determine the solubility product of the slightly soluble salt calcium oxalate,cac2o4 by titrating 200cm^3 sample of a suturated solution of this salt with 0.00135mol dm^3 HCl solution.calculate Ksp?
Don't get lazy in chemistry. Find the caps key. cac2o4 isn't anything to me. Fortunately you told me what it was. You didn't give the volume.
mols = M x L. Convert to 1000 cc
Ksp = (Ca^2+)(C2O4^=)
Subtitute into Ksp expression and solve.
To calculate the solubility product (Ksp) of calcium oxalate (CaC2O4), we need to find the concentration of each ion present in the saturated solution.
Given:
Volume of the saturated solution (V) = 200 cm^3 = 0.2 dm^3
Concentration of HCl solution (C) = 0.00135 mol dm^3
First, let's calculate the moles of HCl used in the titration:
Moles of HCl = concentration (C) x volume (V)
= 0.00135 mol dm^-3 x 0.2 dm^3
= 0.00027 mol
Since HCl is a strong acid and it reacts completely, the moles of HCl used are equal to the moles of calcium oxalate that react.
Using the balanced chemical equation:
CaC2O4 (s) + 2HCl (aq) -> CaCl2 (aq) + 2H2C2O4 (aq)
We can see that 1 mole of CaC2O4 reacts with 2 moles of HCl.
So, the moles of CaC2O4 = 0.00027 mol / 2 = 0.000135 mol
Now, we can use the moles of calcium oxalate to find the solubility in terms of molarity (M):
Solubility of CaC2O4 (S) = moles (n) / volume (V)
= 0.000135 mol / 0.2 dm^3
= 0.000675 mol dm^-3
The solubility is in terms of molarity (mol dm^-3).
The solubility product constant (Ksp) is the product of the concentrations of the ions in the saturated solution raised to the power of their stoichiometric coefficients.
For the dissolution of CaC2O4:
CaC2O4 (s) -> Ca^2+ (aq) + C2O4^2- (aq)
Ksp = [Ca^2+] x [C2O4^2-]
Therefore, Ksp = (0.000675 mol dm^-3) x (0.000675 mol dm^-3) = 4.55625 x 10^-7
The solubility product (Ksp) of calcium oxalate (CaC2O4) is 4.55625 x 10^-7.
To determine the solubility product (Ksp) of calcium oxalate (CaC2O4), you can follow these steps:
Step 1: Convert the volume of the HCl solution to liters:
The given volume is 200 cm^3, which is equivalent to 200/1000 = 0.2 L.
Step 2: Calculate the number of moles of HCl:
To find the number of moles, you can use the formula:
moles = concentration × volume
moles = 0.00135 mol dm^-3 × 0.2 L
moles = 0.00027 mol
Step 3: Determine the stoichiometry of the reaction:
The balanced equation for the reaction between calcium oxalate (CaC2O4) and HCl is:
CaC2O4 + 4HCl → CaCl2 + 2CO2 + 2H2O
From the equation, we can see that 1 mole of CaC2O4 reacts with 4 moles of HCl. Therefore, the moles of CaC2O4 in the saturated solution are equal to 0.00027 mol / 4 = 0.0000675 mol.
Step 4: Calculate the concentration of CaC2O4:
The volume of the saturated solution is not given. However, we can assume that it is large enough such that the concentration of CaC2O4 is essentially constant. Therefore, we can take the concentration as the initial concentration and assume it does not change during the titration.
Step 5: Calculate the solubility product (Ksp):
The solubility product equation for calcium oxalate states that:
Ksp = [Ca2+][C2O42-]
Since calcium oxalate dissociates into one calcium ion (Ca2+) and one oxalate ion (C2O42-), the concentration of Ca2+ is equal to 0.0000675 mol/L, and the concentration of C2O42- is also equal to 0.0000675 mol/L. Thus:
Ksp = (0.0000675 mol/L) × (0.0000675 mol/L)
Ksp = 4.55625 × 10^-9
Therefore, the solubility product (Ksp) of calcium oxalate, CaC2O4, is approximately 4.55625 × 10^-9.