1. Using the appropriate K sp values, find the concentration of Cu 2 + ions in t
ID: 827668 • Letter: 1
Question
1. Using the appropriate Ksp values, find the concentration of Cu2+ ions in the solution at equilibrium after 650 mL of 0.50 M aqueous Cu(NO3)2 solution has been mixed with 300 mL of 0.40 M aqueous KOH solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19).
2. Now find the concentration of OH? ions in this solution at equilibrium. (Enter in M.)
Determine which reactions are taking place, and what will be precipitating from the Ksp values. Find the equilibrium concentrations of each species present. Remember, some ions are spectator ions.Explanation / Answer
No Ksp value is necessay to find the concentration of NO3- ions in the solution at equilibrium!
650 mL of 0.50 M Cu(NO3)2 is: 650mL x 0.50M = 0.325 mol of Cu(NO3)2.
300 mL of 0.4 M KOH is: 300mL x 0.4M = 0.12 mol of KOH.
The volume is 950ml = 0.950L after mixing the chemicals. Since NO3- ions does not precipitate out, the NO3- concentration is (note that one Cu(NO3)2 molecule contributes two NO3- ions):
[NO3-] = 2*(0.325 mol)/(0.950L) = 0.684M.
To find [OH-] is a different story. 0.325 mol of Cu(NO3)2 reacts with 0.12 mol of KOH, KOH is the limiting reactant. The Ksp of Cu(OH)2 (at 25
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