It has been a while that I've reviewed solubility and I can't quite grasp the concept behind this.
433. A sample of solid lead bromide is placed in a 0.2-molar NaBr solution and allowed to reach equilibrium. What is the concentration of Pb2+ ions at equilibrium?
A. 1x10^-7M
B. 2x10^-6M
C. 5x10^-4M
D. 1x10^-3M
Answer: D
I remember that one of the ways to approach this problem is through the ICE table. Which would give me Ksp = x (0.2)^2
However, I don't understand how come the solubility of Br in equilibrium remains as what it was already present in the solution from NaBr? Shouldn't the solubility of Br be a little bigger? 😕
433. A sample of solid lead bromide is placed in a 0.2-molar NaBr solution and allowed to reach equilibrium. What is the concentration of Pb2+ ions at equilibrium?
A. 1x10^-7M
B. 2x10^-6M
C. 5x10^-4M
D. 1x10^-3M
Answer: D
I remember that one of the ways to approach this problem is through the ICE table. Which would give me Ksp = x (0.2)^2
However, I don't understand how come the solubility of Br in equilibrium remains as what it was already present in the solution from NaBr? Shouldn't the solubility of Br be a little bigger? 😕