We’re being asked to determine the concentration of silver ions [Ag+] when 23 g of AgCN(g) are placed in 150 mL of 0.15 M nitric acid (HNO3).
We're going to calculate the concentration of silver ions using the following steps:
Step 1: Write the balanced reaction.
Step 2: Find the equilibrium constant (K) for the net ionic equation.
Step 3: Construct an ICE chart for the reaction.
Step 4: Write the K expression and calculate for [Ag+].
Step 1: Write the balanced reaction.
Reactants:
AgCN is composed of Ag+ and CN-
HNO3 is a strong acid and will completely ionize in the solution.
HNO3 → H+ + NO3-
Reaction:
Determine the concentration of silver ions [Ag1+] in M when 23 g of AgCN(g) are placed in 150 mL of 0.15 M nitric acid (molecular mass of AgCN = 133.9 g/mol).
A. 6.0×10-17 M
B. 6.8×10-6 M
C. 1.5×10-4 M
D. 4.7×10-3 M
E. 2.9×10-3 M
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