1) Write out the solubility equilibrium reactions, and Ksp expressions, for the following insoluble compounds. AgCl, CaCO3, Al2O3 Be sure to include states of matter in your reactions. 2) What does the reaction the solubility product describe? 3) Think of a way can you determine if your solution is saturated.

1) Write out the solubility equilibrium reactions, and Ksp expressions, for the following insoluble compounds. AgCl, CaCO3, Al2O3 Be sure to include states of matter in your reactions. 2) What does the reaction the solubility product describe? 3) Think of a way can you determine if your solution is saturated.

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter18: Chemical Equilibrium

Section: Chapter Questions

Problem 86E

See similar textbooks

Related questions

Q: 2.a. Write equilibrium expressions for solubility products of substances: i. Fe (OH)2 ii. Fe2S3…

A: To write the equilibrium expression for the solubility products of the below substance and also to…

Q: Calculate the pH of a saturated solution of lead hydroxide. See the Solubility Product Constant…

Q: The solubility product for Pb(Cl)2 is K = 1.60 * 10-5, the solubility product for Pb(F)2 is K = 3.70…

A: The objective is to determine the dissociation constant of H+.GivenSolubility product or ksp for…

Q: Considering the concentrations of ions at equilibrium in the simulation, what is the molar…

A: The question is based on the concept of solubility product principle. It states that when a weak…

Q: Which of the following compounds will have the highest molar solubility in pure water? O Fe(OH)3,…

Q: The Ksp of beryllium hydroxide, Be(OH)₂, is 6.92 x 10-22. Calculate the solubility of this compound…

Q: e equilibrium of saturated barium chromate solution is shown. Determine how the equilibrium will be…

A: Solution According to lupus Chatelier’s principle, adding further chemical to a system can shift the…

Q: .. A student evaluated the molar solubility of Mg(OH)2 under a variety of conditions. In each of the…

A: The common-ion effect refers to the reduction in solubility of an ionic precipitate when a soluble…

Q: Silver carbonate (Ag2CO3) has a solubility product constant (Ksp) of 8.1x 10-21. Calculate the molar…

A: Given: Solubility product (Ksp) of Ag2CO3 = 8.1x 10-21

Q: 15. The molar solubility of mercury (II) iodide in water at 0°C is 3.02 x 10¹ mol/L. What is the…

Q: Question 53 AgCl has Ksp = 1.8 x 10-10. What is its molar solubility? O 9.0 x 10-11 M O 3.6 x 10-4 M…

Q: The Solubility Product Constant for silver carbonate is 8.1 x 10-12. The molar solubility of silver…

A: Solubility Product Constant is defined as a constant for the dissolution of a solid substance into…

Q: A student measures the molar solubility of lead phosphate in a water solution to be 7.85×10-10 M.…

A: The molar solubility of lead phosphate is = 7.85×10-10 M The solubility product constant for this…

Q: The molar solubility of AgCl is 1.3 x 10-5 mol/L. Suppose that 1.863 mg of AgCl was added in 1.0 L…

A: Correct Option : c. Qsp < Ksp

Q: Write the expression for the solubility-product constant for the following ionic compound, Hg2Br2

A: The solubility product constant, denoted as Ksp, is a measure of the extent to which a solid…

Question

1) Write out the solubility equilibrium reactions, and Ksp expressions, for the
following insoluble compounds. AgCl, CaCO3, Al2O3 Be sure to include states of
matter in your reactions.
2) What does the reaction the solubility product describe?
3) Think of a way can you determine if your solution is saturated.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: Defination

VIEW

Step 2: Calculation of Ksp

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A small quantity of a soluble salt is placed in water. Equilibrium between dissolved and undissolved salt may or may not be attained. Explain.
Hard water has a high concentration of calcium and magnesium ions. Focusing on the calcium ion, a common home water -softening process is based on a reversible chemical change that can be expressed by Na2Ze(s)+Ca2+(aq)CaZe(s)+2Na+(aq). Na2Ze represents a solid resin that is like an ionic compound between sodium ions and zeolite ions, a complex arrangement of silicate and aluminate groups; CaZe is the corresponding calcium compound. When, during the day, is this system most likely to reach equilibrium? Why doesnt it reach equilibrium and stay there? Periodically it is necessary to recharge the water softner by running salt water, NaCl(aq), through it. Why is this necessary? What concept is discussed in this chapter does the recharging process illustrate? Zeolite ions are used in home water softners because they have a porous but rigid structure that is weakly attracted to cations, readily allowing an exchange among different ions.
. Under what circumstances can we compare the solubilities of two salts by directly comparing the values of their solubility products?
How is the strength of an acid related to the position of its ionization equilibrium? Write the equations for the dissociation (ionization) of HCI, HNO3, and HClO4in water. Since all these acids are strong acids, what does this indicate about the basicity of the Cl-, NO3, and ClO4ions? Are aqueous solutions of NaCl, NaNO3, or NaClO4basic?
What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.
In the chapter discussion of precipitate formation, we ran the precipitation reaction to completion and then let some of the precipitate redissolve to get back to equilibrium. To see why, redo Example 15-6, where Initial Cocentration (mol/L) Equilibrium Concentration (mol)/L [Mg2+]0 = 3.75 103 [F]0 = 6.25 102 reactstoformMgF2ymol/Mg2+ [Mg2+] = 3.75 103 y [F] = 6.25 102 2y
The equilibrium constants for dissolving silver sulfate and silver sulfide in water are 1.7 105 and 6 1030, respectively. (a) Write the balanced dissociation reaction equation and the associated equilibrium constant expression for each process. (b) Which compound is more soluble? Explain your answer. (c) Which compound is less soluble? Explain your answer.
Silver undergoes similar reactions as those shown for gold. Both metals react with cyanide ion in the presence of oxygen to form soluble complexes, and both are reduced by zinc. The reaction of Ag+ with cyanide ion may be viewed as two sequential steps: (1) Ag+(aq)+CN(aq)AgCN(s) (2) AgCN(s)+CN(aq)[Ag(CN)2](aq)Ag+(aq)+2CN(aq)[Ag(CN)2](aq)Kf=1.31021 a. Use the solubility product equilibrium constant (Appendix J) of AgCN(s) to determine the equilibrium constant for Step 1. b. Use the equilibrium constants from Step 1 and the overall reaction to determine the equilibrium constant for Step 2. c. Excess AgCN(s) is combined with 1.0 L of 0.0071 M CN (aq) and allowed to equilibrate. Calculate the equilibrium concentrations of CN and [Ag(CN)2] using the equilibrium constant for Step 2. Assume no change in volume occurs.
Draw a nanoscale (particulate) level diagram for an equilibrium mixture of
. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
The amino acid alanine has two isomers, -alanine and -alanine. When equal masses of these two compounds are dissolved in equal amounts of a solvent, the solution of -alanine freezes at the lowest temperature. Which form, -alanine or -alanine, has the larger equilibrium constant for ionization (HXH++X)?
5.4. Supersaturated solutions can be made in which more solute is dissolved in solution than would normally dissolve. These solutions are inherently unstable, however. A seed crystal of calcium acetate, , precipitates the excess solute from a supersaturated solution of calcium acetate. When the excess solute has finished precipitating, a chemical equilibrium is established. Write the chemical equations for that equilibrium, and write the net chemical reaction that occurs overall.