1.0dm\(^3\) of distilled water was used to wash 2.0g of a precipitation of AgCl. If...
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1.0dm\(^3\) of distilled water was used to wash 2.0g of a precipitation of AgCl. If the solubility product of AgCl is 2.0 \(\times\) 10\(^{10}\) mol\(^2\)dm\(^6\), what quality of silver was lost in the process?
- A)2.029 \(\times\) 10\(^{-3}\) mol dm\(^{-3}\)
- B)1.414 \(\times\) 10\(^{-3}\) mol dm\(^{3}\)
- C)2.029 \(\times\) 10\(^{-5}\) mol dm\(^{3}\)
- D)1.414 \(\times\) 10\(^{-5}\) mol dm\(^{3}\)
Correct Answer: D)1.414 \(\times\) 10\(^{-5}\) mol dm\(^{3}\)
Explanation
First, let's understand the solubility product constant, Ksp. Ksp is the equilibrium constant for a solid substance dissolving in an aqueous solution. It represents the level at which a solute dissolves in solution. In this case, the solubility product of AgCl (Silver Chloride) is given as 2.0
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