Solubility Product Constant: Ksp Practice Problems

At 25°C, 0.787 g of iron (II) fluoride is contained in a 1.00 L saturated FeF₂ solution. Determine the solubility-product constant of this compound at this temperature.

At 25°C, a total mass of 0.052 grams of barium selenate (BaSeO₄) is dissolved in a 1.00 L saturated BaSeO₄ solution. What is the solubility-product constant (K_sp) of BaSeO₄ at this temperature?

A mass of 0.736 g of the compound CsIO₄ dissolves in one liter of solution. Calculate the K_sp of CsIO₄.

Determine the solubility of BiI₃ (K_sp = 7.71×10^–19)  in pure water. Report your answer in grams per liter. 

Cesium nitrate (CsNO₃) has a solubility of 0.259 g/mL. Determine the value of K_sp for CsNO₃.

Cinnabar (HgS) is a brick-red colored sulfide of mercury. It has been traditionally used to prepare vermilion, a coloring pigment. A cinnabar-coated statue rests in the Narayan Mandir of Karachi's old city Narainpura. Suppose that the statue has 500 mg of cinnabar on it and is exposed to acidic rain and other atmospheric phenomena. The statue is washed in acid rain and the water has a pH of 4.50. How many years will it take for all of the cinnabar to get removed from the statue? On average, it rains 40 days a year in Karachi. Assume that 500 L of water passes over the statue in a single rain and the water gets saturated with HgS. Does the calculated number look reasonable, given that it doesn't rain much in Karachi? What other factors, in addition to acidic rain, might contribute to the loss of the pigment from the statue?

A 0.150 M HCl solution was used to titrate a 0.0120 mol sample of Ni(OH)₂(s) (K_sp = 5.5×10^–16) in 150.0 mL of water. Calculate the volume (in milliliters) of the HCl solution required to neutralize Ni(OH)₂ completely.

Ba(CH₃COO)₂ has a solubility of 600 g/L. Determine the value of K_sp for Ba(CH₃COO)₂.

Provide the balanced net ionic equation and the Ksp expression when solid Hg₂CO₃ dissolves in water to form a solution.

The correct K_sp expression for Cd₃(AsO₄)₂ is:

The solubility of rubidium chloride, RbCl, is 5.79 M. Calculate the value of K_sp for RbCl.

Provide the solubility product constant expression for ammonium perchlorate (NH₄ClO₄). What is the K_sp value if [NH₄⁺] in the solution is 1.85 M?

If the value of K_sp for Ca₃(PO₄)₂ is 1.0×10⁻²⁵, what is its solubility in g/L?

If the value of K_sp for PbI₂ is 9.8×10⁻⁹, what is its molar solubility?

At 25 ºC. A solution of MgCO₃ exerts an osmotic pressure of 97.12 mmHg. Given complete dissociation of MgCO₃, calculate the Ksp of MgCO₃.

Carbonate minerals are minerals that contain carbonate (CO₃^2–) as one of their major components. Two examples of these carbonate minerals are malachite (Cu₂(OH)₂CO₃) with K_sp = 6.9×10^–34 and azurite (Cu₃(CO₃)₂(OH)₂) with K_sp = 1.3×10^–45. Provide the expression for the solubility product constant for malachite and azurite.

At 27 °C, a saturated solution of magnesium carbonate has an osmotic pressure of 98 torr. Calculate its solubility product constant at this temperature 

If the solubility of SrCrO₄ is dependent on pH, what is the equilibrium constant for the following reaction based on the K_b expression of the CrO₄^2– ion?  (K_a HCrO₄^– = 3.0×10^–8)
SrCrO₄(s) + H₂O(l) ⇌ Sr²⁺ (aq) + HCrO₄^– (aq) + OH^–(aq)

Copper ions can be used to disinfect swimming pools. It is advised to use a concentration of roughly 0.2 ppm. To maintain this concentration, a slightly soluble salt can be added to the pool. What is the concentration of Cu⁺ in parts per million that is in equilibrium with CuCl (K_sp = 1.7×10^–7)?

True or False. For a given compound, the "solubility-product constant" and "solubility" are equal. 

Provide the solubility-product constant expression for Cr₂(CO₃)₃.

