Calculate a value for the solubility of (NH4)2C2O4H2O in g/100 cm3
at 298 K
To calculate the solubility of (NH4)2C2O4H2O in g/100 cm3 at 298 K, we need to refer to the solubility product constant and the molar mass of (NH4)2C2O4H2O.
1. Find the solubility product constant (Ksp) for (NH4)2C2O4H2O. This value represents the equilibrium constant for the dissolution of the compound. You can usually find this value in a reference book or online database. Let's assume the Ksp for (NH4)2C2O4H2O is 1.23 x 10^-4.
2. Set up the dissolution reaction of (NH4)2C2O4H2O:
(NH4)2C2O4H2O ⇌ 2NH4+ + C2O4^2-
3. Write the expression for the solubility product constant (Ksp):
Ksp = [NH4+]^2 * [C2O4^2-]
4. Since (NH4)2C2O4H2O completely dissociates into 2 NH4+ ions and 1 C2O4^2- ion, the expression can be simplified as:
Ksp = (2x)^2 * (1x) = 4x^2
5. Assuming x represents the molar solubility of (NH4)2C2O4H2O, we can solve for x using the Ksp value:
1.23 x 10^-4 = 4x^2
6. Rearrange the equation and solve for x:
x^2 = (1.23 x 10^-4) / 4
x = √[(1.23 x 10^-4) / 4]
7. Calculate the value of x using a calculator:
x ≈ 0.00625
8. Finally, convert the molar solubility to g/100 cm3. Since the compound dissociates into two NH4+ ions, the molar mass of (NH4)2C2O4H2O is 152.13 g/mol. Therefore, the solubility is:
solubility = x * molar mass * (100/1000)
solubility = 0.00625 * 152.13 * (100/1000)
solubility ≈ 0.956 g/100 cm3
Therefore, the solubility of (NH4)2C2O4H2O at 298 K is approximately 0.956 g/100 cm3.