Manganese(II) Arsenate is insoluble in water at room temperature. (Note: Arsenate = AsO4³-) In the presence of aqueous ammonia, solid Manganese(II) Arsenate becomes more soluble and aqueous tetraamminemanganese (II) ion forms. When solid Manganese(II) arsenate was placed in a 2.00 M solution of ammonia, at equilibrium, 0.308 M of ammonia remains. If the Kf of tetraamminemanganese (II) ion is 250.0, Determine the Ksp of Manganese(II) arsenate Hint: You will have to figure out the Kspf of the overall chemical equation first, then solve for Ksp by using Kf and Kspf

Manganese(II) Arsenate is insoluble in water at room temperature. (Note: Arsenate = AsO4³-) In the presence of aqueous ammonia, solid Manganese(II) Arsenate becomes more soluble and aqueous tetraamminemanganese (II) ion forms. When solid Manganese(II) arsenate was placed in a 2.00 M solution of ammonia, at equilibrium, 0.308 M of ammonia remains. If the Kf of tetraamminemanganese (II) ion is 250.0, Determine the Ksp of Manganese(II) arsenate Hint: You will have to figure out the Kspf of the overall chemical equation first, then solve for Ksp by using Kf and Kspf

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter21: Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 21.196QP

See similar textbooks

Similar questions

An aqueous solution is prepared in which 0.00113 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a total volume of 1.00 L. Kf for Ni(NH3)62+ is equal to 5.5 × 108. Calculate the concentration of Ni(H2O)62+ ions at equilibrium in the solution formed
Consider the insoluble compound iron(II) carbonate, FeCO3 . The iron(II) ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of FeCO3 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Fe(CN)64-, Kf = 7.7×10³6 . Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group 2 more group attempts remaining
Consider the insoluble compound iron(II) carbonate , FeCO3 . The iron(II) ion also forms a complex with cyanide ions . Write a balanced net ionic equation to show why the solubility of FeCO3 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction.For Fe(CN)64- , Kf = 7.7×1036 . Be sure to specify states such as (aq) or (s).
A saturated solution of Mg3(PO4)2 has a concentration of 0.939 mg per liter. Calculate the solubility product constant for Mg3(PO4)2.
Calculate the concentration of [Ag(S2O3)2]3- in a solution which contains 8.5E-6 M Ag+ ions and twice that molar concentration of thiosulfate ions at equilibrium? The Kf for [Ag(S2O3)2]3- is 4.7 x 1013. Your answer should have 2 sig figs.
Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction: I-(aq) + I2(aq) = I3-(aq) K = 710. For each of the following cases calculate the equilibrium ratio of [I3-] to [I2]. 1a) 6.00×10-2 mol of I2 is added to 1.00 L of 6.00×10-1 M KI solution. 1b)The solution above is diluted to 11.00 L. how do i do this? is an icetable required?
Consider the insoluble compound cobalt(II) carbonate, CoCO3. The cobalt(II) 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)2+, K = 7.7x104. Be sure to specify states such as (aq) or (s). K= Submit Answer Retry Entire Group 3 more group attempts remaining
The formation constant of a complex ion [M(NH3)4]2+(aq) is 8.8E8. If a solution is prepared by adding 0.4 mol of [M(NH3)4]Cl2 to 525.0 mL of water, what is the equilibrium concentration of free M2+(aq) ions? Include 3 significant figures
determine the equilibrium constant Keq if the concentration of iron(III) thiocynate is 0.322 M and the concentration of the thicyante ion is 0.013 M and the concentration of iron is 0.13 M.
What are the main equilibria involved in the CO2–Carbonate system and what kind of equilibrium constant is associated with each (K?)?
If 150 mL 0.0180 M Ni(NO3)2 and 125 mL of 0.25 M ammonia (NH3) are diluted to 500 mL with deionized water. What is the concentration of Ni(NH3)42+ in solution assumed to be at equilibrium? Kr for [Ni(NH3)4²+] is 3.7 x 1016 O 724 x 102 M O 6.9 x 10¹ M O 0.018 M O 5.4 x 10-3 M
In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCL42. Co²+ (aq) is pink and CoC14²(aq) is blue. At low temperature the pink color predominates. At high temperature the blue color is strong. If we represent the equilibrium as: CoC14²(aq) Co²+ (aq) + 4Cl¯ (aq) We can conclude that: 1. This reaction is O exothermic. O endothermic. O neutral. O More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: O increases. O decreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of CoC₁4²: O increases. O decreases. O remains the same. O More information is needed to answer this question.

SEE MORE QUESTIONS

Recommended textbooks for you

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning