Chromium(VI) forms two different oxyanions, the orange dichromate ion, Cr20,2-, and the yellow chromate ion, CrO42-. (See the following photos.) The equilibrium reaction between the two ions is Cr,0,²-(aq) + H,0(1) 2CrO,(ag) + 2H*(aq) Explain why orange dichromate solutions turn yellow when sodium hydroxide is added. 250 250m PYREN 50m TRENT PYREX

Chromium(VI) forms two different oxyanions, the orange dichromate ion, Cr20,2-, and the yellow chromate ion, CrO42-. (See the following photos.) The equilibrium reaction between the two ions is Cr,0,²-(aq) + H,0(1) 2CrO,(ag) + 2H*(aq) Explain why orange dichromate solutions turn yellow when sodium hydroxide is added. 250 250m PYREN 50m TRENT PYREX

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

ess Consider the insoluble compound silver hydroxide, AgOH. The silver ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Ag(NH3)2+, Kf = 1.1×107. Be sure to specify states such as (aq) or (s). Knet + +
Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. NO, (aq) + H20 ()=HNO, (aq) + OH¯ (aq) K =
Fe (s) + 2 Ag+ (aq) ⇋ Fe2+(aq+) + 2 Ag(s) K = 0.98546 Hg2Cl2 (s) + 2 NaBr (aq) ⇋ 2 NaCl (aq) + Hg2Br2 (s) K = 996.2 Using the information above, determine the value of the equilibrium constant for this reaction. 4 NaCl (aq) + 2 Hg2Br2 (s) ⇋ 2 Hg2Cl2 (s) + 4 NaBr (aq) Report your answer on scientific notation (1.23e-4)
The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A]=0.100 M, [C]=0.0340 M, and [AC5]=0.100 M. Determine the formation constant, Kf, of AC5. The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.1580.158 M. What is the Ksp of AB?
Hydrogen, a potential fuel, is found in great abundance in water. To separate the hydrogen from the oxygen, water must be thermally decomposed. At 1000°C, the equilibrium constant for this reaction is 7.3 x 10-182H2O(g) + heat <-> 2H2(g) + O2(g) a) If the initial concentration of H2O is 0.350 M, what is the equilibrium concentration of H2? b) Suggest three stresses that could be applied to the equilibrium system to produce more hydrogen.
Consider the following equilibrium: 4Ag(s) + O2(g) ---> 2Ag2O(s). At 298 K, the equilibrium constant for this reaction is K = 8.44 X 10^3. What is the change in Gf under standard state conditions for Ag2O(s)?
Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. NH3 (aq) + H2O(1) =NH,* (aq) + OH(aq) K=-
Consider the insoluble compound cobalt(II) carbonate, COCO3 . The cobalt(I) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of COCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction For Co(NH3), Kf= 7.7×104. Be sure to specify states such as (aq) or (s). 2+ K =
Given the following reactions and their equilibrium constants,calculate the value for the overall formation constant forAg(NH3)2+. In addition, write the equilibrium expression forthe formation of Ag(NH3)2+.½Ag+(aq) + ½Cl–(aq) ⇋ ½AgCl(s) K1 = 7.45 x 104Ag(NH3)2+(aq) + Cl–⇋ AgCl(s) + 2NH3(aq) K2 = 323Ag+(aq) + 2NH3(aq) ⇋ Ag(NH3)2+(aq) Kf = ?
Calcium hydroxide will precipitate from solution by the following equilibrium: 2+ Ca²+ (aq) + 2OH(aq) + Ca(OH)₂ (s) Write the equilibrium expression for this reaction.
Here are the equilibrium constants for two reactions of nitrogen with oxygen. What is the equilibrium constant for N₂O (g) + 1/2O₂(g) → 2NO (g)? N₂(g) + O₂(g) = 2NO(g) K= 4.1 × 10^-31 N₂(g) + 1/2O₂(g) = N₂O(g) K=2.4 × 10^-18
Consider the insoluble compound zinc carbonate, ZnCO3. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)4²-, Kf = 2.9×10¹5. Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group 2 more group attempts remaining