (-) (4.64) (=) Answer: [H+] = 2.3 x 10-5 M c) Determine [OH-] for this solution. Solution: Use [H+] x [OH-] = 1 x 10-14 M to solve for [OH-] as follows [OH-] = (1 x 10-14) / [H+] = (1 x 10-14) / [2.3 x 10-5 ] = Answer: [OH-] = 4.3 x 10-10 M d) Determine pOH for this solution. 14 - 4.64 = Solution: pH + pOH = 14, so 14 - pH = pOH Answer: pOH = 9.36

Directions: Fill in the following table, round all answers to one decimal. Show work below. [H+] pH [OH-] pOH Acid, Base 4.64 4.3 x 10-10 M or Neutral? 1. 2.3 x 10-5 M 7.3 8.1 x 10-4 M 2. 9.36 A 3. 12.8 1.4 x 10-5 M 4. 5.0 x 10-2 M 11.5 5. 6.7 6. 13.2 7. 8. 7.7 x 10-11 M 9. 10.