Questions: How many milliliters of a 0.352 MM NaOH solution are needed to react with 0.0250 L of 0.275 MM HCl? NaOH(aq) + HCl(aq) -> NaCl(aq) + H2O(l) 19.5 mL 2.42 mL 32.0 mL 0.0195 L

Solution Steps

The balanced chemical equation for the reaction between NaOH and HCl is: \[ \mathrm{NaOH}(\mathrm{aq}) + \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{NaCl}(\mathrm{aq}) + \mathrm{H}_2\mathrm{O}(\mathrm{l}) \]

First, we need to calculate the moles of HCl present in the solution. The volume of HCl solution is 0.0250 L and its molarity is 0.275 M. \[ \text{Moles of HCl} = \text{Molarity} \times \text{Volume} = 0.275 \, \text{M} \times 0.0250 \, \text{L} = 0.006875 \, \text{moles} \]

From the balanced equation, we see that the reaction between NaOH and HCl is in a 1:1 molar ratio. Therefore, the moles of NaOH needed to react with 0.006875 moles of HCl is also 0.006875 moles.

We know the molarity of the NaOH solution is 0.352 M. We can use the formula: \[ \text{Volume} = \frac{\text{Moles}}{\text{Molarity}} = \frac{0.006875 \, \text{moles}}{0.352 \, \text{M}} = 0.01953 \, \text{L} \] Converting this volume to milliliters: \[ 0.01953 \, \text{L} \times 1000 \, \text{mL/L} = 19.53 \, \text{mL} \]

Final Answer