Calculate the concentration of potassium chloride and silver nitrate solutions based on experimental data.

From the previous problem's Table 1, the mass of $\text{KCl}$ used was $1.86 \text{ g}$.
The relative molecular mass of $\text{KCl}$ is $74.6 \text{ g/mol}$.

Assuming the $\text{KCl}$ was dissolved in $250 \text{ cm}^3$ to prepare the standard solution (a common practice for such preparations).
Volume of $\text{KCl}$ solution = $250 \text{ cm}^3 = 0.250 \text{ dm}^3$.

Rounding to three significant figures:

2. To determine the concentration of the $\text{AgNO}_3$ solution.

The balanced chemical equation for the reaction between $\text{AgNO}_3$ and $\text{KCl}$ is:

The mole ratio of $\text{AgNO}_3$ to $\text{KCl}$ is $1:1$. So, $n_{\text{AgNO}_3} = 1$ and $n_{\text{KCl}} = 1$.

From the previous problem's context and calculations:
Concentration of $\text{KCl}$ ($M_{\text{KCl}}$) = $0.0997319 \text{ mol/dm}^3$ (unrounded value from Q1)
Volume of $\text{KCl}$ ($V_{\text{KCl}}$) = $25 \text{ cm}^3$ (pipetted into the conical flask)
Mean titre volume of $\text{AgNO}_3$ ($V_{\text{AgNO}_3}$) = $24.95 \text{ cm}^3$ (calculated in the previous step for the last question you sent).

Rearranging to solve for $M_{\text{AgNO}_3}$:

Rounding to three significant figures: