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Chapter 4: Problem 33

State whether each of the following statements is true or false. Justify your answer in each case. (a) Sulfuric acid is a monoprotic acid. (b) \(\mathrm{HCl}\) is a weak acid. (c) Methanol is a base.

Short Answer

Expert verified
(a) False. Sulfuric acid (\(\mathrm{H_2SO_4}\)) is a diprotic acid, as it can donate two protons (\(\mathrm{H^+}\)) per molecule. (b) False. Hydrochloric acid (\(\mathrm{HCl}\)) is a strong acid, as it dissociates completely in water. (c) False. Methanol (\(\mathrm{CH_3OH}\)) is an alcohol, not a base, as it does not have the properties of a typical base.

Step by step solution

01

a) Sulfuric acid is a monoprotic acid.

This statement is false. A monoprotic acid is an acid that can donate only one proton (\(\mathrm{H^+}\)) per molecule when it dissociates in water. Sulfuric acid (\(\mathrm{H_2SO_4}\)) is a diprotic acid as it can donate two protons (\(\mathrm{H^+}\)) per molecule. The dissociation of sulfuric acid in water can be written as: \[ \mathrm{H_2SO_4 \rightarrow H^+ + HSO_4^-} \] \[ \mathrm{HSO_4^- \rightarrow H^+ + SO_4^{2-}} \] Since sulfuric acid can donate two protons, it is not a monoprotic acid and this statement is false.
02

b) \(\mathrm{HCl}\) is a weak acid.

This statement is false. An acid's strength is determined by its ability to dissociate completely into its ions in water. Hydrochloric acid (\(\mathrm{HCl}\)) is a strong acid because it dissociates completely in water. The dissociation of \(\mathrm{HCl}\) in water can be written as: \[ \mathrm{HCl \rightarrow H^+ + Cl^-} \] Since \(\mathrm{HCl}\) dissociates completely into its ions, it is a strong acid, not a weak acid. Therefore, this statement is false.
03

c) Methanol is a base.

This statement is false. Methanol (\(\mathrm{CH_3OH}\)) is an alcohol, not a base. A base is a substance that can accept protons (\(\mathrm{H^+}\)) or donate electron pairs. Methanol does not have the properties of a typical base, as it does not have a basic functional group (such as an amine group) that can donate electron pairs or accept protons. Methanol's structure is as follows: \[ \mathrm{CH_3 - OH} \] Although the oxygen atom in methanol has a pair of non-bonded electrons, it does not have a significant tendency to donate electron pairs or accept protons, thus it cannot be considered as a base. Therefore, this statement is false.

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Most popular questions from this chapter

Determine the oxidation number of sulfur in each of the following substances: (a) barium sulfate, \(\mathrm{BaSO}_{4}\), (b) sulfurous acid, \(\mathrm{H}_{2} \mathrm{SO}_{3}\), (c) strontium sulfide, \(\mathrm{SrS}\), (d) hydrogen sulfide, \(\mathrm{H}_{2} \mathrm{~S}\). (e) Locate sulfur in the periodic table in Exercise 4.47; what region is it in? (f) Which region(s) of the period table contains elements that can adopt both positive and negative oxidation numbers?

Suppose you have a solution that might contain any or all of the following cations: \(\mathrm{Ni}^{2+}, \mathrm{Ag}^{+}, \mathrm{Sr}^{2+}\), and \(\mathrm{Mn}^{2+}\). Addition of \(\mathrm{HCl}\) solution causes a precipitate to form. After filtering off the precipitate, \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution is added to the resulting solution and another precipitate forms. This is filtered off, and a solution of \(\mathrm{NaOH}\) is added to the resulting solution. No precipitate is observed. Which ions are present in each of the precipitates? Which of the four ions listed above must be absent from the original solution?

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.

The commercial production of nitric acid involves the following chemical reactions: $$ \begin{aligned} 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) & \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) \\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{NO}_{2}(g) \\ 3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) & \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g) \end{aligned} $$ (a) Which of these reactions are redox reactions? (b) In each redox reaction identify the element undergoing oxidation and the element undergoing reduction. (c) How many grams of ammonia must you start with to make \(1000.0 \mathrm{~L}\) of a \(0.150 \mathrm{M}\) aqueous solution of nitric acid? Assume all the reactions give \(100 \%\) yield.

A 1.248-g sample of limestone rock is pulverized and then treated with \(30.00 \mathrm{~mL}\) of \(1.035 \mathrm{M} \mathrm{HCl}\) solution. The excess acid then requires \(11.56 \mathrm{~mL}\) of \(1.010 \mathrm{M} \mathrm{NaOH}\) for neutralization. Calculate the percentage by mass of calcium carbonate in the rock, assuming that it is the only substance reacting with the \(\mathrm{HCl}\) solution.
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