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Chapter 4: Problem 20

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

Short Answer

Expert verified
In aqueous solutions, the solutes present are as follows: 1. Acetone (Nonelectrolyte): CH3COCH3 2. Hypochlorous acid (Weak electrolyte): HClO, H+, ClO- 3. Ammonium chloride (Strong electrolyte): NH4+, Cl- For a 0.1 mol solution: 1. Acetone contains 0.1 mol of solute particles. 2. Hypochlorous acid contains between 0.1 and 0.2 mol of solute particles. 3. Ammonium chloride contains 0.2 mol of solute particles.

Step by step solution

01

Identify solutes in aqueous solutions of each compound

Here is a list of given compounds and their classification as electrolytes: 1. Acetone (CH3COCH3) - Nonelectrolyte 2. Hypochlorous acid (HClO) - Weak electrolyte 3. Ammonium chloride (NH4Cl) - Strong electrolyte In the case of a nonelectrolyte, the compound does not dissociate into ions. In weak electrolytes, the compound partially dissociates into ions. For strong electrolytes, the compound completely dissociates into ions. Solutes in aqueous solutions for each compound are as follows: 1. Acetone: CH3COCH3 2. Hypochlorous acid: HClO, H+, ClO- 3. Ammonium chloride: NH4+, Cl-
02

Determine the number of moles of solute particles in a 0.1 mol solution of each compound

Let's examine each compound: (a) Acetone: Since it is a nonelectrolyte, it remains intact in the solution, so there are 0.1 mol of acetone molecules in the solution. (b) Hypochlorous acid: As a weak electrolyte, it partially dissociates into ions. However, the exact degree of dissociation is not given, so we only know that the number of moles of solute particles will be somewhere between 0.1 and 0.2 moles. (c) Ammonium chloride: This strong electrolyte completely dissociates into its constituent ions: NH4+ and Cl-. Therefore, every 0.1 mol of ammonium chloride dissociates into 0.1 mol of NH4+ ions and 0.1 mol of Cl- ions, resulting in a total of 0.2 mol of solute particles.
03

Summary

In aqueous solutions, the solutes present are as follows: 1. Acetone (Nonelectrolyte): CH3COCH3 2. Hypochlorous acid (Weak electrolyte): HClO, H+, ClO- 3. Ammonium chloride (Strong electrolyte): NH4+, Cl- For a 0.1 mol solution: 1. Acetone contains 0.1 mol of solute particles. 2. Hypochlorous acid contains between 0.1 and 0.2 mol of solute particles. 3. Ammonium chloride contains 0.2 mol of solute particles.

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Most popular questions from this chapter

Which element is oxidized, and which is reduced in the following reactions? \begin{equation} \begin{array}{l}{\text { (a) } \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)\longrightarrow} \\ {\text { (b) } 3 \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{Al}(s) \longrightarrow} \\\\\quad \quad\quad\quad\quad\quad\quad\quad\quad\quad\quad{3 \mathrm{Fe}(s)+2 \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)}\\\\{\text { (c) } \mathrm{Cl}_{2}(a q)+2 \operatorname{Nal}(a q) \longrightarrow \mathrm{I}_{2}(a q)+2 \mathrm{NaCl}(a q)} \\ {\text { (d) } \mathrm{PbS}(s)+4 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)+4 \mathrm{H}_{2} \mathrm{O}(l)}\end{array} \end{equation}

Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid, (b) chromium with hydrobromic acid, (c) tin with hydrochloric acid, (d) aluminum with formic acid, HCOOH.

Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a netionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactions in part (a), how could you distinguish any of the three magnesium substances from the other two?

(a) What volume of 0.115 \(\mathrm{M} \mathrm{HClO}_{4}\) solution is needed to neutralize 50.00 \(\mathrm{mL}\) of 0.0875 \(\mathrm{M} \mathrm{NaOH} ?(\mathbf{b})\) What volume of 25.8 \(\mathrm{mL}\) of an AgNO \(_{3}\) solution is needed to precipitate all the \(\mathrm{Cl}^{-}\) ions in a 785 -mg sample of \(\mathrm{KCl}\) (forming AgCl), what is the molarity of the AgNO \(_{3}\) solution? (d) If 45.3 \(\mathrm{mL}\) of a 0.108 \(M \mathrm{HCl}\) solution is needed to neutralize a solution of \(\mathrm{KOH}\) , how many grams of \(\mathrm{KOH}\) must be present in the solution?

Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium bicarbonate on it and then mopping up the resulting solution. The sodium bicarbonate reacts with sulfuric acid according to: \begin{equation} \begin{array}{r}{2 \mathrm{NaHCO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+} \quad\\\ {2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g)}\end{array} \end{equation} Sodium bicarbonate is added until the fizzing due to the formation of \(\mathrm{CO}_{2}(g)\) stops. If 27 \(\mathrm{mL}\) of 6.0 \(\mathrm{MH}_{2} \mathrm{SO}_{4}\) was spilled, what is the minimum mass of \(\mathrm{NaHCO}_{3}\) that must be added to the spill to neutralize the acid?
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