The solubility product of barium chromate is 2.4 ×10^-10, the maximum concentration of barium ni

step 1 Dear students, in problem 151 of chapter 7 ionic equilibrium we have asked that the solubility p

The solubility product of barium chromate is 2.4 ×10^-10,...

The solubility product of barium chromate is $2.4 \times$ $10^{-10}$, the maximum concentration of barium nitrate possible without precipitation in a solution of $6 \times$ $10^{-4} \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}$ is (1) $4 \times 10^{\top} \mathrm{M}$ (2) $1.2 \times 10^{10} \mathrm{M}$ (3) $6 \times 10^{4} \mathrm{M}$ (4) $3 \times 10^{4} \mathrm{M}$

The solubility product of barium chromate is $2.4 \times$ $10^{-10}$, the maximum concentration of barium nitrate possible without precipitation in a solution of $6 \times$ $10^{-4} \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}$ is
(1) $4 \times 10^{\top} \mathrm{M}$
(2) $1.2 \times 10^{10} \mathrm{M}$
(3) $6 \times 10^{4} \mathrm{M}$
(4) $3 \times 10^{4} \mathrm{M}$

Key Concepts

Common Ion Effect

The common ion effect refers to the decrease in solubility of a salt when another compound, which shares an ion in common with the salt, is present. This shift in equilibrium effectively lowers the concentration of a particular ion that is necessary to maintain saturation, thereby affecting the overall solubility of the salt involved.

Solubility Product (Ksp)

The solubility product is an equilibrium constant that applies to sparingly soluble salts. It defines the product of the concentrations of the constituent ions at equilibrium in a saturated solution, each raised to the power of its stoichiometric coefficient. This constant is used to determine whether a precipitate will form when two solutions are mixed, by comparing the ionic product to the Ksp value.

Precipitation

Precipitation occurs when the product of the ion concentrations in a solution exceeds the solubility product, resulting in the formation of a solid phase from the dissolved ions. Understanding when and how precipitation takes place is essential in controlling reaction outcomes in aqueous solutions.

Chemical Equilibrium

Chemical equilibrium is the state in which the forward and reverse reactions occur at equal rates, resulting in constant concentrations of reactants and products over time. In the context of solubility and precipitation, equilibrium concepts help determine the conditions under which no further net dissolution or precipitation occurs, as dictated by the solubility product.

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