Question

What is the molar solubility of silver carbonate (Ag2CO3) in water? The solubility product constant for Ag2CO3 is 8.1 x 10-12 at 25°C OA 1.4 x 10-6 OB 2.0 x 10-4 OC 40 x 10-6 OD.1.3 x 10-4 OE 2.7 * 10-12

Answer 1

The molar solubility of silver carbonate (Ag2CO3) in water can be calculated using the solubility product constant (Ksp). For Ag2CO3, the molar solubility is equal to twice the molar solubility of Ag⁺. Using the Ksp value of 8.1 x 10⁻¹², the molar solubility of Ag2CO3 is approximately 1.3 x 10⁻⁴ M.

Step-by-step explanation:

The molar solubility of silver carbonate (Ag2CO3) in water can be calculated using the solubility product constant (Ksp). The equation for the dissociation of Ag2CO3 in water is:

Ag2CO3 ⇌ 2Ag⁺ + CO3²⁻

From the equation, we can see that for every 1 mole of Ag2CO3 that dissolves, 2 moles of Ag⁺ and 1 mole of CO3²⁻ are produced. Therefore, the molar solubility of Ag2CO3 is equal to twice the molar solubility of Ag⁺.

Using the Ksp value of 8.1 x 10⁻¹², we can set up the expression:

Ksp = [Ag⁺]²[CO3²⁻]

Since the concentration of CO3²⁻ in the solution is equal to the concentration of Ag2CO3 (assuming 100% dissociation), we can substitute [Ag2CO3] for [CO3²⁻] in the expression:

Ksp = (2x)²(x)

8.1 x 10⁻¹² = 4x³

Solving for x gives the molar solubility of Ag2CO3 as approximately 1.3 x 10⁻⁴ M. Therefore, the correct answer is OD.1.3 x 10⁻⁴.

Answer 2

The molar solubility of Ag2CO3 in water at 25°C is calculated as 1.3 x 10^-4 M, using the solubility product constant (Ksp) of 8.1 x 10^-12.

Step-by-step explanation:

The molar solubility of silver carbonate (Ag2CO3) in water can be calculated using its solubility product constant (Ksp), which is given as 8.1 × 10-12 at 25°C. If we let x be the molarity of Ag2CO3 that dissolves to form a saturated solution, the dissolution reaction would be:

Ag2CO3 (s) → 2Ag+ (aq) + CO32- (aq)

At equilibrium, the molar concentrations of the ions will be [Ag+] = 2x and [CO32-] = x. Plugging these values into the expression for Ksp, we get:

Ksp = [Ag+]2[CO32-] = (2x)2 × x = 4x3

8.1 × 10-12 = 4x3

Solving for x gives us the molar solubility of Ag2CO3, which is the molarity of a saturated solution:

x = ∓(8.1 × 10-12 / 4) = 1.3 × 10-4 M

Therefore, option D, 1.3 x 10-4 M, is the correct molar solubility of silver carbonate in pure water at 25°C.