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Chapter 4: Problem 77

Pure acetic acid, known as glacial acetic acid, is a liquid with a density of \(1.049 \mathrm{~g} / \mathrm{mL}\) at \(25^{\circ} \mathrm{C}\). Calculate the molarity of a solution of acetic acid made by dissolving \(20.00 \mathrm{~mL}\) of glacial acetic acid at \(25^{\circ} \mathrm{C}\) in enough water to make \(250.0 \mathrm{~mL}\) of solution.

Short Answer

Expert verified
The molarity of the acetic acid solution is 1.396 M.

Step by step solution

01

Calculate the mass of acetic acid using its density and volume

To calculate the mass of acetic acid in the given volume, we use the formula: mass = density 脳 volume The volume of glacial acetic acid is 20.00 mL, and its density is 1.049 g/mL. Plugging in the values, we get: mass = 1.049 g/mL 脳 20.00 mL mass = 20.98 g So, the mass of acetic acid dissolved is 20.98 g.
02

Convert the mass of acetic acid to moles using its molar mass

To find the moles of acetic acid, we will use the molar mass of acetic acid: molar mass of acetic acid = 60.05 g/mol Now, we can find the moles by dividing the mass of acetic acid by its molar mass: moles of acetic acid = mass / molar mass moles of acetic acid = 20.98 g / 60.05 g/mol moles of acetic acid = 0.349 mol We have 0.349 moles of acetic acid.
03

Calculate the molarity using the moles of acetic acid and the final volume of the solution

Finally, we can calculate the molarity of the solution using the moles of acetic acid and the final volume of the solution: Molarity (M) = moles of solute / volume of solution (in liters) The final volume of the solution is 250.0 mL, which we need to convert to liters: 250.0 mL = 250.0 / 1000 L = 0.250 L Now, we can calculate the molarity of the solution: Molarity = 0.349 mol / 0.250 L Molarity = 1.396 mol/L Therefore, the molarity of the acetic acid solution is 1.396 M.

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Most popular questions from this chapter

When methanol, \(\mathrm{CH}_{3} \mathrm{OH},\) is dissolved in water, a nonconducting solution results. When acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH},\) dissolves in water, the solution is weakly conducting and acidic in nature. Describe what happens upon dissolution in the two cases, and account for the different results.

(a) Is the concentration of a solution an intensive or an extensive property? (b) What is the difference between \(0.50 \mathrm{~mol}\) \(\mathrm{HCl}\) and \(0.50 \mathrm{M} \mathrm{HCl} ?\)

Suppose you have \(5.00 \mathrm{~g}\) of powdered magnesium metal, \(1.00 \mathrm{~L}\) of \(2.00 \mathrm{M}\) potassium nitrate solution, and \(1.00 \mathrm{~L}\) of \(2.00 \mathrm{M}\) silver nitrate solution. (a) Which one of the solutions will react with the magnesium powder? (b) What is the net ionic equation that describes this reaction? (c) What volume of solution is needed to completely react with the magnesium? (d) What is the molarity of the \(\mathrm{Mg}^{2+}\) ions in the resulting solution?

Acetone, \(\mathrm{CH}_{3} \mathrm{COCH}_{3},\) is a nonelectrolyte; hypochlorous acid, \(\mathrm{HClO},\) is a weak electrolyte; and ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl},\) is a strong electrolyte. (a) What are the solute particles present in aqueous solutions of each compound? (b) If \(0.1 \mathrm{~mol}\) of each compound is dissolved in solution, which one contains \(0.2 \mathrm{~mol}\) of solute particles, which contains \(0.1 \mathrm{~mol}\) of solute particles, and which contains somewhere between 0.1 and 0.2 mol of solute particles?

(a) Use the following reactions to prepare an activity series for the halogens: $$ \begin{aligned} \mathrm{Br}_{2}(a q)+2 \mathrm{NaI}(a q) & \longrightarrow 2 \mathrm{NaBr}(a q)+\mathrm{I}_{2}(a q) \\ \mathrm{Cl}_{2}(a q)+2 \mathrm{NaBr}(a q) & \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{Br}_{2}(a q) \end{aligned} $$ (b) Relate the positions of the halogens in the periodic table with their locations in this activity series. (c) Predict whether a reaction occurs when the following reagents are mixed: \(\mathrm{Cl}_{2}(a q)\) and \(\mathrm{KI}(a q) ; \operatorname{Br}_{2}(a q)\) and \(\operatorname{LiCl}(a q)\)
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