What is the solubility of AgCl when it is in a solution of 0.15 M NaCl? (AgCl has Ksp = 1.8 x 10-10.) Make a reaction table. Include rows for initial concentration, change in concentration, and equilibrium concentration. Write down the equation for the Ksp of the reaction. What is the concentration of Cl-? Plug that number into the Ksp equation to determine the solubility of AgCl when it is in a solution of 0.15 M NaCl .
You need to show what you don't understand about these problems. It's too late in the day for me to work all of these for you. But I'll be happy to help you through them if you explain what is giving you trouble.
To determine the solubility of AgCl when it is in a solution of 0.15 M NaCl, we need to construct a reaction table and use the Ksp equation. Here's how you can do it step by step:
1. Write the balanced equation for the dissociation of AgCl in water:
AgCl ⇌ Ag⁺ + Cl⁻
2. Construct a reaction table with three rows: initial concentration, change in concentration, and equilibrium concentration.
For AgCl:
Initial Concentration: No AgCl initially dissolved in water, so the initial concentration is 0.
Change in Concentration: +x (since x represents the amount of AgCl that dissolves)
Equilibrium Concentration: x (the solubility of AgCl)
For Ag⁺:
Initial Concentration: 0
Change in Concentration: +x
Equilibrium Concentration: x
For Cl⁻:
Initial Concentration: 0.15 M (given)
Change in Concentration: -x (since x represents the amount of Cl⁻ that combines with Ag⁺ to form AgCl)
Equilibrium Concentration: 0.15 - x
3. Write down the equation for the Ksp of the reaction:
Ksp = [Ag⁺][Cl⁻]
Since AgCl dissociates to produce one Ag⁺ and one Cl⁻ ion, the equilibrium expression becomes:
Ksp = (x)(0.15 - x)
4. Determine the concentration of Cl⁻:
Since the concentration of NaCl is given as 0.15 M, the concentration of Cl⁻ is also 0.15 M.
5. Plug the concentration of Cl⁻ into the Ksp equation to determine the solubility of AgCl:
Ksp = (x)(0.15 - x)
1.8 x 10⁻¹⁰ = (x)(0.15 - x)
Now you can solve this equation to find the value of x, which represents the solubility of AgCl in the presence of 0.15 M NaCl.