Zinc carbonate dissolves in water to the extent of 1.12 x 10-4 g/L at 25 C. Calculate the solubility product Ksp for ZnCO3 at 25 C.
A mixture of gaseous hydrogen and gaseous iodine are in equilibrium with hydrogen iodide, as shown in the following equation.
H2 (g) + I2 (g) <=> 2HI (g)
Calculate the concentration of HI when the equilibrium constant is 1 x 105, the equilibrium concentration of H2 is 0.04M, and the equilibrium concentration of I2 is 0.009M.
Marcus, you should post your own question and not go piggy back on another. I mistook your post for a new question as an answer to Indigo's question. I'll do both here.
ZnCO3(s) ==> Zn^2+(aq) + [CO3^2-](aq)
(ZnCO3) = 1.12e-4 g/L or 1.12/molar mass ZnCO3 = 1.12/125.4 = 8.93E-7M
Ksp = (Zn^2+)(CO3^2-) = (8.93E-7)(8.93E-7) = ?
My calculator is on the blink so check the numbers very closely.
For the question by Marcus Z.
H2 (g) + I2 (g) <=> 2HI (g)
K = (HI)^2/(H2)(I2) = 1E5
The problem gives you H2 and I2 and K. Plug in those value and solve for the one unknown of HI. Post your work if you get stuck.
To calculate the solubility product (Ksp) for ZnCO3 at 25°C, we need to use the given solubility and the stoichiometry of the compound.
1. Write the balanced chemical equation for the dissolution of ZnCO3 in water:
ZnCO3(s) ⇌ Zn2+(aq) + CO32-(aq)
2. Determine the concentration of the zinc ion (Zn2+) and the carbonate ion (CO32-) in the saturated solution using the solubility given:
Solubility = 1.12 x 10-4 g/L = 1.12 x 10-4 g/dm3 (since 1 L = 1 dm3)
Molar mass of ZnCO3 = 125.4 g/mol
Concentration of Zn2+ = solubility/ZnCO3 molar mass = 1.12 x 10-4 g/dm3 divided by 125.4 g/mol
Concentration of CO32- = concentration of Zn2+ (since they have a 1:1 stoichiometric ratio)
3. Substitute the concentrations of Zn2+ and CO32- into the Ksp expression:
Ksp = [Zn2+][CO32-]
4. Plug in the calculated concentrations:
Ksp = (Concentration of Zn2+)(Concentration of CO32-)
And that's how you calculate the solubility product (Ksp) for ZnCO3 at 25°C.