Question

1. The Solubility Product Constant for iron(III) sulfide is 1.4×10^-88.

If iron(III) sulfide is dissolved in water you can say that the equilibrium concentrations of iron(III) and sulfide ions are: ...
...A. High
...B. Moderate
...C. Low

The solubility of iron(III) sulfide in water is: ...
...A. High
...B. Moderate
...C. Low

2. The Solubility Product Constant for nickel(II) carbonate is 6.6×10^-9.

If nickel(II) carbonate is dissolved in water you can say that the equilibrium concentrations of nickel and carbonate ions are: ...
...A. High
...B. Moderate
...C. Low

The solubility of nickel(II) carbonate in water is: ...
...A. High
...B. Moderate
...C. Low

3.

For each of the salts on the left, match the salts on the right that can be compared directly, using K_sp values, to estimate solubilities.

(If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g, ABC.)

	1.	silver sulfite		A. FeCO3
	2.	silver bromide		B. CaSO4
				C. Ag2CO3
				D. Ba3(PO4)2

Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water.

silver sulfite			silver bromide
Ksp =			Ksp =

4.

or each of the salts on the left, match the salts on the right that can be compared directly, using K_sp values, to estimate solubilities.

(If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g, ABC.)

	1.	cobalt(II) sulfide		A. PbS
	2.	nickel(II) hydroxide		B. Co(OH)2
				C. Ni(CN)2
				D. Cr(OH)3

Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water.

cobalt(II) sulfide			nickel(II) hydroxide
Ksp =			Ksp =

Note: Multiply out any number and put it first in the K_sp expression. Combine all exponents for s.

Note: Multiply out any number and put it first in the K_sp expression. Combine all exponents for s.

Answer 1