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11 Dec 2019

RANK the salts given in the table below from least soluble to most soluble in water. (use the letters to rank them)

Salt # Name Ksp
A SrF2 8x10-10
B CaSO4 6x10-5
C Ag3PO4 2x10-18
D CoS 5x10-22
E AgBr 5x10-13
least soluble < < < < most soluble

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Related questions


Calculate delta G for the following reactions.

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 25⁰C.

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 25⁰C.

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)

Silver bromide, AgBr (s), is an essential reagent in black and white film developing. It is,

however, only sparingly soluble in water. AgBr (s) has K = 5.0 × 10-13, making it difficult to

rinse AgBr from the film negative with water.

Instead, excess AgBr is removed by an aqueous solution of sodium thiosulfate (Na2S2O3), which forms the complex ion Ag(S2O3)23-:

Ag+ (aq) + 2 S2O32- (aq) Ag(S2O3)23- (aq) Kf = 4.7 × 10+13 a) To see how this helps, first determine the molar solubility of AgBr (s) in water.

sp

b) The large formation constant of Ag(S2O3)23- (aq) means that almost all of the silver is complexed with the thiosulfate. To determine how much, calculate the [Ag+] at equilibrium in a 1.0 L solution that initially contains 0.001 M silver ions and 0.200 M sodium thiosulfate. Do so by setting up an ICE table and assuming that x is small compared to 0.200 (but not 0.001). Show that this results in a value of x = [Ag(S2O3)23-] = 0.001. In other words, all of the Ag+ complexes.

c) Your result from part b suggests that no Ag+ remains in solution. This obviously can’t be correct, since it would result in an infinitely large reaction quotient that wouldn’t be equal to an admittedly large equilibrium constant. To determine the correct [Ag+], use the equilibrium concentrations determined in part b as your initial concentrations in a new ICE table. Then use Kf to determine [Ag+]. [This approach is called a stoichiometric shift and is useful when a reaction starts with only reactants but goes almost to completion. Is essence, we are approaching the equilibrium from the direction of all Ag(S2O3)23- and no Ag+ as opposed to the direction of all Ag+ and no Ag(S2O3)23-.]

d) Before we determine the solubility of AgBr (s) in a thiosulfate solution, we need to know the appropriate equilibrium constant. To find it, determine the value of the equilibrium constant for the reaction:

AgBr (s) + 2 S2O32- (aq) <-->Ag(S2O3)23- (aq) + Br - (aq) Kc = ??

e) Finally, calculate the molar solubility of AgBr (s) in 1.0 M sodium thiosulfate. In other words, what is [Ag(S2O3)23-] for the reaction given in part d when the initial concentration of thiosulfate is 1.0 M?

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