(a) Will Co(OH)2 precipitate from solution if the pH of a 0.020 M solution of Co(NO3)2 is adjust

step 1 We are asked to solve two problems for this section. First, we're asked to predict whether a cob

(a) Will Co(OH)2 precipitate from solution if the pH of a...

(a) Will $\mathrm{Co}(\mathrm{OH})_{2}$ precipitate from solution if the $\mathrm{pH}$ of a $0.020 \mathrm{M}$ solution of $\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}$ is adjusted to $8.5 ?$ (b) Will $\mathrm{AgIO}_{3}$ precipitate when $20 \mathrm{~mL}$ of $0.010 \mathrm{M} \mathrm{AgNO}_{3}$ is mixed with $10 \mathrm{~mL}$ of $0.015 \mathrm{M} \mathrm{NaIO}_{3} ?\left(K_{s p}\right.$ of $\mathrm{AgIO}_{3}$ is $\left.3.1 \times 10^{-8} .\right)$

(a) Will $\mathrm{Co}(\mathrm{OH})_{2}$ precipitate from solution if the $\mathrm{pH}$ of a $0.020 \mathrm{M}$ solution of $\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}$ is adjusted to $8.5 ?$
(b) Will $\mathrm{AgIO}_{3}$ precipitate when $20 \mathrm{~mL}$ of $0.010 \mathrm{M} \mathrm{AgNO}_{3}$ is mixed with $10 \mathrm{~mL}$ of $0.015 \mathrm{M} \mathrm{NaIO}_{3} ?\left(K_{s p}\right.$ of $\mathrm{AgIO}_{3}$ is $\left.3.1 \times 10^{-8} .\right)$

Key Concepts

Solubility Product Constant (Ksp)

The solubility product constant is an equilibrium constant that applies to the dissolution of a sparingly soluble compound. It expresses the maximum product of the ion concentrations that can exist in solution before a precipitate forms. Comparing the ion product to the Ksp allows us to predict whether precipitation will occur in a given chemical system.

Ion Product vs. Ksp

The ion product is calculated by multiplying the concentrations of the ions produced by a dissolved compound. By comparing this product to the corresponding Ksp value, it is possible to determine if the solution is supersaturated. If the ion product exceeds the Ksp, the solution is supersaturated and precipitation will occur; if it is less, no precipitate forms.

Precipitation Reactions

Precipitation reactions occur when two soluble compounds react in solution to form an insoluble product, leading to the formation of a solid precipitate. These reactions are driven by the interaction of ions that combine to exceed the solubility limits defined by their Ksp values.

Effect of pH on Solubility

The pH of a solution can significantly affect the solubility of compounds, especially those involving hydroxide ions. Changes in pH can alter the concentration of hydroxide ions, which in turn can shift the equilibrium for the formation or dissolution of metal hydroxide precipitates. This concept is vital in understanding the conditions under which precipitation or dissolution occurs.

Dilution and Mixing Calculations

When solutions are combined, the resulting concentrations of the ions change due to dilution. Accurate determination of the final ion concentrations requires accounting for the total volume of the mixed solutions. This is essential in evaluating whether the new ion concentrations will lead to conditions that surpass the solubility product threshold, resulting in precipitation.

Transcript

Please give Ace some feedback