The solubility of AgBr is 7.1 X 10⁻⁷ M. This dissolved AgBr produces equal moles of Ag⁺ and Br⁻, then the solubility product of this equilibrium reaction would be:
Correct answer: A. 5.041 X 10⁻¹³
- A. 5.041 X 10⁻¹³
- B. 4.941 X 10⁺¹³
- C. 7.1 X 10⁻⁷
- D. 14.082 X 10⁻¹⁴
Explanation
For AgBr, Ksp equals the concentration of Ag plus times that of Br minus, and both equal the solubility, so Ksp is the solubility squared: 7.1 x 10 to the minus 7, squared, is 50.41 x 10 to the minus 14, which is 5.041 x 10 to the minus 13. The value 14.082 x 10 to the minus 14 comes from doubling the solubility instead of squaring it.
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About Solubility Product
The solubility product constant, Ksp, represents the equilibrium concentrations of ions from a sparingly soluble salt, each raised to its stoichiometric power. Problems involve writing Ksp expressions, calculating molar solubility, applying the common-ion effect and predicting precipitation from the ionic product.
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