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Chapter 16: Problem 54

What is the special name given to the equilibrium constant for the dissolving of an ionic solute in water?

Short Answer

Expert verified
The special name given to the equilibrium constant for the dissolving of an ionic solute in water is called the "Solubility Product Constant (Ksp)". It is used to predict the solubility of sparingly soluble salts and determine the degree of solubility of an ionic solute in water.

Step by step solution

01

Definition of Equilibrium Constant

An equilibrium constant (K) is a dimensionless value that expresses the ratio of the concentrations of the products to the concentrations of the reactants in a chemical reaction at equilibrium. It is expressed using the equilibrium concentrations of the species involved in the equilibrium expression, raised to the power of their stoichiometric coefficients.
02

Introduction to Solubility

Solubility refers to the maximum amount of solute that can dissolve in a solvent at a given temperature and pressure. When an ionic solute dissolves in water, it dissociates into its constituent ions. The equilibrium is established between the undissolved solute and the ions in solution.
03

Equilibrium Constant for the Dissolving of an Ionic Solute in Water

For the dissolving of an ionic solute in water, the equilibrium constant is called the "solubility product constant" and is represented by Ksp. The solubility product constant is a measure of how much of the ionic solute can dissolve in water at equilibrium.
04

Special Name for Equilibrium Constant for Dissolving of an Ionic Solute in Water

The special name given to the equilibrium constant for the dissolving of an ionic solute dissolved in water is called the "Solubility Product Constant (Ksp)". It is an important concept used to predict the solubility of sparingly soluble salts and helps in determining the degree of solubility of an ionic solute in water.

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Most popular questions from this chapter

Suppose the reaction system $$\mathrm{UO}_{2}(s)+4 \mathrm{HF}(g) \rightleftharpoons \mathrm{UF}_{4}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$$ has already reached equilibrium. Predict the effect of each of the following changes on the position of the equilibrium. Tell whether the equilibrium will shift to the right, will shift to the left, or will not be affected. a. Additional \(\mathrm{UO}_{2}(s)\) is added to the system. b. 5.0 mol of \(\mathrm{Xe}(g)\) is added to the system. c. The reaction is performed in a glass reaction vessel; HF(g) attacks and reacts with glass. d. Water vapor is removed. e. The size of the reaction vessel is increased.

As you know from Chapter \(7,\) most metal carbonate salts are sparingly soluble in water. Below are listed several metal carbonates along with their solubility products, \(K_{\mathrm{sp}} .\) For each salt, write the equation showing the ionization of the salt in water, and calculate the solubility of the salt in mol/L. $$\begin{aligned}&\text { Salt } \quad K_{\mathrm{sp}}\\\&\mathrm{BaCO}_{3} \quad 5.1 \times 10^{-9}\\\&\mathrm{CdCO}_{3} \quad 5.2 \times 10^{-12}\\\&\mathrm{CaCO}_{3} \quad 2.8 \times 10^{-9}\\\&\mathrm{CoCO}_{3} \quad 1.5 \times 10^{-13}\end{aligned}$$

As you learned in Chapter \(7,\) most metal hydroxides are sparingly soluble in water. Write balanced chemical equations describing the dissolving of the following metal hydroxides in water. Write the expression for \(K_{\mathrm{sp}}\) for each process. a. \(\mathrm{Cu}(\mathrm{OH})_{2}(s)\) b. \(\operatorname{Cr}(\mathrm{OH})_{3}(s)\) c. \(\mathrm{Ba}(\mathrm{OH})_{2}(s)\) d. \(\operatorname{Sn}(O H)_{2}(s)\)

What is meant by the solubility product for a sparingly soluble salt? Choose a sparingly soluble salt and show how the salt ionizes when dissolved in water, and write the expression for its solubility product.

Explain why the position of a heterogeneous equilibrium does not depend on the amounts of pure solid or pure liquid reactants or products present.
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