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Chapter 4: Problem 18

A typical solution used in general chemistry laboratories is 3.0 M HCl. Describe, in detail, the composition of 2.0 L of a 3.0-M HCl solution. How would 2.0 L of a \(3.0-M \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) solution differ from the same quantity of the HCl solution?

Short Answer

Expert verified
The composition of 2.0 L of a 3.0 M HCl solution consists of 6.0 moles of HCl dissolved in water, where HCl completely dissociates into 6.0 moles of H+ ions and 6.0 moles of Cl- ions. Comparatively, 2.0 L of a 3.0 M HC2H3O2 (acetic acid) solution also contains 6.0 moles of solute; however, it does not completely dissociate due to its weak acidic nature, resulting in fewer H+ and C2H3O2- ions. This makes the HCl solution more acidic than the HC2H3O2 solution.

Step by step solution

01

Find the number of moles of solute in each solution

To find the number of moles of solute in a solution, we can use the equation: moles = Molarity * Volume. For the 3.0 M HCl solution: moles of HCl = Molarity * Volume moles of HCl = 3.0 mol/L * 2.0 L moles of HCl = 6.0 mol For the 3.0 M HC2H3O2 solution: moles of HC2H3O2 = Molarity * Volume moles of HC2H3O2 = 3.0 mol/L * 2.0 L moles of HC2H3O2 = 6.0 mol Now that we know the number of moles of solute in each solution, we can compare their compositions.
02

Describe the composition of the 3.0 M HCl solution

A 2.0 L solution of 3.0 M HCl contains 6.0 moles of HCl dissolved in enough water to make 2.0 L of the solution. Hydrochloric acid (HCl) is a strong acid, meaning that it completely dissociates (separates) into its constituent ions (H+ and Cl-) in solution. In this case, we would have 6.0 moles of H+ ions and 6.0 moles of Cl- ions in the 2.0 L solution.
03

Describe the composition of the 3.0 M HC2H3O2 solution

A 2.0 L solution of 3.0 M HC2H3O2 (acetic acid) contains 6.0 moles of HC2H3O2 dissolved in enough water to make 2.0 L of the solution. Acetic acid is a weak acid, which means that it does not completely dissociate into its constituent ions (H+ and C2H3O2-) in the solution. Thus, in this case, there will be fewer than 6.0 moles of H+ ions, and fewer than 6.0 moles of C2H3O2- ions in the solution, with some HC2H3O2 molecules remaining undissociated (intact).
04

Compare the two solutions

Based on the above analysis, we can see that both 3.0 M HCl and 3.0 M HC2H3O2 solutions contain 6.0 moles of solute in 2.0 L of water. In the HCl solution, all 6.0 moles of HCl dissociate into H+ and Cl- ions. However, in the HC2H3O2 solution, not all 6.0 moles of acetic acid dissociate into H+ and C2H3O2- ions due to its weak acidic nature. As a result, the HCl solution would have a higher concentration of H+ ions, making it more acidic than the HC2H3O2 solution.

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Most popular questions from this chapter

Citric acid, which can be obtained from lemon juice, has the molecular formula \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}\) . A 0.250 -g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?

A 6.50-g sample of a diprotic acid requires 137.5 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid.

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