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 + +
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?
Calculate the molar solubility of Ga(OH)3 (Kp 7.28 x 10 36) in a solution that is buffered at pH = 3.22.
A student combines Fe(NO3)3 solution and KSCN solution to produce a solution in which the initial concentrations of Fe3+(aq) and SCN–(aq) are both 4 × 10–2 M. The chemical equilibrium forms FeSCN2+(aq): Fe3+ + SCN- <=> FeSCN2+ The absorbance of this solution (from FeSCN2+) is measured as 0.235, and Beer's law equation (the trend line from best fitting) as Abs = 243 x Concentration of FeSCN2+ + 0.012 Determine the equilibrium concentration for FeSCN2+ in mol/L.
The blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium. Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1) Upon addition of LiCl to this equilibrium in solution, which observation would be expected? The solution turns blue. The solution turns yellow. The Cu2+ salts precipitate out of solution. The volume of water decreases. Incorrect O O O
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
6. Consider the following equilibria: 1 Ca²+ (aq) + 2 OH- (aq) 2 ¹2 H₂O(1) H₂O*(aq) + OH-(aq) Ca(OH)₂(s) K=1.5 x 105 K = 1.0 x 10-14 Given these equilibria, what is the equilibrium constant, K, for the following reaction? 3: Ca(OH)2 (s) + 2 H3O*(aq) ≤ Ca²+ (aq) + 2 H₂O(1)
Upon analyzing a seawater sample, it was found that the concentration of bicarbonate ions (HCO3-) is 0.09 m, the activity of calcium ions (Ca2+) is 10^-6, and the pH of the seawater sample is 8.0. (a) Will calcite precipitate in this seawater sample? (b) Calculate the required activity of Mg2+ ions for dolomite to precipitate.
Write a balanced net ionic equation to show why the solubility of Mg(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Be sure to specify states such as (aq) or (s). Mg(OH)2(s) + 2HCl(aq) MgCl2(aq) + 2H2O(l) K =
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]=0.0230 M, and [AC5]=0.100 M. Determine the formation constant, Kf, of AC5. Kf = 155367729.8 The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.152 M. What is the Ksp of AB? Ksp = ?
4) Write an equilibrium reaction for the following processes: A) Sublimation of I2(s) I B) Reaction between the weak acid, HCN (aq) and the weak base, NH3(aq).