Predict which of the following pairs of solutions, when mixed together, will cause a precipitate to form. (Select all that apply.) Ksp values are: CoS 4.0 * 10-21 Hg2Cl2 3.5 * 10-18 PbCl2 2.4 * 10-4 Ag2SO4 1.5 * 10-5 Group of answer choices 1.5 L of 0.025 M BaCl2 and 1.25 L of 0.014 M Pb (NO3) 2 25 mL of 1 * 10-5 M Co (NO3) 2 and 75 mL of 5 * 10-4 M Na2S 500 mL of 7.5 * 10-4 M AlCl3 and 100 mL of 1.7 * 10-5 M Hg2 (NO3) 2. 650 mL of 0.0080 M K2SO4 and 175 mL of 0.15 M AgNO3

25 mL of 1 * 10-5 M Co (NO₃) ₂ and 75 mL of 5 * 10-4 M Na₂S

500 mL of 7.5 * 10-4 M AlCl₃ and 100 mL of 1.7 * 10-5 M Hg₂ (NO₃) ₂.

650 mL of 0.0080 M K₂SO₄ and 175 mL of 0.15 M AgNO₃

Explanation:

When 2 compounds that produce an insoluble substance are mixed together, A precipitate will be formed if Q of reaction > Ksp

For the solutions:

1.5 L of 0.025 M BaCl₂ and 1.25L of 0.014 M Pb (NO₃) ₂.

Ksp is:

PbCl₂ (s) ⇄ Pb²⁺ (aq) + 2Cl⁻ (aq)

Ksp = 2.4x10⁻⁴ = [Pb²⁺][Cl⁻]²

Molar concentration of each ion is:

[Pb²⁺] = 1.25L ₓ (0.014mol / L) = 0.0175mol / 2.75L = 6.36x10⁻³M

[Cl⁻] = 2 ₓ 1.5L ₓ (0.025mol / L) = 0.075mol / 2.75L = 0.0273M

Replacing in Ksp expression to find Q:

Q = [6.36x10⁻³M][0.0273M]² = 4.73x10⁻⁶

As Q < Ksp, the mixture will not produce a precipitate.

25 mL of 1 * 10-5 M Co (NO₃) ₂ and 75 mL of 5 * 10-4 M Na₂S

Ksp is:

CoS (s) ⇄ Co²⁺ (aq) + S²⁻ (aq)

Ksp = 4.0x10⁻²¹ = [Co²⁺][S²⁻]

Molar concentration of each ion is:

[Co²⁺] = 0.025L ₓ (1x10⁻⁵mol / L) = 2.5x10⁻⁷mol / 0.1L = 2.5x10⁻⁶M

[S²⁻] = 0.075L ₓ (5x10⁻⁴mol / L) = 3.75x10⁻⁵mol / 0.1L = 3.75x10⁻⁴M

Replacing in Ksp expression to find Q:

Q = [2.5x10⁻⁶M][3.75x10⁻⁴M] = 9.38x10⁻⁶

As Q > Ksp, the mixture will produce a precipitate.

500 mL of 7.5 * 10-4 M AlCl₃ and 100 mL of 1.7 * 10-5 M Hg₂ (NO₃) ₂.

Ksp is:

Hg₂Cl₂ (s) ⇄ 2Hg⁺ (aq) + 2Cl⁻ (aq)

Ksp = 3.5x10⁻¹⁸ = [Hg⁺]²[Cl⁻]²

Molar concentration of each ion is:

[Hg⁺] = 2ₓ0.100L ₓ (1.7x10⁻⁵mol / L) = 3.4x10⁻⁶mol / 0.6L = 5.67x10⁻⁶M

[Cl⁻] = 3 ₓ 0.500L ₓ (7.5x10⁻⁴mol / L) = 1.125x10⁻³mol / 0.6L = 1.88x10⁻³M

Replacing in Ksp expression to find Q:

Q = [5.67x10⁻⁶M]²[1.88x10⁻³M]² = 1.14x10⁻⁶

As Q > Ksp, the reaction will produce a precipitate.

650 mL of 0.0080 M K₂SO₄ and 175 mL of 0.15 M AgNO₃

Ksp is:

Ag₂SO₄ (s) ⇄ 2Ag⁺ (aq) + SO₄²⁻ (aq)

Ksp = 1.5x10⁻⁵ = [Ag⁺]²[SO₄²⁻]

Molar concentration of each ion is:

[Ag⁺] = 0.175L ₓ (0.15mol / L) = 0.02625mol / 0.825L = 0.0318M

[SO₄²⁻] = 0.650L ₓ (0.080mol / L) = 0.052mol / 0.825L = 0.0630M

Replacing in Ksp expression to find Q:

Q = [0.0318M]²[0.0630M] = 6.37x10⁻⁵

As Q > Ksp, the reaction will produce a precipitate.