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Chapter 4: Problem 63

Describe how to prepare \(1.00 \mathrm{~L}\) of \(0.646 \mathrm{M} \mathrm{HCl}\) solution, starting with a \(2.00 \mathrm{M} \mathrm{HCl}\) solution.

Short Answer

Expert verified
To prepare a \(1.00 \mathrm{~L}\) of \(0.646 \mathrm{M} \mathrm{HCl}\) solution, one would need to take \(0.323 \mathrm{L}\) (or \(323 \mathrm{mL}\)) of the \(2.00 \mathrm{M} \mathrm{HCl}\) solution and then dilute it with water until the total volume of the solution becomes \(1.00 \mathrm{L}\).

Step by step solution

01

Identify the known values

In this case, we know the initial molarity \(M1 = 2.00 \mathrm{M}\), final molarity \(M2 = 0.646 \mathrm{M}\) and final volume \(V2 = 1.00 \mathrm{L}\). The initial volume \(V1\) for the more concentrated solution is what we need to find.
02

Apply the dilution formula

Apply the formula \(M1V1 = M2V2\) by substituting the known values into it. This would look like \(2.00 \mathrm{M} * V1 = 0.646 \mathrm{M} * 1.00 \mathrm{L}\)
03

Solve for \(V1\)

To get the volume \(V1\), you would then divide both sides of the equation by \(2.00 \mathrm{M}\). This yields: \(V1 = (0.646 \mathrm{M} * 1.00 \mathrm{L}) / 2.00 \mathrm{M}\)
04

Calculate the Volume

After performing the division, the resulting volume \(V1\) is therefore the amount of the \(2.00 \mathrm{M} \mathrm{HCl}\) solution required to make \(1.00 \mathrm{L}\) of a \(0.646 \mathrm{M} \mathrm{HCl}\) solution.

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Most popular questions from this chapter

Hydrogen halides (HF, HCl, HBr, HI) are highly reactive compounds that have many industrial and laboratory uses. (a) In the laboratory, HF and HCl can be generated by reacting \(\mathrm{CaF}_{2}\) and \(\mathrm{NaCl}\) with concentrated sulfuric acid. Write appropriate equations for the reactions. (Hint: These are not redox reactions.) (b) Why is it that HBr and HI cannot be prepared similarly, that is, by reacting \(\mathrm{NaBr}\) and \(\mathrm{NaI}\) with concentrated sulfuric acid? (Hint: \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a stronger oxidizing agent than both \(\mathrm{Br}_{2}\) and \(\mathrm{I}_{2} .\) ) (c) \(\mathrm{HBr}\) can be prepared by reacting phosphorus tribromide \(\left(\mathrm{PBr}_{3}\right)\) with water. Write an equation for this reaction.

Based on oxidation number, explain why carbon monoxide (CO) is flammable but carbon dioxide \(\left(\mathrm{CO}_{2}\right)\) is not.

Describe the basic steps involved in diluting a solution of known concentration.

You are given a water-soluble compound X. Describe how you would determine whether it is an electrolyte or a nonelectrolyte. If it is an electrolyte, how would you determine whether it is strong or weak? \(?\)

Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte: (a) \(\mathrm{H}_{2} \mathrm{O},\) (b) \(\mathrm{KCl}\) (c) \(\mathrm{HNO}_{3}\) (d) \(\mathrm{CH}_{3} \mathrm{COOH}\) (e) \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\).
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