Question

d. calculate the volume, in liters measured at the conditions in the laboratory, that the h₂(g) produced in the reaction would have if it were dry.
e. the laboratory procedure specified that the concentration of the hcl solution be 2.0 m, but only 12.3 m hcl solution was available. describe the steps for safely preparing 50.0 ml of 2.0 m hcl(aq) using 12.3 m hcl solution and materials selected from the list below. show any necessary calculation(s).

Explanation:

Step1: Use dilution formula

The dilution formula is \(C_1V_1 = C_2V_2\), where \(C_1 = 12.3\space M\), \(C_2=2.0\space M\), and \(V_2 = 50.00\space mL\).

Step2: Solve for \(V_1\)

Rearrange the formula to \(V_1=\frac{C_2V_2}{C_1}\). Substitute the values: \(V_1=\frac{2.0\space M\times50.00\space mL}{12.3\space M}\)

$$V_1=\frac{100}{12.3}\space mL\approx 8.13\space mL$$

Step3: Describe the preparation steps

1. Use the \(10.0\space mL\) graduated cylinder to measure out approximately \(8.13\space mL\) of \(12.3\space M\space HCl\).
2. Transfer the measured \(HCl\) to the \(50.00\space mL\) volumetric flask.
3. Add distilled water to the flask, filling it up to the mark (using the dropper for the final adjustments to ensure accuracy).

Answer:

The volume of \(12.3\space M\space HCl\) needed is approximately \(8.13\space mL\). The steps are: measure \(8.13\space mL\) of \(12.3\space M\space HCl\) with \(10.0\space mL\) graduated cylinder, transfer to \(50.00\space mL\) volumetric flask, and dilute to mark with distilled water.