Lesson test: Solubility and precipitation

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Solubility and precipitation

1.[2p]
Silver chloride has $K_{s p} = 1.77 \times 10^{- 10}$ . What is its molar solubility in pure water, in mol dm⁻³?

CorrectNot quite: 1.33e-5

2.[3p]
Calcium fluoride has $K_{s p} = 3.9 \times 10^{- 11}$ and dissolves as $Ca \to C + 2$ . What is its molar solubility, in mol dm⁻³?

CorrectNot quite: 2.14e-4

3.[3p]
What is the solubility of silver chloride, in mol dm⁻³, in $0.010$ mol dm⁻³ sodium chloride?

CorrectNot quite: 1.77e-8

4.[3p]
Silver chromate has a solubility product a hundred and sixty times smaller than silver chloride's, yet is nearly five times more soluble. Why?

The two salts have different stoichiometries, so solubility relates to $K_{s p}$ by a different power

Correct

One of the published constants must be wrong

The answer is: The two salts have different stoichiometries, so solubility relates to $K_{sp}$ by a different power

Chromate ions are larger than chloride ions

The answer is: The two salts have different stoichiometries, so solubility relates to $K_{sp}$ by a different power

Silver chromate is coloured

The answer is: The two salts have different stoichiometries, so solubility relates to $K_{sp}$ by a different power

5.[2p]
Calcium carbonate dissolves in dilute acid while silver chloride does not, because carbonate is a base and chloride is not.

True

Correct

False

The answer is: True

6.[2p]
A solution has an ion product $Q$ smaller than $K_{s p}$ . What happens?

Any solid present dissolves

Correct

More solid precipitates

The answer is: Any solid present dissolves

Nothing can be said without knowing the temperature

The answer is: Any solid present dissolves

The solution is supersaturated

The answer is: Any solid present dissolves

7.[3p]
Equal volumes of $0.0020$ mol dm⁻³ silver nitrate and $0.0020$ mol dm⁻³ sodium chloride are mixed. What is the ion product $Q$ immediately after mixing?

CorrectNot quite: 1.0e-6

8.[3p]
Which of these increase the solubility of a sparingly soluble salt?

Select all that apply

Adding a ligand that forms a complex with the cation

Correct

Adding acid, when the anion is the conjugate base of a weak acid

Correct

Adding an inert salt, which lowers the activity coefficients

Correct

Adding a salt with an ion in common

The answer is: Adding a ligand that forms a complex with the cation, Adding acid, when the anion is the conjugate base of a weak acid, Adding an inert salt, which lowers the activity coefficients

9.[3p]
Match each observation to its cause.

Limestone caves
Ammonia clearing a silver chloride precipitate
Scale in a kettle
A precipitate washed in dilute reagent

a salt that dissolves exothermically
the common ion effect
carbonate dissolved by weakly acidic rain
complex ion formation

Show the answer

Limestone caves: carbonate dissolved by weakly acidic rain Ammonia clearing a silver chloride precipitate: complex ion formation Scale in a kettle: a salt that dissolves exothermically A precipitate washed in dilute reagent: the common ion effect

1.[2p] Silver chloride has Ksp=1.77×10-10. What is its molar solubility in pure water, in mol dm⁻³?

2.[3p] Calcium fluoride has Ksp=3.9×10-11 and dissolves as Ca→C+2. What is its molar solubility, in mol dm⁻³?

3.[3p] What is the solubility of silver chloride, in mol dm⁻³, in 0.010 mol dm⁻³ sodium chloride?

4.[3p] Silver chromate has a solubility product a hundred and sixty times smaller than silver chloride's, yet is nearly five times more soluble. Why?

5.[2p] Calcium carbonate dissolves in dilute acid while silver chloride does not, because carbonate is a base and chloride is not.

6.[2p] A solution has an ion product Q smaller than Ksp. What happens?

7.[3p] Equal volumes of 0.0020 mol dm⁻³ silver nitrate and 0.0020 mol dm⁻³ sodium chloride are mixed. What is the ion product Q immediately after mixing?

8.[3p] Which of these increase the solubility of a sparingly soluble salt?

9.[3p] Match each observation to its cause.

1.[2p]
Silver chloride has $K_{s p} = 1.77 \times 10^{- 10}$ . What is its molar solubility in pure water, in mol dm⁻³?

2.[3p]
Calcium fluoride has $K_{s p} = 3.9 \times 10^{- 11}$ and dissolves as $Ca \to C + 2$ . What is its molar solubility, in mol dm⁻³?

3.[3p]
What is the solubility of silver chloride, in mol dm⁻³, in $0.010$ mol dm⁻³ sodium chloride?

4.[3p]
Silver chromate has a solubility product a hundred and sixty times smaller than silver chloride's, yet is nearly five times more soluble. Why?

5.[2p]
Calcium carbonate dissolves in dilute acid while silver chloride does not, because carbonate is a base and chloride is not.

6.[2p]
A solution has an ion product $Q$ smaller than $K_{s p}$ . What happens?

7.[3p]
Equal volumes of $0.0020$ mol dm⁻³ silver nitrate and $0.0020$ mol dm⁻³ sodium chloride are mixed. What is the ion product $Q$ immediately after mixing?

8.[3p]
Which of these increase the solubility of a sparingly soluble salt?

9.[3p]
Match each observation to its cause.