Math Problem Statement
The solubility product of Car 3.4×10-11 What is its solubility in 0.01 M solution of NaF
a. 3.4×10-7 mol L-1
C. 3.4×10-2 mol L-1
b. 3.4×10-5 mol L-1
d. 3.4 mol L-1
Solution
To solve this problem, we'll assume that the compound in question is , which dissociates in water as follows:
Given:
- The solubility product,
- The concentration of is 0.01 M, meaning the initial concentration of ions is 0.01 M.
Let be the solubility of in the 0.01 M solution. The concentration of ions will be and the concentration of ions will be (since each produces 2 ions).
The solubility product expression for is:
[ K_{sp} = [Ca^{2+}][F^-]^2 ]
Substituting the values:
Since is very small, the solubility will be much smaller than 0.01 M, so can be neglected compared to 0.01 M:
Thus, the correct answer is:
a.
Would you like more details or have any questions? Here are some related questions you might find interesting:
- How does the common ion effect influence the solubility of ?
- What would be the solubility of in pure water?
- How does vary with temperature?
- What happens to the solubility of if concentration increases?
- Can you explain the significance of the solubility product constant?
Tip: When dealing with solubility in the presence of a common ion, always consider simplifying assumptions to make the calculation more straightforward.
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Math Problem Analysis
Mathematical Concepts
Chemical Equilibrium
Solubility Product
Formulas
Solubility Product Expression
Theorems
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Suitable Grade Level
High School
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