Assuming no change in volume, calculate the minimum mass of NaCl necessary to dissolve 0.01 mole

step 1 This is problem 53 from chapter 15 and you're asking to find out how much mass of silver chlorid

Assuming no change in volume, calculate the minimum mass of...

Assuming no change in volume, calculate the minimum mass of $\mathrm{NaCl}$ necessary to dissolve $0.01$ mole of $\mathrm{AgCl}$ in $100 \mathrm{~L}$ solution. $K_{\mathrm{sp}}$ of $\mathrm{AgCl}=2.0 \times 10^{-10}$ and $K_{\mathrm{i}}$ of $\mathrm{AgCl}_{2}^{-}=2.5 \times 10^{5}$ (a) $117 \mathrm{~g}$ (b) $11.7 \mathrm{~kg}$ (c) $58.5 \mathrm{~kg}$ (d) $585 \mathrm{~g}$

Assuming no change in volume, calculate the minimum mass of $\mathrm{NaCl}$ necessary to dissolve $0.01$ mole of $\mathrm{AgCl}$ in $100 \mathrm{~L}$ solution. $K_{\mathrm{sp}}$ of $\mathrm{AgCl}=2.0 \times 10^{-10}$ and $K_{\mathrm{i}}$
of $\mathrm{AgCl}_{2}^{-}=2.5 \times 10^{5}$
(a) $117 \mathrm{~g}$
(b) $11.7 \mathrm{~kg}$
(c) $58.5 \mathrm{~kg}$
(d) $585 \mathrm{~g}$

Key Concepts

Formation Constant

The formation constant (often noted as Kf) quantifies the equilibrium between the free metal ions and the ligand with the complex ion. A high formation constant means that the complex is very stable and forms readily, which can shift the solubility equilibrium by effectively reducing the concentration of the free metal ion.

Stoichiometry in Equilibrium Calculations

Understanding the mole relationships between reactants and products is crucial in equilibrium problems. When additional reagents (like a salt providing a common ion or ligand) are introduced, stoichiometric calculations help determine how many moles of a substance are required to drive the equilibrium in a desired direction, such as dissolving an amount of precipitate.

Solubility Equilibrium

This concept deals with the balance between a solid and its dissolved ions in solution. The solubility product constant (Ksp) quantifies the maximum concentration of ions that can exist in equilibrium with the solid, and it is used to predict whether a precipitate will dissolve or form under given conditions.

Complex Ion Formation

Complex ion formation involves the binding of a metal ion with one or more ligands to form a complex. In solution, this can greatly increase the apparent solubility of an otherwise sparingly soluble salt. The stability of the complex is described by a formation constant, which indicates how strongly the metal ion binds to the ligand.

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