Question

What would the molarity of the final solution be if (1.150x10^-2) L of (2.53x10^0) M HCl is placed in a (6.0000x10^2) mL volumetric flask and diluted to the mark with distilled water?

Answer 1

81778 Chemistry, Other

What would the molarity of the final solution be if $(1.150 \times 10^{-2}) \mathrm{L}$ of $(2.53 \times 10^{0}) \mathrm{M} \mathrm{HCl}$ is placed in a $(6.0000 \times 10^{2}) \mathrm{mL}$ volumetric flask and diluted to the mark with distilled water?

Answer:

The amount of moles of the reactant must be the same in both solutions:

$$\begin{array}{l} 0.015 \cdot 2.53 = 600 \cdot X \\ 0.029 = 600 \cdot X \\ C_{M} (HCl) = X = 0.00005 \, \mathrm{M} \end{array}$$

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