Chapter 14
1. Give the formula of the conjugate acid and the conjugate base of ammonia, NH3
conjugate acid:
conjugate base:
2. A) Calculate the pH of a 0.068 M solution HCN. Ka = 6.2 X 10¯¹⁰
B) Calculate the % dissociation of the HCN solution in A).
3. Calculate the pH of a 0.49 M solution of NaC2H3O2. (HC2H3O2 Ka = 1.8x10¯⁵)
4. Calculate the concentration of a hydrofluoric acid solution, HF (aq), Ka=7.2x10¯⁴, , that would have a pH of 1.17.
5. What is the pH of a 0.25 M Fe(NO3)3 solution (Ka for Fe(OH2)+³ = 4.0 x10¯³
6. For each of the following salts in solution, label as either acidic, basic, or neutral pH.
NH4CN (NH3 Kb = 5.6x10¯¹⁰; , HCN Ka = 6.2x10¯¹⁰)

Chapter 15
1. What ratio of KOCN/ HOCN will produce a buffer with pH = 3.10? Ka for HCN = 6.2x10¯¹⁰
2. Calculate the pH for a buffer solution prepared by mixing 100. mL of 0.60 M NH3 and 200. mL of 0.45 M NH4CI. Kb for NH3 = 1.8x10¯⁵
3. How many grams of KNO2 must be added to 5.00 liters of 0.67 M HNO2 solution to produce a buffer with pH = 3.15? Assume no change in volume. Ka for HNO2 = 4.5x10¯⁴
4. If 0.10 mole of HCI is bubbled into 1.0 liter of 0.25 M NH3 solution, what will be the pH of the resulting solution?
5. Which is the best indicator for the titration of HCI solution with NaOH solution, i.e. the most nearly ideal one?
                  Acid Range Color   pH Range    Basic Range Color
                            pink               1.2-2.8             yellow
                            blue               3.4-4.6             yellow
                           yellow             6.5-7.8             purple
                         colorless          9.9-11.1                red
          none of these indicators

Consider the titration of 100.0 mL of 0.100 M HF (Ka = 7.2x10-4 with 0.100 M NaOH.
6. What is the pH of after the addition of 30.0 mL of NaOH?
7. What is the pH of after the addition of 50.0 mL of NaOH? (half way to equivalence pt)
8. What is the pH at the equivalence point of the titration?
9. What is the pH after the addition 115 mL of NaOH?

Chapter 16
1. The solubility of Ce(OH)3 is 9.93 X 10¯⁴ g/L at 25°C. Calculate the solubility product for Ce(OH)3.
2. The value of Ksp for SrSO4 is 2.8 X 10¯⁷. What is the molar solubility of SrSO4?
3. Calculate the concentration of F- ions in saturated CaF2 solution at 25°C. Ksp = 3.9 x 10¯¹¹.
4. If the pH of a saturated solution of Al(OH)3 is 6.2 at 25°C, calculate Ksp for Al(OH)3.
5. How many grams of MgF2 will dissolve in 150. mL of water at 25 °C? Ksp = 6.4 X 10¯⁹
6. Ksp for lead (II) fluoride is 3.7 X 10¯⁸. What is the molar solubility of PbF2 in 0.10 M NaF?
7. If 750.0 mL of 4.00x10¯³‪ M Ce(NO3)3 are mixed with 300.0 mL of 2.00x10¯² M KIO3, will a precipitate form? (Ksp for Ce(IO3)3 is 1.9x10¯¹⁰)
8. Calculate the concentration of Cu2+ ions in a 0.010 M [CU(NH3)4 4]²+ solution at 25°C. Kd for [Cu(NH3)4 12+ = 8.5 X 10¯¹³‪‪

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