A 1.000L solution is prepared in which Au+, Ag+, and Cu+ ions are present in solution as nitrates...
Question:
A 1.000L solution is prepared in which {eq}Au^+ {/eq}, {eq}Ag^+ {/eq}, and {eq}Cu^+ {/eq} ions are present in solution as nitrates all at a concentration of 0.001M a solution of sodium chloride is slowly added. Which compound will begin to precipitate first?
Ksp of AuCl = {eq}2.0 \times 10^{-13} {/eq}, AgCl = {eq}1.8 \times 10^{-10} {/eq}, CuCl = {eq}1.9 \times 10^{-7} {/eq}
Ksp Values:
In chemistry, a solution is deemed saturated when it can no longer dissolve additional solute at the prevailing temperature. At this point, the undissolved solute is in equilibrium with the dissolved solute. If we consider a sparingly soluble salt, the equilibrium between its ions and the undissolved salt is governed by the solubility product constant or Ksp. Using the Ksp value, we can assess whether a salt is very soluble or not in water such that the higher the Ksp value, the more soluble the salt is.
Answer and Explanation: 1
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View this answerThe given salts all have 1 mole of cation and 1 mole of anion per mole of salt. Hence, we can directly compare the Ksp value to determine which...
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Solubility Equilibrium: Using a Solubility Constant (Ksp) in Calculations
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Chapter 11 / Lesson 5
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Learn about solubility product constant. Understand the definition of Ksp, the Ksp formula, how to calculate Ksp, and how to find molar solubility from Ksp.
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