3) Determine the molar solubility of chromium(I) hydroxide in a buffered solution with pH = 11.45. formation of complex ion: Cr(aq) + 40H(aq) + Cr(OH)« (aq) K= 8 x 109 dissolution of chromium(II) hydroxide: Cr(OH)3(aq) + Cr (aq) + 30H(aq) Kep = 3.0 x 1029 %3D

What is the molar solubility (in mols/L)of silver chloride in 2.00 M NH3(aq) given that Ksp of AgCl = 1.77x10-10 and Kf of Ag(NH3)2* is 1.70x107? Express your answer in decimal notation rounded to three significant figures.

[PBCI,] complex K; = 2.5 x 1015 For the aqueous at 25 °C. Suppose equal volumes of 0.0030M Pb(NO,) solution and 0.38M KCl solution are mixed. Calculate the equilibrium molarity of aqueous Pb- 2+ ion. Round your answer to 2 significant digits. ?

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

What mass of AgBr will dissolve in 500.0 mL of 5.90 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the reaction Ag⁺(aq) + 2NH₃(aq) ⇌ Ag(NH₃)₂⁺(aq) K = 1.7 × 10⁷.

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 =

Given the following values of equilibrium constants: [Ag(NH,)2]* = Ag* (aq) + 2NH3(aq) K 6.3 x 10-5 Ag,SO3(s) = 2Ag* (ag) + SO?-(aq) K= 1.50 x 10-14 What is the value of the equilibrium constant for the following reaction? Ag, SO3 (s) + 4NH3 (aq) = 2[Ag(NH,)2]+ +SO (aq)

Copper(I) ions in aqueous solution react with NH₂ (aq) according to Cu+ (aq) + 2NH₂ (aq) → Cu(NH3)2(aq) Kf6.3 x 10¹0 x Calculate the solubility (in g-L) of CuBr(s) (Ksp = 6.3 × 10%) in 0.88 M NH₂ (aq). solubility of CuBr(s):

Consider the insoluble compound zinc sulfide, ZnS . The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnS (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= + +

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