Does any solid Cu(OH)2 form when 0.075 g of KOH is dissolved in 1.0 L of 1.0 ×10^-3 M Cu(NO3)2 ?

Name: Problem 86, Chapter 19: Chemistry: The Molecular Nature of Matter and Change
Uploaded: 2020-05-19T19:26:59-08:00
Duration: 3 min 35 s
Channel: Kaden Hamblin
Description: Does any solid Cu(OH)2 form when 0.075 g of KOH is dissolved in 1.0 L of 1.0 ×10^-3 M Cu(NO3)2 ?

step 1 The first thing we need to do is convert the concentration of OH minus, which is in grams. It's

Does any solid Cu(OH)2 form when 0.075 g of KOH is dissolved...

Does any solid $\mathrm{Cu}(\mathrm{OH})_{2}$ form when 0.075 $\mathrm{g}$ of KOH is dissolved in 1.0 $\mathrm{L}$ of $1.0 \times 10^{-3} \mathrm{M} \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2} ?$

Key Concepts

Precipitation Reactions

Precipitation reactions occur when two soluble ionic compounds in solution react to form one or more insoluble compounds, known as precipitates. These reactions are driven by the formation of a product that has low solubility in water, and they are often analyzed by comparing the reaction’s ionic product to the solubility product constant (Ksp) of the precipitate.

Solubility Product (Ksp)

The solubility product constant, or Ksp, is an equilibrium constant specific to the dissolution of a sparingly soluble salt in water. It quantifies the maximum product of the ion concentrations that can exist in solution before the salt begins to precipitate. By comparing the calculated ionic product to the Ksp, one can predict whether a precipitate will form under given conditions.

Molarity and Concentration Calculations

Molarity is a measure of the concentration of a solute in a solution, expressed in moles per liter. In precipitation problems, calculating the molar concentrations of the reacting ions after mixing solutions is crucial, as these concentrations determine whether the ionic product exceeds the Ksp threshold necessary for precipitation.

Reaction Stoichiometry

Reaction stoichiometry involves using the balanced chemical equation to relate the amounts of reactants and products. In the context of precipitation reactions, it is important to determine the stoichiometric ratios between the ions that combine to form the precipitate, which helps in predicting the extent of the reaction and whether sufficient ions are present to exceed the solubility product.

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