Concept explainers
Write balanced equations and solubility product expressions for the solubility equilibria of the following compounds:
Interpretation:
Thebalanced equation and the solubility product constant of the given compounds are to be calculated.
Concept introduction:
The amount of solute dissolved in a given volume of the solvent to form a saturated solution at a given temperatureis termed as the solubility of the solute in the solvent at that temperature.
The solubility product of a sparingly-soluble salt is given as the product of the concentration of the ions raised to the power equal to the number of times the ion occurs in the equation, after the dissociation of the electrolyte.
The number of moles of the solute dissolved per litre of the solution is called molar solubility.
For a general reaction:
The solubility product can be calculated by the expression as:
Here,
Answer to Problem 45QP
Solution:
Balanced equation:
Solubility product:
Balanced equation:
Solubility product:
Balanced equation:
Solubility product:
Balanced equation:
Solubility product:
Balanced equation:
Solubility product:
Balanced equation:
Solubility product:
Explanation of Solution
a)
The balanced equation for the dissociation of
Let
The initial change equilibrium table for the ionisation of
The equilibrium expression for the reaction is written as follows:
Here,
Substitute the values of
Hence, the solubility product constant of
b)
The balanced equation for the dissociation of
Let
The initial change equilibrium table for the ionisation of
The equilibrium expression for the reaction is written as follows:
Here,
Substitute the values of
Hence, the solubility product constant of
c)
The balanced equation for the dissociation of
Let
The initial change equilibrium table for theionization of
The equilibrium expression for the reaction is written as follows:
Here,
Substitute the values of
Hence, the solubility product constant of
d)
The balanced equation for the dissociation of
Let
The initial change equilibrium table for the ionisation of
The equilibrium expression for the reaction is written as follows:
Here,
Substitute the values of
Hence, the solubility product constant of
e)
The balanced equation for the dissociation of
The ICE table for the ionisation for
Let
The equilibrium expression for the reaction is written as follows:
Here,
Substitute the values of
Hence, the solubility product constant of
f)
The balanced equation for the dissociation of
Let
The initial change equilibrium table for the ionisation of
The equilibrium expression for the reaction is written as follows:
Here,
Substitute the values of
Hence, the solubility product constant of
Want to see more full solutions like this?
Chapter 17 Solutions
Chemistry - With Access (Looseleaf) (Custom)
- What is the molar solubility of BaSO₄?arrow_forwardDuring the preparation of saturated Ca(OH)2 solution, a student inadvertently transferred a small grain of solid Ca(OH)2 into the 125 mL Erlenmeyer flask with the solution and conducted the titration with HCl. How will the resulting calculations for molar solubility and solubility product compare to the true values?arrow_forwardThe solubility product constant of Cu(OH)2 and Mg(OH)2 are 1.6 × 10-9 and 6.0 × 10-12, respectively. In terms of calculating molar solubility, which of these hydroxides is less soluble?arrow_forward
- determine the molar solubility of Mg(OH)2arrow_forwardThe solubility of CuI is 2 x 10 ̄6 molar. Whatis the solubility product constant, K sp, for CuI?arrow_forwardA 27.6 mL sample of 0.275 M methylamine, CH3NH2, is titrated with 0.275 M hydroiodic acid.After adding 10.8 mL of hydroiodic acid, the pH isarrow_forward
- Calculate the molar solubility of Ag₂CrO₄.arrow_forwardThe Ksp of mercury(II) hydroxide, Hg(OH)2, is 3.60×10^−26. Calculate the molar solubility, s, of this compound.arrow_forwardThe hydroxide ion has the formula OH−. The solubility-product constants for three generic hydroxides are given here. Generic hydroxide KspKspK_sp XOH 1.20×10^−8 Y(OH)2 3.10×10^−10 Z(OH)3 5.70×10^−15 At a pH of 10.5, arrange the solutions containing the following generic hydroxides in order of decreasing concentration of the cation remaining in the solution (i.e., in order of increasing completeness of precipitation).arrow_forward
- You have two different concentrations of a buffer solution, 2.0 M and 0.20 M, to which 0.01 mol HCl has been added. Which of these solutions has the higher buffer capacity? In other words, which would be able to resist pH via the addition of acid longer?arrow_forwardA 100.0 mL solution of 0.125 mol/L Hydrobromic Acid, HBr, is being titrated with 0.375 mol/L Potassium Hydroxide KOH. What is the pH of the solution after 50.0 mL of KOH has been added?arrow_forwardCalculate the molar solubility of Mg(OH)2 in 1.00 M NH4Cl (aq).arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning