the Ksp of Ag2CO3 is 8.1x10-12. what is the molar solubility of silver carbonate?
can you please walk me through this?
Ag2CO3 ==> 2Ag^+ + CO3^-2
Ksp = (Ag^+)^2(CO3^-2)
Set up and ICE chart, substitute into the Ksp expression, and solve. Post your work if you get stuck.
Sure! To determine the molar solubility of silver carbonate (Ag2CO3), we need to use the solubility product constant (Ksp) value. The Ksp expression for Ag2CO3 is:
Ag2CO3(s) ⇌ 2 Ag+(aq) + CO3 2-(aq)
According to the equation, 1 mole of Ag2CO3 dissociates into 2 moles of Ag+ ions and 1 mole of CO3 2- ions.
Let's assume that the molar solubility of Ag2CO3 is "s" moles per liter.
So, at equilibrium, the concentration of Ag+ ions and CO3 2- ions will both be 2s moles per liter (because of the stoichiometric coefficients in the balanced equation).
Therefore, the expression for Ksp can be written as:
Ksp = [Ag+]^2 * [CO3 2-]
Substituting the equilibrium concentrations in terms of "s", we get:
8.1x10^(-12) = (2s)^2 * s
Now, we need to solve this equation to find the value of "s". Let's go step by step:
1. Expand the equation:
8.1x10^(-12) = 4s^3
2. Rearrange the equation and isolate s:
s^3 = (8.1x10^(-12)) / 4
3. Take the cube root of both sides:
s = ∛((8.1x10^(-12)) / 4)
Now, plug in this value into a calculator to find the molar solubility of Ag2CO3.
Sure! To find the molar solubility of silver carbonate (Ag2CO3), we can use the solubility product constant (Ksp) equation. The Ksp expression for Ag2CO3 is:
Ksp = [Ag+]^2 * [CO3^2-]
Since Ag2CO3 dissociates into two Ag+ ions and one CO3^2- ion, we can substitute the molar solubility of Ag2CO3 with 's' and rewrite the Ksp expression as:
Ksp = (2s)^2 * s
8.1x10^(-12) = 4s^3
From here, we can solve for 's', which represents the molar solubility of Ag2CO3.
1. Take the cube root of both sides of the equation:
(cube root of 8.1x10^(-12)) = cube root of (4s^3)
2. Simplify the equation:
s = (cube root of 8.1x10^(-12))/2
3. Calculate the value:
s = 1.3x10^(-4) M
Therefore, the molar solubility of silver carbonate (Ag2CO3) is approximately 1.3x10^(-4) moles per liter (M).