How much 0.1 M KCl is needed to dissolve 10 gm of precipitate?

To determine the amount of 0.1 M KCl needed to dissolve 10 grams of precipitate, you'll need to calculate the number of moles of the precipitate and then use stoichiometry to find the corresponding amount of KCl.

Here's how you can do it step by step:

1. Find the molar mass of the precipitate. This will depend on the identity of the precipitate. Let's assume the molar mass of the precipitate is 100 g/mol.

2. Calculate the number of moles of the precipitate using the formula:
Moles = Mass / Molar mass
Moles = 10 g / 100 g/mol
Moles = 0.1 mol

3. Use stoichiometry to determine the amount of KCl needed. Since the molar ratio between the precipitate and KCl is 1:1 (assuming it is a 1:1 reaction), the number of moles of KCl needed will also be 0.1 mol.

4. Calculate the volume of 0.1 M KCl needed using the formula:
Volume (in liters) = Moles / Molarity
Volume = 0.1 mol / 0.1 mol/L
Volume = 1 L

Therefore, you would need 1 liter of 0.1 M KCl to dissolve 10 grams of the precipitate.