Q1. Ksp = 1E-24 M^2

Q2. Ksp = 8.79E-18 M

Q3.a. 3.52E-4M = Solubility

Q3.b.If the Ksp values are close and the ionic ratios are different you must calculate the solubility to determine which is the most soluble.

Q4.1.59E-9M^2

Q5. x=1.0E-5 mol

Q6.a. 1.2E-3M

Q6.b. Solubility = 7.1E-7M – assumption 7.1E-7<< Q7. 1.43g (Limiting reagent question)

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For question number 10 0n the solubility product problems I am getting an answer of 2*10^-8 as the Q value and though the right answer is 5*10^-7. What art the intermediate steps?

Check solutions posted

I don’t respond to questions on external links

Sir, for question # 4 on page 126, I am getting ksp value of 3.481 X 10 ^-5

and this was the expression i used to calculate ksp : ksp = (0.0059) (0.0059)

Can you tell me what is the mistake i did?

Check the solution posted

Sir for question number 2 on page 125 I am getting 4.39×10^-18

the equation I used was 2(1.3×10^-6)^2 x (1.3×10^-6)

Why is my answer wrong?

Check the solution posted page 125 and 126

For question 7 where we had to find the mass that will precipitate, I’m getting the same answer w/o using Ksp or calculating the solubility.

Your solution is right as Ksp is <<<< small