# Problem: 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 MB. 6.8×10-6 MC. 1.5×10-4 MD. 4.7×10-3 ME. 2.9×10-3 M

###### FREE Expert Solution

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:

88% (230 ratings) ###### Problem Details

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