What mass (in grams) of AgCl will dissolve in 250 mL of water if the Ksp = 1.7x10 − 10 ? (MM of AgCl = 143.32 g/mol)
To solve this problem, we need to use the Ksp expression and the given information.
The Ksp expression for silver chloride (AgCl) is as follows:
Ksp = [Ag+][Cl-]
Given that the Ksp value for AgCl is 1.7x10^-10, we can set up the equation as follows:
1.7x10^-10 = [Ag+][Cl-]
Since AgCl is a very insoluble compound, we can assume that it fully dissociates in water. This means that the concentration of Ag+ will be equal to the concentration of Cl-.
Let's assume that 'x' grams of AgCl will dissolve in 250 mL of water. We need to find the value of 'x'. To find the concentration of Ag+ (and Cl-), we need to convert the mass of AgCl to moles.
First, calculate the number of moles of AgCl:
moles = mass / molar mass
moles = x grams / 143.32 g/mol
The concentration of Ag+ and Cl- is given by:
concentration = moles / volume
concentration = (x grams / 143.32 g/mol) / 0.250 L
Since the concentration of Ag+ is equal to the concentration of Cl-, we can substitute these concentrations into the Ksp expression:
1.7x10^-10 = [(x grams / 143.32 g/mol) / 0.250 L]^2
Now, we can solve for 'x' by rearranging the equation and solving for 'x':
x grams = (1.7x10^-10 * (0.250 L)^2 * 143.32 g/mol)^(1/2)
By plugging in the given values and evaluating the expression, we can find the mass of AgCl that will dissolve in 250 mL of water.