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Chapter 4: Problem 45

True or false: (a) If a substance is oxidized, there must be more oxygen in the substance. (b) If a substance is oxidized, it must lose at least one electron and form an anion.

Short Answer

Expert verified
(a) False: While oxidation often involves reacting with oxygen, it is not a requirement for a substance to have more oxygen when oxidized. (b) False: Although oxidation involves losing electrons, losing an electron does not guarantee the formation of an anion; instead, a cation is often formed.

Step by step solution

01

(a) Analyzing Oxidation and Oxygen Content

Oxidation is the process where a substance loses electrons, often by reacting with oxygen. While oxygen is often involved in the oxidation process, it's not a requirement for oxidation to occur. Therefore, it is possible for a substance to be oxidized without necessarily having an increase in oxygen content. Answer: False
02

(b) Analyzing Oxidation and Electron Loss

Oxidation is the loss of electrons from a substance. When a substance is oxidized, it will lose at least one electron. However, losing an electron does not guarantee the formation of an anion. Anions are negatively charged particles formed due to an excess of electrons. When a substance loses electrons, it often forms a cation (positively charged), not an anion. Answer: False

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Most popular questions from this chapter

What kind of reaction is the "water-splitting" reaction? $\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2}(g)+1 / 2 \mathrm{O}_{2}(g)$ (a) an acid-base reaction (b) a metathesis reaction (c) a redox reaction (d) a precipitation reaction [Section 4.4]

Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the aqueous \(\mathrm{HCl}\) in the stomach and each of the following substances used in various antacids: (a) $\mathrm{Al}(\mathrm{OH})_{3}(s),(\mathbf{b}) \mathrm{Mg}(\mathrm{OH})_{2}(s),(\mathbf{c}) \mathrm{MgCO}_{3}(s),$ (d) \(\mathrm{NaAl}\left(\mathrm{CO}_{3}\right)(\mathrm{OH})_{2}(s)\) (e) \(\mathrm{CaCO}_{3}(s)\)

(a) By titration, \(15.0 \mathrm{~mL}\) of \(0.1008 \mathrm{Msodium}\) hydroxide is needed to neutralizea \(0.2053-\mathrm{g}\) sample of a weak acid. What is the molar mass of the acid if it is monoprotic? (b) An elemental analysis of the acid indicates that it is composed of $5.899 \mathrm{H}, 70.6 \% \mathrm{C},\( and \)23.5 \% \mathrm{O}$ by mass. What is its molecular formula?

You choose to investigate some of the solubility guidelines for two ions not listed in Table \(4.1,\) the chromate ion \(\left(\mathrm{CrO}_{4}^{2-}\right)\) and the oxalate ion \(\left(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\right) .\) You are given \(0.01 \mathrm{M}\) solutions \((\mathrm{A}, \mathrm{B}, \mathrm{C}, \mathrm{D})\) of four water- soluble salts: \begin{tabular}{lll} \hline Solution & Solute & Color of Solution \\ \hline \(\mathrm{A}\) & \(\mathrm{Na}_{2} \mathrm{CrO}_{4}\) & Yellow \\ \(\mathrm{B}\) & $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ & Colorless \\ \(\mathrm{C}\) & \(\mathrm{AgNO}_{3}\) & Colorless \\ \(\mathrm{D}\) & \(\mathrm{CaCl}_{2}\) & Colorless \\ \hline \end{tabular} When these solutions are mixed, the following observations are made: \begin{tabular}{lll} \hline Experiment Number & Solutions Mixed & Result \\ \hline 1 & \(\mathrm{~A}+\mathrm{B}\) & Noprecipitate, yellow solution \\ 2 & \(\mathrm{~A}+\mathrm{C}\) & Red precipitate forms \\ 3 & \(\mathrm{~A}+\mathrm{D}\) & Yellow precipitate forms \\ 4 & \(\mathrm{~B}+\mathrm{C}\) & White precipitate forms \\ 5 & \(\mathrm{~B}+\mathrm{D}\) & White precipitate forms \\ 6 & \(\mathrm{C}+\mathrm{D}\) & White precipitate forms \\ \hline \end{tabular} (a) Write a net ionic equation for the reaction that occurs in each of the experiments. (b) Identify the precipitate formed, if any, in each of the experiments.

Hard water contains \(\mathrm{Ca}^{2+}, \mathrm{Mg}^{2+}\), and \(\mathrm{Fe}^{2+}\), which interfere with the action of soap and leave an insoluble coating on the insides of containers and pipes when heated. Water softeners replace these ions with \(\mathrm{Na}^{+} .\) Keep in mind that charge balance must be maintained. (a) If \(1500 \mathrm{~L}\) of hard water contains \(0.020 \mathrm{M} \mathrm{Ca}^{2+}\) and \(0.0040 \mathrm{M} \mathrm{Mg}^{2+}\), how many moles of Nat are needed to replace these ions? (b) If the sodium is added to the water softener in the form of \(\mathrm{NaCl}\), how many grams of sodium chloride are needed?
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