Activity 4 Another example of going from KSP to Solubility. Then, another application of LeChatelier’s Principle: The Common Ion Effect: BaSO4 is a very toxic ion, yet BaSO4 is used for gastrointestinal x-rays because it is opaque to x-rays. The drink given is actually a suspension, with solid BaSO4 suspended in the solution, so the solution is saturated. KSP for this compound is 1.10 x 10-10. (a) What is the concentration of Ba2+ in a saturated solution of BaSO4? (b) Given the toxicity of Ba2+ ions, why do you think magnesium sulfate is added to the drink? Hint: What would the presence of more sulfate ions do to the amount of dissolved Ba2+ in the solution? Think Le Chatelier’s Principle! Note: sulfate ions are called “common ions” here. (c) Suppose you start with the saturated solution of BaSO4 from part (a) of this problem. Now, figure out what the solubility of BaSO4 becomes if enough MgSO4 is added to the solution to make it 0.10 M in MgSO4. Start by writing the equilibrium. Let S equal the concentration of Ba2+. The difference here is that the SO42- has an initial concentration of 0.10 M. Set up the problem as in any ICE problem. Recall that KSP is 1.10 x 10-10.
Activity 4 Another example of going from KSP to Solubility. Then, another application of LeChatelier’s Principle: The Common Ion Effect:
BaSO4 is a very toxic ion, yet BaSO4 is used for gastrointestinal x-rays because it is opaque to x-rays. The drink given is actually a suspension, with solid BaSO4 suspended in the solution, so the solution is saturated. KSP for this compound is 1.10 x 10-10.
(a) What is the concentration of Ba2+ in a saturated solution of BaSO4?
(b) Given the toxicity of Ba2+ ions, why do you think magnesium sulfate is added to the drink?
Hint: What would the presence of more sulfate ions do to the amount of dissolved Ba2+ in the solution? Think Le Chatelier’s Principle! Note: sulfate ions are called “common ions” here.
(c) Suppose you start with the saturated solution of BaSO4 from part (a) of this problem. Now, figure out what the solubility of BaSO4 becomes if enough MgSO4 is added to the solution to make it 0.10 M in MgSO4. Start by writing the equilibrium. Let S equal the concentration of Ba2+. The difference here is that the SO42- has an initial concentration of 0.10 M. Set up the problem as in any ICE problem. Recall that KSP is 1.10 x 10-10.
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