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A student is adding a saturated solution of lead (II) sulphate (Ksp = 1.3 x 10-…

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Wize High School Grade 12 Chemistry Textbook > Acids and Bases

Solubility Product Constant, Ksp

4 Activities

A student is adding a saturated solution of lead (II) sulphate (Ksp = 1.3 x 10-8) to a reaction mixture but the label which used to have the concentration given is missing. Calculate the volume of solution the student needs to add in order to add 2.5 x 10-5 mol of Pb2+ ions.
More Solubility Product Constant, Ksp Questions:
For the following reaction, define Ksp.
SrCO3(s) <----> Sr2+(aq) + CO32-(aq)
Given the following values of Ksp for four slightly soluble sulphides at 25 °C.
SulphideKspCdS3.6×10–29CuS8.7×10–36PbS8.4×10–28MnS5.1×10–15\def\arraystretch{1.5} \begin{array}{c} \rm Sulphide &&K_{sp} \\ \hline CdS&& 3.6 \times10^{–29}\\ CuS && 8.7 \times10^{–36} \\ PbS&& 8.4 \times 10^{–28} \\ MnS&&5.1 \times10^{–15}\\ \end{array}
Which one of the following ions exists in the lowest concentration in a solution in which the sulphide ion concentration had been fixed at some (fairly large) constant value at 25°C?
Solubility Product: Ion Affects
You are trying to dissolve AgBr(s) in an aqueous solution. Which salt should you add to increase the solubility of silver bromide?
Does a precipitate of PbBr2 form if 50.0 mL of 0.0100 M Pb(NO3)2 is mixed with 50.0 mL of 0.100 M NaBr? (Ksp PbBr2 = 2.1 x 10-6)
The Ksp for CuBr is 6.3x10−9. When 1.00 mL of 0.0010 M CuNO3 is mixed with 1.00 mL of 0.0010 M NaBr, will a precipitate form? Assume that any sodium salts or nitrate salts fully dissociate in water.
Solubility
A student is preparing to test the molar solubility of PbHPO4 (s) (Ksp=3.5×10−12) in different aqueous solutions. When this salt dissociates, it produces Pb2+ (aq) and the amphiprotic ion HPO42− (aq).They prepare separate beakers with 100 mL of each of the following solutions to test:
water
0.1 M Pb(NO3)2 (aq) (which fully dissociates in water)