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Chapter 4: Problem 66

You have \(505 \mathrm{~mL}\) of a \(0.125 \mathrm{M} \mathrm{HCl}\) solution and you want to dilute it to exactly \(0.100 M\). How much water should you add?

Short Answer

Expert verified
Therefore, 126 mL of water should be added to dilute the solution to exactly 0.100 M.

Step by step solution

01

Identify given values

The initial volume \(V_1\) of the HCl solution is 505 mL or 0.505 liters (since the volume in the equation should be in liters), the initial molarity \(M_1\) is 0.125 M, the final molarity \(M_2\) is 0.100 M. We need to find the final volume \(V_2\) to determine how much water is added.
02

Use the dilution formula to find \(V_2\)

Apply the formula \(M_1V_1 = M_2V_2\) to solve for \(V_2\): substituting the known values, \((0.125 M)(0.505 L) = (0.100 M)(V_2)\) which simplifies to \(V_2 = 0.631 L\)
03

Find the volume of water added

To find the volume of water added, subtract the initial volume from the final volume. The operation \(0.631 L - 0.505 L\) gives a value of 0.126 L, or 126 mL

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Most popular questions from this chapter

A \(5.00 \times 10^{2}-\mathrm{mL}\) sample of \(2.00 \mathrm{M} \mathrm{HCl}\) solution is treated with \(4.47 \mathrm{~g}\) of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains unchanged.

How does an acid-base indicator work?

Characterize the following compounds as soluble or insoluble in water: (a) \(\mathrm{CaCO}_{3}\) (b) \(\mathrm{ZnSO}_{4}\) (c) \(\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2},\) (d) \(\mathrm{HgSO}_{4}\) (e) \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\).

Describe the steps involved in preparing a solution of known molar concentration using a volumetric flask.

Explain why a solution of \(\mathrm{HCl}\) in benzene does not conduct electricity but in water it does.
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