The solubility of AgCl in water is 0.001435 g per litre at 15^∘ C. The solubility product of Ag

step 1 In this problem, solubility of AGCL is equal to solubility of of AGCL by molecular weight of AGC

The solubility of AgCl in water is 0.001435 g per litre at...

The solubility of $\mathrm{AgCl}$ in water is $0.001435 \mathrm{~g}$ per litre at $15^{\circ} \mathrm{C}$. The solubility product of $\mathrm{AgCl}$ is $(\mathrm{Ag}=108, \mathrm{Cl}=35.3)$
(a) $10^{-5}$
(b) $10^{-10}$
(c) $2 \times 10^{-10}$
(d) $10^{-9}$

Key Concepts

Unit Conversion and Molar Mass Calculation

Converting solubility given in grams per liter to molarity requires the use of the molar mass of the compound. Accurate conversion is crucial for determining the concentration of ions in solution, which is then used in the solubility product expression. This process involves dividing the mass solubility by the molar mass of the compound.

Stoichiometry of Dissolution

The stoichiometry of dissolution refers to the ratio in which a compound dissociates into its constituent ions. For salts that dissociate into one cation and one anion, the concentration of each ion in a saturated solution will be equal to the molar solubility, simplifying the calculation of the solubility product.

Molar Solubility

Molar solubility is the number of moles of a solute that can dissolve per liter of solution. Converting the solubility from grams per liter to moles per liter by dividing by the molar mass allows the determination of ion concentrations in a saturated solution, which is essential for calculating the solubility product.

Solubility Product (Ksp)

The solubility product is an equilibrium constant that applies to the dissolution of a sparingly soluble salt, defined as the product of the molar concentrations of the individual ions raised to the power of their stoichiometric coefficients when the salt is in a saturated solution. It is a key concept in chemical equilibrium and helps predict whether a precipitate will form under given conditions.

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