When 25.0 mL of a 2.37E-4 M magnesium sulfate solution is combined with 25.0 mL of a 5.79E-4 M sodium carbonate solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to

When 25.0 mL of a 2.37E-4 M magnesium sulfate solution is combined with 25.0 mL of a 5.79E-4 M sodium carbonate solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 52A

See similar textbooks

Similar questions

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.
Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, and arsenates—except those of the ammonium ion and the alkali metals—are insoluble. (a) Write the expression for the equilibrium constant for the reaction represented by the equation CaCO3(s)Ca2+(aq)+CO32(aq). Is Kc1,1, or 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation 3Ba2+(aq)+2PO43(aq)Ba3( PO4)2(s). Is Kc1,1, or 1? Explain your answer.
Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give heterogeneous equilibria?
Which of the systems described in Exercise 13.15 give homogeneous equilibria? Which give heterogeneous equilibria?
5.8. The hemoglobin in blood establishes an equilibrium with oxygen gas very quickly. The equilibrium can be represented as where “heme” stands for hemoglobin and “” stands for the hemoglobin-oxygen complex. The value for the equilibrium constant for this reaction is about . Carbon monoxide also binds with hemoglobin by the following reaction: This reaction has an equilibrium constant of . Which reaction’s equilibrium lies farther toward products? Does your answer justify the toxicity of ?
. Under what circumstances can we compare the solubilities of two salts by directly comparing the values of their solubility products?
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.
For the following reactions, predict whether the pressure of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. (a) H2O(l)H2O(g) (b) N2(g)+3H2(g)2NH3(g) (c) C2H4(g)+H2O(g)C2H5OH(g)
. 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.
. 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.
Silver(I) sulfate (Ksp=1.2105) is used in the electroplating of silver. A 1.0-L solution is prepared by mixing 15 g of silver nitrate with 20 g (2 significant figures) of potassium sulfate. Will a precipitate form? At what [Ag+] concentration will precipitation (if any) start?
. Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the inter-conversion reaction?