Commercial silver-plating operations frequently use a solution containing the complex Ag(CN)2− ion. Because the formation constant (Kf) is quite large, this procedure ensures that the free Ag+ concentration in solution is low for uniform electrodeposition. In one process, a chemist added 9.0 L of 5.0 M NaCN to 90.0 L of 0.20 M AgNO3. Calculate the concentration of free Ag+ ions at equilibrium. See Table 17.5 for Kf value.
Interpretation: The concentration of free
Concept Introduction:
Reaction of coordination compounds: Complex ion undergoes ligand exchange (or substitution) reactions in solution. The rate of reaction is depends on the nature of metal ions and the ligands.
Formation constant:
No. of moles:
To Identify: The concentration of free
Answer to Problem 22.71QP
Answer
The calculated concentration of free
Explanation of Solution
Find the concentration of free
The formation constant for the above reaction:
- Concentration of cyanide ions:
The concentration of cyanide ions is calculated as shown above. The concentration of cyanide ions is used at the equilibrium formation constant.
- Concentration of silver ions:
The concentration of silver ions is calculated as shown above. The concentration of silver ion is used at the equilibrium formation constant.
- Determine the concentrations after complete reaction.
In order to calculate the concentration of silver ions, all the known values are substituted in the equilibrium formation constant. Thus, the obtained concentration of silver ions is
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Chapter 22 Solutions
EBK CHEMISTRY: ATOMS FIRST
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