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Chapter 4: Problem 13

State whether each of the following statements is true or false. Justify your answer in each case. (a) Electrolyte solutions conduct electricity because electrons are moving through the solution. (b) If you add a nonelectrolyte to an aqueous solution that already contains an electrolyte, the electrical conductivity will not change.

Short Answer

Expert verified
(a) False, because ions, not electrons, conduct electricity. (b) True, because nonelectrolytes do not affect ion concentration.

Step by step solution

01

Understanding Electrolyte Solutions

Electrolyte solutions conduct electricity due to the presence of ions. In these solutions, cations and anions carry electric current by moving through the solution, not electrons.
02

Evaluating Statement (a)

Statement (a) is incorrect. In electrolyte solutions, the electric current is conducted by the movement of ions (charged particles), not electrons. Thus, stating that electrons move through the solution is false.
03

Understanding Nonelectrolytes

Nonelectrolytes do not dissociate into ions when dissolved in water; they do not contribute to electrical conductivity. Adding them to a solution containing an electrolyte should not affect the total ion concentration.
04

Evaluating Statement (b)

Statement (b) is true. Adding a nonelectrolyte to a solution already containing an electrolyte should not change the electrical conductivity, as nonelectrolytes do not provide additional ions that can carry a charge.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electrical Conductivity
Electrical conductivity refers to the ability of a substance to conduct electricity. In the context of solutions, it's crucial to understand that this happens due to the presence of charged particles, known as ions. These ions move through the solution, allowing electric current to pass.
Ions are produced when an electrolyte, such as salt, dissolves in water. The electrolyte dissociates into positive and negative ions, which are free to move around. This movement of ions is what allows the solution to conduct electricity.
It's a common misconception that electrons move through the solution to conduct electricity, but in fact, it's the ions that do the job.
  • Ions are essential for conductivity.
  • The solution needs movement of these ions to conduct electricity.
Thus, electrolyte solutions are good conductors of electricity due to the ion movement.
Nonelectrolytes
Nonelectrolytes are substances that, when dissolved in water, do not produce ions. Because they do not dissociate into charged particles, they do not contribute to the electrical conductivity of a solution.
Examples of nonelectrolytes include sugar and urea. These compounds dissolve in water, but their molecules remain intact and do not split into ions. As a result, adding a nonelectrolyte to a solution that already contains an electrolyte does not significantly change the electrical conductivity.
  • Nonelectrolytes don't form ions in solutions.
  • These substances do not help in conducting electricity.
Thus, a nonelectrolyte does not affect the electrical conductivity, reinforcing the understanding that the presence of ions is necessary for conducting electricity.
Ions in Solutions
Ions in solutions are the charged particles that enable the conduction of electricity. When an electrolyte dissolves in water, it breaks down into its constituent ions. For example, a salt like sodium chloride (NaCl) dissociates into sodium ions (Na+) and chloride ions (Cl-).
These ions move freely in the solution, allowing them to carry electrical current through the liquid. The more ions that are present, the better the solution can conduct electricity. This is why a concentrated electrolyte solution conducts electricity more efficiently than a dilute one.
  • Electrolytes dissociate into ions.
  • More ions equate to better conductivity.
Understanding how ions function in solutions helps us grasp why some solutions are conductors and others are not.

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Most popular questions from this chapter

A fertilizer railroad car carrying \(129,840 \mathrm{~L}\) of commercial aqueousammonia (30\% ammonia by mass) tips over and spills. The density of the aqueous ammonia solution is \(0.88 \mathrm{~g} / \mathrm{cm}^{3}\). What mass of citric acid, \(\mathrm{C}(\mathrm{OH})(\mathrm{COOH})\left(\mathrm{CH}_{2} \mathrm{COOH}\right)_{2},\) (which contains three acidic protons) is required to neutralize the spill?

The average adult human male has a total blood volume of 5.0 \(\mathrm{L}\). If the concentration of sodium ion in this average individual is \(0.135 \mathrm{M},\) what is the mass of sodium ion circulating in the blood?

Neurotransmitters are molecules that are released by nerve cells to other cells in our bodies, and are needed for muscle motion, thinking, feeling, and memory. Dopamine is a common neurotransmitter in the human brain.(a) Predict what kind of reaction dopamine is most likely to undergo in water: redox, acid-base, precipitation, or metathesis? Explain your reasoning. (b) Patients with Parkinson's disease suffer from a shortage of dopamine and may need to take it to reduce symptoms. An IV (intravenous fluid) bag is filled with a solution that contains \(400.0 \mathrm{mg}\) dopamine per \(250.0 \mathrm{~mL}\) of solution. What is the concentration of dopamine in the IV bag in units of molarity? (c) Experiments with rats show that if rats are dosed with \(3.0 \mathrm{mg} / \mathrm{kg}\) of cocaine (that is, \(3.0 \mathrm{mg}\) cocaine per \(\mathrm{kg}\) of animal mass \(),\) the concentration of dopamine in their brains increases by \(0.75 \mu M\) after 60 seconds. Calculate how many molecules of dopamine would be produced in a rat (average brain volume \(5.00 \mathrm{~mm}^{3}\) ) after 60 seconds of a \(3.0 \mathrm{mg} / \mathrm{kg}\) dose of cocaine.

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) \(\mathrm{P}_{4}(s)+10 \mathrm{HClO}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) $$ 4 \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+10 \mathrm{HCl}(a q) $$ (b) \(\mathrm{Br}_{2}(l)+2 \mathrm{~K}(s) \longrightarrow 2 \mathrm{KBr}(s)\) (c) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g)\) (d) \(\mathrm{ZnCl}_{2}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow \mathrm{Zn}(\mathrm{OH})_{2}(s)+\) $$ 2 \mathrm{NaCl}(a q) $$

Federal regulations set an upper limit of 50 parts per million (ppm) of \(\mathrm{NH}_{3}\) in the air in a work environment [that is, 50 molecules of \(\mathrm{NH}_{3}(g)\) for every million molecules in the air]. Air from a manufacturing operation was drawn through a solution containing \(1.00 \times 10^{2} \mathrm{~mL}\) of \(0.0105 \mathrm{M} \mathrm{HCl}\). The \(\mathrm{NH}_{3}\) reacts with HCl according to: $$ \mathrm{NH}_{3}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NH}_{4} \mathrm{Cl}(a q) $$ After drawing air through the acid solution for 10.0 min at a rate of \(10.0 \mathrm{~L} / \mathrm{min},\) the acid was titrated. The remaining acid needed \(13.1 \mathrm{~mL}\) of \(0.0588 \mathrm{M} \mathrm{NaOH}\) to reach the equivalence point. (a) How many grams of \(\mathrm{NH}_{3}\) were drawn into the acid solution? (b) How many ppm of \(\mathrm{NH}_{3}\) were in the air? (Air has a density of \(1.20 \mathrm{~g} / \mathrm{L}\) and an average molar mass of \(29.0 \mathrm{~g} / \mathrm{mol}\) under the conditions of the experiment.) \((\mathbf{c})\) Is this manufacturer in compliance with regulations?
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