Nickel ions have an EPA acceptable level of 0.1 ppm in water. Will a saturated nickel(II) carbonate solution (K_sp = 1.42×10^–7) produce a nickel ion solution that exceeds the EPA limit?

What is the required minimum pH to completely precipitate Cd(OH)₂ (K_sp = 2.5×10^–14) such that the remaining concentration of Cd²⁺ (aq) is less than 1.0 µg/L, or 1.0 ppb?

If the K_sp of Ni(OH)₂ is 5.48×10^–16, what is the pH needed to precipitate Ni(OH)₂ when 3.5 lb of Ni(NO₃)₂ is dissolved in 5000 gallons of water?

Based on K_sp values, which has a greater molar solubility between MgF₂ (K_sp = 5.16×10^–11) and PbI₂ (K_sp = 9.8×10^–9)?

Identify the compound that has the smallest K_sp value from the following general ionic compounds and their molar solubilities in pure water.

The molar solubility of CaF₂ in pure water is 3.32×10^–4. Calculate K_sp.

Calcium oxalate (CaC₂O₄) crystals can be formed in the kidneys and are the most common type of kidney stones. They are formed when there are high concentrations of calcium and oxalate and too little liquid in the kidney. The normal level of calcium in the blood is 8.6 to 10.3 mg/dL. If the calcium concentration in the blood is 9.0 mg/dL and the K_sp of calcium oxalate is 2.7×10^–9, what is the minimum concentration of oxalate that will cause the formation of calcium oxalate crystals?

Write the balanced equation and the K_sp expression when K₂SO₄ dissolves in water.

Write the balanced equation and the K_sp expression when NiCl₂ dissolves in water.

Write the balanced equation and the K_sp expression when MgCrO₄ dissolves in water.

Which compound, M₂X or MX₃, would have the lower molar solubility? The K_sp for both is 8.1×10^–6.

Determine the molar solubility of silver iodide (AgI) in pure water (K_sp = 8.51×10^–17)

What mass (in grams) of calcium sulfate (CaSO₄, MW = 136.14 g/mol) can be dissolved in 3.35 L of water? K_sp for CaSO₄ is 9.10×10^–6.

Consider the following solubility equilibrium for copper(II) arsenate:

Cu₃(AsO₄)_2(s) ⇌ 3 Cu²⁺_(aq) + 2 AsO₄^3–_(aq)

Write a solubility product expression for this sparingly soluble salt.

Calculate the pH at which a solution of Nickel(II) hydroxide (Ni(OH)₂) should be buffered so that the concentration of Ni²⁺ ions in the solution is 1.15×10^–5 M. (K_sp of Ni(OH)₂ = 2.00×10^–15)

A saturated solution of Iron(III) hydroxide (Fe(OH)₃, MW = 106.87 g/mol) contains 5.89×10^–10 M OH^– ions. Calculate the K_sp of Iron(III) hydroxide in water.

Barium chromate (BaCrO₄, MW = 253.32 g/mol) has a solubility of 2.78×10^–3 g/L water. Calculate the solubility product (K_sp) of barium chromate.

Magnesium arsenate, Mg₃(AsO₄)₂, dissociates reversibility in its aqueous solutions:

Mg₃(AsO₄)_2(s) ⇌ 3 Mg²⁺_(aq) + 2 AsO₄^3–_(aq)

The solubility of magnesium arsenate in water at room temperature is very low. Based on this information, which of the following statements are true?

Consider the following sparingly soluble salt equilibrium:

Fe(OH)_2(s) ⇌ Fe²⁺_(aq) + 2 OH^–_(aq); K_sp = 8.00×10^–16 at 25 °C.

What is the solubility of Fe(OH)₂ (in g/100 mL units) in water at this temperature? Report your answer in three significant figures.

Lead(II) chloride, PbCl₂, is a sparingly soluble salt with a solubility product (K_sp) of 1.60×10^–5 at 25 °C. Calculate the molarity of a saturated solution of PbCl₂ at 25 °C.

The solubility product (K_sp) of scandium(III) fluoride is 4.20×10^–18 at 25 °C. Calculate the concentration of Sc³⁺ ions when [F^–] = 1.25×10^–5 M.

Determine the solubility of LiF (s) at 60.00 °C if its ΔH° of solution and solubility at 25.00 °C is 2.18 kJ/mol and 0.0616 mol/L, respectively.