If adding 22.7 mL of 0.6 M HCl to 1.00 L of a solution of AgNO₃ precipitated 1.95 g of AgCl, what was the concentration of the original AgNO₃ solution?
AgNO₃(aq) + HCl(aq) $\rightarrow$ AgCl(s) + HNO₃(aq)

Question

If adding 22.7 mL of 0.6 M HCl to 1.00 L of a solution of AgNO₃ precipitated 1.95 g of AgCl, what was the concentration of the original AgNO₃ solution?
AgNO₃(aq) + HCl(aq)

\rightarrow

AgCl(s) + HNO₃(aq)

Quizplus · Accepted Answer

First, calculate the moles of AgCl formed using its molar mass (143.32 g/mol): $ \frac{1.95 \, \text{g}}{143.32 \, \text{g/mol}} = 0.0136 \, \text{mol} $. Since the reaction between Ag+ and Cl- produces AgCl in a 1:1 ratio, the moles of Ag+ originally present in the 1.00 L solution must also be 0.0136 mol. Therefore, the concentration of Ag+ (and thus AgNOS) in the original solution is $ \frac{0.0136 \, \text{mol}}{1.00 \, \text{L}} = 1.36 \times 10^{-2} \, \text{M} $.

If Adding 22 →\rightarrow→ AgCl(s) + HNO3(aq) A) 1

If Adding 22 $\rightarrow$ AgCl(s) + HNO₃(aq)
A) 1