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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. \begin{equation} \begin{array}{l}{\text { (a) Sulfuric acid is a monoprotic acid. }} \\ {\text { (b) HCl is a weak acid. }} \\ {\text { (c) Methanol is a base. }}\end{array} \end{equation}

Short Answer

Expert verified
(a) FALSE. Sulfuric acid (H₂SO₄) is a diprotic acid, not a monoprotic acid, as it can donate two protons per molecule. (b) FALSE. HCl is a strong acid, not a weak acid, as it dissociates completely in water. (c) FALSE. Methanol (CH3OH) does not typically exhibit basic properties. Instead, it can act as a weak acid by donating a proton from its hydroxyl group.

Step by step solution

01

(a) Determine the nature of sulfuric acid

Sulfuric acid (H₂SO₄) is an acid, so we need to determine if it is monoprotic or not. A monoprotic acid is one that can donate only one proton (H⁺) per molecule. Looking at the chemical formula of sulfuric acid (H₂SO₄), we can see that it contains two hydrogen atoms. This means sulfuric acid can donate two protons per molecule. Therefore, it should be classified as a diprotic acid. So the statement (a) "Sulfuric acid is a monoprotic acid" is FALSE.
02

(b) Determine the acidity of HCl

HCl (hydrochloric acid) is an acid. We need to decide on its strength – whether it is a weak acid or a strong acid. The strength of an acid is determined by how much it dissociates in water. Strong acids dissociate completely in water, while weak acids dissociate only partially. HCl, when dissolved in water, completely dissociates into H⁺ and Cl⁻ ions. \( HCl (aq) \rightarrow H^+ (aq) + Cl^-(aq) \) Since HCl dissociates completely, it is considered a strong acid, not a weak acid. So the statement (b) "HCl is a weak acid" is FALSE.
03

(c) Determine if methanol is a base

Methanol (CH3OH) is an organic compound and belongs to the group of alcohols. We need to examine if it exhibits basic properties or not. A base typically accepts protons (H⁺) in a chemical reaction. Methanol does not typically accept protons in its reactions. Instead, it can act as a weak acid by donating a proton (H⁺) from its hydroxyl group (OH). \( CH3OH \leftrightharpoons H^+ (aq) + CH3O^- (aq) \) So the statement (c) "Methanol is a base" is FALSE.

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Most popular questions from this chapter

The U.S. standard for arsenate in drinking water requires that public water supplies must contain no greater than 10 parts per billion \((\mathrm{ppb})\) arsenic. If this arsenic is present as arsenate, AsO \(_{4}^{3-},\) what mass of sodium arsenate would be present in a 1.00 -L sample of drinking water that just meets the standard? Parts per billion is defined on a mass basis as $$\mathrm{ppb}=\frac{\text { g solute }}{\mathrm{g} \text { solution }} \times 10^{9}$$

Which of the following ions will always be a spectator ion in a precipitation reaction? (a) \(\mathrm{Cl}^{-},(\mathbf{b}) \mathrm{NO}_{3}^{-},(\mathbf{c}) \mathrm{NH}_{4}^{+},(\mathbf{d}) \mathrm{S}^{2}\) , (e) \(\mathrm{SO}_{4}^{2-} .\) [Section 4.2\(]\)

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?

Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) \(\mathrm{NaCH}_{3} \mathrm{COO}\) and \(\mathrm{HCl},\) (b) \(\mathrm{KOH}\) and \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2},(\mathbf{c}) \mathrm{Na}_{2} \mathrm{S}\) and \(\mathrm{CdSO}_{4}\) .

Because the oxide ion is basic, metal oxides react readily with acids.(a) Write the net ionic equation for the following reaction: $$\mathrm{FeO}(s)+2 \mathrm{HClO}_{4}(a q) \longrightarrow \mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$$ (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between \(\mathrm{NiO}(s)\) and an aqueous solution of nitric acid.
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