In reaction with aqueous ammonia, Zn(OH)2 forms a complex ion. Explain the term complex ion, and explain how the formation of such a species can affect the solubility of a salt.

Consider the insoluble compound copper (II) carbonate, CuCO3. The copper(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of CuCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)42+, K = 6.8x1012. Be sure to specify states such as (aq) or (s). K = [Review Topics] [References] Use the References to access important values if needed for this question. Submit Answer ? + Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support Previous Email Instructor Next> Save and Exit

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 + +

1. At a certain temperature, the solubility product constant* of copper (II) iodate, Cu(IO3)2, is 7.17x10-8 M3. Calculate the solubility of this compound for this temperature.*Unless stated otherwise all solubility product constants are for water. 2. Calculate the solubility of copper (II) iodate in 0.21 M copper (II) nitrate. Ksp* is 7.4x10-8M3.*You should know that the Ksp must refer to the copper iodate because all nitrate compounds are soluble and strong electrolytes!   3. What is the initial (before any reaction takes place) lead nitrate concentration when 6.0 mL of 0.171 M lead nitrate is added to 11 mL of 0.0086 M sodium chloride?

Calculate the molar solubility of Ga(OH)3 (Kp 7.28 x 10 36) in a solution that is buffered at pH = 3.22.

Write the balanced chemical equation for each of the reactions. Include phases. When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms. equation: However, when additional aqueous hydroxide is added, the precipitate redissolves, forming a soluble [Pb(OH), 1²(aq) complex ion. equation: Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Be

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)

The solubility product, Ksp, for Fe(OH)3 is 1.6 × 10–39. What is the solubility of Fe(OH)3 in a buffer solution with pH = 10, in moles per litre?   A) 1.1 × 10–9 mol.L–1  B) 4.0 × 10–23 mol.L–1 C) 8.8 × 10–11 mol.L–1 D) 1.6 × 10–27 mol.L–1

For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K,, data in the ALEKS Data tab. compound AgCl Ca, (PO₂)₂ Ba(OH)₂ Does solubility change with pH? yes Ono Oyes O no Oyes O no pH = 5 O highest solubility pH = 6 O O X pH = 8 O ?

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 =