Answer:
Ksp = 4.86 *10^-9
Explanation:
Step 1: Data given
The solubility of CuBr in water at 25°C is measured to be 0.010 g/L
Temperature = 25.0 °C
Step 2: The balanced equation
CuBr ⇔ Cu+(aq) + Br-(aq)
Step 3: Convert g/L to mol /L
0.010 g/L / / 143.45 g/mol = 6.97 * 10^-5 mol/L
Step 4: Define Ksp
Ksp = [Cu+][Br-]
There is a 1:1 ratio between CuBr and Cu+ and Br¯. T
This means, when 6.97 *10^-5 mol/L of CuBr dissolves, it produces 6.97 *10^-5 mole per liter of Cu+ and 6.97 *10^-5 mole per liter of Br¯ in solution.
Step 5: Calculate Ksp
Ksp = [Cu+][Br-]
Ksp = [6.97*10^-5 M][6.97*10^-5 M]
Ksp = 4.86 *10^-9
