1.0dm3 of distilled water was used to wash 2.0g of precipitate of Agcl. If the solubility product of Agcl is 2.0×10^-5. what is the quantity of silver was lost in the process?

Answer 1

To find the quantity of silver lost in the process, we need to calculate the amount of AgCl that dissolved in the water during the washing process.

First, we need to calculate the initial amount of AgCl that was present in the precipitate:
Initial amount of AgCl = 2.0g

Next, we need to calculate the amount of AgCl that dissolved in the water using the solubility product constant:
Ksp = [Ag+][Cl-] = 2.0 x 10^-5
Let x be the amount of AgCl that dissolves.
Therefore, x^2 = 2.0 x 10^-5
x = √(2.0 x 10^-5)
x ≈ 0.00447 mol

Now, we need to convert the amount of AgCl that dissolved into grams to determine the quantity of silver lost:
Mass of AgCl dissolved = 0.00447 mol x 143.32 g/mol
Mass of AgCl dissolved ≈ 0.64g

Therefore, the quantity of silver lost in the process is approximately 0.64g.