Chromium(VI) forms two different oxyanions, the orange dichromate ion, Cr2O72− , and the yellow chromate ion, CrO42− .
(See the following photos.) The equilibrium reaction between the two ions is
Explain why orange dichromate solutions turn yellow when sodium hydroxide is added.
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Chemistry: An Atoms First Approach
- Write the equilibrium constant expression for each of the following reactions in terms of concentrations. (a) CO2(g) + C(s) 2 CO(g) (b) [Cu(NH3)4)2+(aq) Cu2+(aq) + 4 NH3(aq) (c) CH3CO2H(aq) + H2O() CH3CO2(aq) + H3O+(aq)arrow_forwardBecause calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?arrow_forwardThe creation of shells by mollusk species is a fascinating process. By utilizing the Ca2+ in their food and aqueous environment, as well as some complex equilibrium processes, a hard calcium carbonate shell can be produced. One important equilibrium reaction in this complex process is HCO3(aq)H+(aq)+CO32(aq)K=5.61011 If 0.16 mole of HCO3 is placed into 1.00 L of solution, what will be the equilibrium concentration of CO32?arrow_forward
- The value of the equilibrium constant, K, is dependent on which of the following? (There may be more than one answer.) a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.arrow_forwardWhat 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.arrow_forwardA Boric acid and glycerin form a complex B(OH)3(aq) + glycerin(aq) B(OH)3 glycerin(aq) with an equilibrium constant of 0.90. If the concentration of boric acid is 0.10 M, how much glycerin should be added, per liter, so that 60.% of the boric acid is in the form of the complex?arrow_forward
- Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forwardConsider the reaction 2N2O(g) + O2(g) 4NO(g) Suppose the system is at equilibrium, and then an additional mole of N2O(g) is injected into the system at constant temperature. Once the reaction reestablishes equilibrium, has the amount of N2O increased or decreased from its original equilibrium amount? Explain. What happens to the value of the equilibrium constant with this change?arrow_forward
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