Let's walk through the steps to determine the molarity of the HCl solution from the provided data:
1. Convert volumes from mL to L:
- Volume of the analyte (HCl):
[tex]\[
19.54 \text{ mL} = 19.54 / 1000 = 0.01954 \text{ L}
\][/tex]
- Volume of the titrant (NaOH):
[tex]\[
12.33 \text{ mL} = 12.33 / 1000 = 0.01233 \text{ L}
\][/tex]
2. Calculate the moles of NaOH used:
- Molar concentration of NaOH: [tex]\(0.5 \text{ mol/L}\)[/tex]
- Moles of NaOH:
[tex]\[
0.5 \text{ mol/L} \times 0.01233 \text{ L} = 0.006165 \text{ mol}
\][/tex]
3. Assume a 1:1 molar ratio between HCl and NaOH (as in a standard acid-base titration):
- Since the stoichiometry of the reaction is 1:1, the moles of HCl will be equal to the moles of NaOH.
- Moles of HCl = Moles of NaOH:
[tex]\[
0.006165 \text{ mol}
\][/tex]
4. Calculate the molarity of the HCl solution:
- Molarity (M) is defined as the number of moles of solute divided by the volume of solution in liters.
- Molarity of HCl:
[tex]\[
\frac{0.006165 \text{ mol}}{0.01954 \text{ L}} = 0.3155 \text{ M}
\][/tex]
Therefore, the molarity of the HCl solution is [tex]\(0.3155 \text{ M}\)[/tex].
