# Solubility and Ksp (Worksheet)

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Work in groups on these problems. You should try to answer the questions without referring to your textbook. If you get stuck, try asking another group for help.

## Q1

Use the chemical $$AgCl$$ to describe solubility, molar solubility and solubility product

### Q2

Write balanced equations and solubility product expressions for the following compounds

1. $$CuBr$$
2. $$ZnC_2O_4$$
3. $$Ag_2CrO_4$$
4. $$Hg_2Cl_2$$
5. $$AuCl_3$$
6. $$Mn_3(PO_4)_3$$

### Q3.

Silver Chloride has a larger $$K_{sp}$$ than silver carbonate ($$K_{sp} = 1.6 \times 10^{‐10}$$ and $$8.1 \times 10^{‐12}$$ respectively). Does this mean that $$AgCl$$ also has a larger molar solubility than $$Ag_2CO_3$$? Explain.

### Q4

Calculate the concentration of ions in the following saturated solutions

1. $$[I^‐]$$ in $$AgI$$ solutions with $$[Ag^+ ] = 9.1 \times 10^{‐9}$$
2. $$[Al^{3+}]$$ in $$Al(OH)_3$$ solution with $$[OH^‐ ] = 2.9 \times 10^{‐9}$$

### Q5

From the solubility data given, calculate the solubility product for the following compounds:

1. $$SrF_2$$ $$7.3 \times 10^{‐2} g/L$$
2. $$Ag_3PO_4$$ $$6.7 \times 10^{‐3} g/L$$

### Q6

The molar solubility of $$MnCO_3$$ is $$4.2 \times 10^{‐6}\, M$$. What is $$K_{sp}$$ for this compound?

### Q7

If 20.0 mL of 0.10 M $$Ba(NO_3)_2$$ are added to 50.0 mL of 0.10 M $$Na_2CO_3$$, will $$BaCO_3$$ precipitate? Supply explanation and calculations to support answer.

### Q8

A volume of 75 mL of 0.060 M $$NaF$$ is mixed with 25 mL of 0.15 M $$Sr(NO_3)_2$$. Calculate the concentrations in the final solution of $$NO_3^‐$$, $$Na^+$$, $$Sr^{2+}$$, and $$F^‐$$. ($$K_{sp}$$ for $$SrF_2 = 20. \times 10^{‐10}$$)

### Q9

Calculate the $$K_{sp}$$ for each of the salts whose solubility is listed below.

1. $$CaSO_4$$ at $$5.0 \times 10^{‐3} mol/L$$
2. $$MgF_2$$ at $$2.7 \times 10^{‐3} mol/L$$
3. $$AgC_2H_3O_2$$ at $$1.02 \,g/100 \,mL$$
4. $$SrF_2$$ at $$12.2 \,mg/100 \,mL$$

### Q10

Calculate the solubility in moles/L of each of three salts and the concentration of the cations in mg/mL in each of the saturated solutions.

1. $$AgCN$$ with $$K_{sp} = 2.0 \times 10^{‐12}$$
2. $$BaSO_4$$ with $$K_{sp} = 1.5 \times 10^{‐9}$$
3. $$FeS$$ with $$K_{sp} = 3.7 \times 10^{‐19}$$
4. $$Mg(OH)_2$$ with $$K_{sp} = 9.0 \times 10^{‐12}$$
5. $$Ag_2S$$ with $$K_{sp} = 1.6 \times 10^{‐49}$$
6. $$CaF_2$$ with $$K_{sp} = 4.9 \times 10^{‐11}$$

### Q11

Consider these slightly soluble salts:

• $$PbS$$ with $$K_{sp} = 8.4 \times 10^{‐28}$$
• $$PbSO_4$$ with $$K_{sp} = 1.8 \times 10^{‐8}$$
• $$Pb(IO_3)_2$$ with $$K_{sp} = 2.6 \times 10^{‐13}$$
1. Which is the most soluble?
2. Calculate the solubility in moles/L for $$PbSO_4$$.
3. How many grams of $$PbSO_4$$ dissolve in 1 L of solution?
4. How can you decrease the concentration of $$Pb^{2+}(aq)$$ in a saturated solution of $$PbSO_4$$ solution?
5. What is the concentration in moles/L of $$PbS$$ in a saturated solution of the salt?

### Q12

For each of these substances, calculate the milligrams of metallic ion that can remain at equilibrium in a solution having a $$[OH^‐] = 1.0 \times 10^{‐4}\, mol/L$$.

1. $$Cu(OH)_2$$ with $$K_{sp} = 1.6 \times 106{‐9}$$
2. $$Fe(OH)_3$$ with $$K_{sp} = 6.0 \times 10^{‐38}$$
3. $$Mg(OH)_2$$ with $$K_{sp} = 6.0 \times 10^{‐12}$$