Show all your steps for calculation questions in order to get full points.
1. (4 pts) The solubility product (Ksp) of the insoluble salt AgBr is 5.0 x 10-13. Calculate the equilibrium constant for the following reaction: Ag+(aq) + Br-(aq) AgBr(s).
2. (6 pts) A solution is prepared by adding 50.0 mL of 0.050 M HCl to 150.0 mL of 0.10 M HNO3.
a. Calculate the pH of the solution.
b. Calculate the concentrations of all species in this solution.
3. (4 pts) Calculate the volume of concentrated (12 M) HCl needed to prepare 1-L of a pH = 1.50 solution?
4. (5 pts) Arrange the following 0.10 M solutions in order of most acidic to most basic.
KOH, KCl, KCN, NH4Cl, HCl
5. (6 pts) Calculate the pH of an aqueous solution containing 1.0 x 10-2 M HCl and 1.0 x 10-2 M HCN.
6. (5pts) Carbonate buffers are important in regulating the pH of blood at 7.40. What is the concentration ratio of CO2 (usually written H2CO3) to HCO3- in blood at pH=7.40?
H2CO3(aq) HCO3-(aq) + H+(aq) Ka = 4.3 x 10-7
7. (10 pts) HCN gas, a powerful respiratory inhibitor, is highly toxic. It is a very weak acid (Ka = 6.2 x 10-10) when dissolved in water. If a 50.00-mL sample of 0.100 M HCN is titrated with 0.100 M NaOH, calculate the pH of the solution:
a. before the titration starts.
b. after 8.00 mL of 0.100 M NaOH has been added.
c. at the half-way point of the titration.
d. at the equivalence point of the titration.
Show all your steps for calculation questions in order to get full points.
1. (4 pts) The solubility product (Ksp) of the insoluble salt AgBr is 5.0 x 10-13. Calculate the equilibrium constant for the following reaction: Ag+(aq) + Br-(aq) AgBr(s).
2. (6 pts) A solution is prepared by adding 50.0 mL of 0.050 M HCl to 150.0 mL of 0.10 M HNO3.
a. Calculate the pH of the solution.
b. Calculate the concentrations of all species in this solution.
3. (4 pts) Calculate the volume of concentrated (12 M) HCl needed to prepare 1-L of a pH = 1.50 solution?
4. (5 pts) Arrange the following 0.10 M solutions in order of most acidic to most basic.
KOH, KCl, KCN, NH4Cl, HCl
5. (6 pts) Calculate the pH of an aqueous solution containing 1.0 x 10-2 M HCl and 1.0 x 10-2 M HCN.
6. (5pts) Carbonate buffers are important in regulating the pH of blood at 7.40. What is the concentration ratio of CO2 (usually written H2CO3) to HCO3- in blood at pH=7.40?
H2CO3(aq) HCO3-(aq) + H+(aq) Ka = 4.3 x 10-7
7. (10 pts) HCN gas, a powerful respiratory inhibitor, is highly toxic. It is a very weak acid (Ka = 6.2 x 10-10) when dissolved in water. If a 50.00-mL sample of 0.100 M HCN is titrated with 0.100 M NaOH, calculate the pH of the solution:
a. before the titration starts.
b. after 8.00 mL of 0.100 M NaOH has been added.
c. at the half-way point of the titration.
d. at the equivalence point of the titration.
e. after 52.00 mL of 0.100 M NaOH has been added.
8. (5 pts) Calculate the Ksp value. For bismuth sulfide (Bi2S3), which has a solubility of 1.0 x 10-15 mol/L at 25â°C.
9. (5 pts) Arrange the following group of salts: in order of most soluble to most insoluble.
AgI (Ksp= 1.5 x 10-16), CuI (Ksp= 5.0 x 10-16) and CaSO4 (Ksp= 6.1x 10-5)
e. after 52.00 mL of 0.100 M NaOH has been added.
8. (5 pts) Calculate the Ksp value. For bismuth sulfide (Bi2S3), which has a solubility of 1.0 x 10-15 mol/L at 25â°C.
9. (5 pts) Arrange the following group of salts: in order of most soluble to most insoluble.
AgI (Ksp= 1.5 x 10-16), CuI (Ksp= 5.0 x 10-16) and CaSO4 (Ksp= 6.1x 10-5)
