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Chapter 14: Q2E (page 826)

Question: Write equations that show \({H_2}PO_4^ - \) acting both as an acid and as a base.

Short Answer

Expert verified

When \({H_2}PO_4^ - \) reacts with \({H_2}O\), it gives proton to water. As a result, it acts as an acid. The equation regarding this is as follows

\({H_2}PO_4^ - + {H_2}O \to HPO_4^{2 - } + {H_3}{O^ + }\)

When \({H_2}PO_4^ - \) reacts with \(HCl\), it takes proton from \(HCl\). As a result, it acts as a base.

The equation regarding this is as follows

\({H_2}PO_4^ - + HCl \to {H_3}P{O_4} + C{l^ - }\)

Step by step solution

01

Define the Bronsted-Lowry concept of acid and base.

The Bronsted-lowry concept of acid and base tells that an acid is a proton\(({H^ + })\) donor, and a base is a proton acceptor.

When a Bronsted-Lowry acid loses a proton, a conjugate base is formed. Similarly, when a Bronsted-Lowry base gains a proton, a conjugate acid is formed.

02

\({H_2}PO_4^ - \) as an acid.

\({H_2}PO_4^ - + {H_2}O \to HPO_4^{2 - } + {H_3}{O^ + }\)

Here, \({H_2}PO_4^ - \) is giving proton to water, so it is an acid.

03

\({H_2}PO_4^ - \) as a base.

\({H_2}PO_4^ - + HCl \to {H_3}P{O_4} + C{l^ - }\)

Here, \({H_2}PO_4^ - \) is taking proton, so it is a base.

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Most popular questions from this chapter

The hydronium ion concentration in a sample of rainwater is found to be \(1.7 \times 1{0^{ - 6}}M\) times 25oC. What is the concentration of hydroxide ions in the rainwater?

Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the following equations:

\({\rm{\;(a)\;HN}}{{\rm{O}}_3} + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_3}{{\rm{O}}^ + } + {\rm{NO}}_3^ - \)

\({\rm{b) C}}{{\rm{N}}^ - } + {{\rm{H}}_2}{\rm{O}} \to {\rm{HCN}} + {\rm{O}}{{\rm{H}}^ - }\)

\({\rm{\;(c)\;}}{{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4} + {\rm{C}}{{\rm{l}}^ - } \to {\rm{HCl}} + {\rm{HSO}}_4^ - \)

\({\rm{\;(d)\;HSO}}_4^ - + {\rm{O}}{{\rm{H}}^ - } \to {\rm{SO}}_4^{2 - } + {{\rm{H}}_2}{\rm{O}}\)

\({\rm{\;(e)\;}}{{\rm{O}}^{2 - }} + {{\rm{H}}_2}{\rm{O}} \to 2{\rm{O}}{{\rm{H}}^ - }\)

\({\rm{\;(f)\;}}{\left( {{\rm{Cu}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_3}({\rm{OH}})} \right)^ + } + {\left( {{\rm{Al}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}} \right)^{3 + }} \to {\left( {{\rm{Cu}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_4}} \right)^{2 + }} + {\left( {{\rm{Al}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_5}({\rm{OH}})} \right)^{2 + }}\)

\({\rm{\;(g)\;}}{{\rm{H}}_2}{\rm{S}} + {\rm{NH}}_2^ - \to {\rm{H}}{{\rm{S}}^ - } + {\rm{N}}{{\rm{H}}_3}\)

Which of the following will increase the percentage of \({\rm{N}}{{\rm{H}}_3}\)that is converted to the ammonium ion in water (Hint: Use Le Châtelier's principle)?

(a) Addition of \(NaOH\)

(b) Addition of \(HCl\)

(c) Addition of \(N{H_4}Cl\)

Salicylic acid, \(HO{C_6}{H_4}C{O_2}H\), and its derivatives have been used as pain relievers for a long time. Salicylic acid occurs in small amounts in the leaves, bark, and roots of some vegetation (most notably historically in the bark of the willow tree). Extracts of these plants have been used as medications for centuries. The acid was first isolated in the laboratory in 1838.

(a) Both functional groups of salicylic acid ionize in water, with \({K_a} = 1.0 \times 1{0^{ - 3}}\)for the \( - C{O_2}H\) group and \(4.2 \times 1{0^{ - 13}}\) for the \( - OH \) group. What is the pH of a saturated solution of the acid (solubility \( = 1.8\;g/L)\).

(b) Aspirin was discovered as a result of efforts to produce a derivative of salicylic acid that would not be irritating to the stomach lining. Aspirin is acetylsalicylic acid, \(C{H_3}C{O_2}{C_6}{H_4}C{O_2}H\). The \(C{O_2}H\)functional group is still present, but its acidity is reduced, \({K_a} = 3.0 \times 1{0^{ - 4}}\). What is the pH of a solution of aspirin with the same concentration as a saturated solution of salicylic acid (See Part a).

(c) Under some conditions, aspirin reacts with water and forms a solution of salicylic acid and acetic acid: \(C{H_3}C{O_2}{C_6}{H_4}C{O_2}H(aq) + {H_2}O(l) \to HO{C_6}{H_4}C{O_2}H(aq) + C{H_3}C{O_2}H(aq)\)

i. Which of the acids, salicylic acid or acetic acid, produces more hydronium ions in such a solution?

ii. What are the concentrations of molecules and ions in a solution produced by the hydrolysis of \(0.50\;g\)of aspirin dissolved in enough water to give \(75ml\) of solution?

Determine whether aqueous solutions of the following salts are acidic, basic, or neutral

(a) \( Al{\left( {N{O_3}} \right)_3}\)

(b) \( RbI\)

(c) \( KHC{O_2}\)

(d) \( C{H_3}N{H_3}Br\)
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