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Chapter 11: Problem 13

What yolume of \(0.25 M \mathrm{HCl}\) solution must be diluted to prepare \(1.00 \mathrm{~L}\) of \(0.040 \mathrm{M} \mathrm{HCl}\) ?

Short Answer

Expert verified
To prepare 1.00 L of 0.040 M HCl, 0.16 L of 0.25 M HCl solution must be diluted.

Step by step solution

01

Write the dilution formula

Write down the formula for dilution: \(C_1V_1 = C_2V_2\)
02

Substitute the given values

Plug in the given values of initial and final concentrations and the final volume of the diluted solution: \((0.25 \mathrm{M})V_1 = (0.040 \mathrm{M})(1.00 \mathrm{L})\)
03

Solve for the initial volume \(V_1\)

To find the initial volume of the HCl solution (\(V_1\)), divide both sides by the initial concentration (0.25 M): \(V_1 = \frac{(0.040 \mathrm{M})(1.00 \mathrm{L})}{(0.25 \mathrm{M})}\)
04

Calculate the result

Now, simplify and calculate the value of \(V_1\): \(V_1 = \frac{(0.040 \mathrm{M})(1.00 \mathrm{L})}{(0.25 \mathrm{M})} = 0.16 \mathrm{L}\)
05

Express the result

Finally, we express the result in a clear manner: To prepare 1.00 L of 0.040 M HCl, 0.16 L of 0.25 M HCl solution must be diluted.

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