Consider the insoluble compound nickel(II) carbonate , NiCO3 . The nickel ion also forms a complex with cyanide ions . Write a balanced net ionic equation to show why the solubility of NiCO3 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ni(CN)42- , Kf = 1.0×1031 . Be sure to specify states such as (aq) or (s).   +       +   K =

For the aqueous [HgI4]complex Ky = 6.76 × 1029 at 25 °C. Suppose equal volumes of 0.0062 M Hg (NO3)2 solution and 0.42M Nal solution are mixed. Calculate the equilibrium molarity of aqueous Hg** ion. Round your answer to 2 significant digits. ☐ M

10) Ce³+ exhibits pH dependent solubility. If Ce(NO3)3 is dissolved in an acidic solution to a concentration of 0.025 M, at what pH has 95% of the cerium been removed as the insoluble hydroxide salt? Ce(OH)3 pKsp=21.2

In 0.15m Cu2 (03 (aq) Solution, Write the chemical equation of the reaction With the ksp expression: KSp= [Fe²] ³- [Pou] ²

Please use the values in the resources listed below instead of the textbook values. Sometimes equilibria for complex ions are described in terms of dissociation constants, Ka. For the complex ion Cu(CN)4 3- the dissociation reaction is as follows. [Cu*]• [CN 14 Kd [Cu(CN)43-] Cu(CN)4 3- = Cu+ + 4 CN- = 5.0X10° n-31 = Calculate the value of the formation constant, Kf, for Cu(CN)4°¯. 4.0

Consider the insoluble compound nickel (II) hydroxide, Ni(OH)2. The nickel ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Ni(OH)2 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ni(CN)4²-, Kf = 1.0×10³¹ . Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group No more group attempts remain

For the aqueous [Ag (NH3)₂ complex K₁=1.12 × 107 at 25 °C. + Suppose equal volumes of 0.0042M AgNO3 solution and 0.86M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ag ion. Round your answer to 2 significant digits. M x10 Times 10 to an exponent

Write a balanced net ionic equation to show why the solubility of Cu(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).   +       +   K =

The chemical reaction for the formation of the red-orange iron(III) thiocyanate complex ion is Fe3+ (aq) +  SCN- (aq)  <==> [FeSCN2+] (aq)   What is the source of the Fe3+ ions?   What is the source of the SCN- ions?   The equilibrium constant for this reaction is given by what