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Chapter 14: Q4E (page 826)

Question: Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry acid: (a) \(HN{O_3}\) (b) \(PH_4^ + \) (c) \({H_2}S\) (d) \(C{H_3}C{H_2}COOH\) (e) \({H_2}PO_4^ - \) (f) \(H{S^ - }\)

Short Answer

Expert verified

All the given six species act as a Bronsted-lowry acid as all these species donates a proton (\({H^ + }\)) to another molecule. The required equations are as follows.

Step by step solution

01

Define the concept of Bronsted-Lowry acid

The concept states that any compound that can transfer a proton to any other compound is an acid. In other words, the proton donor in a chemical reaction is a Bronsted-Lowry acid.

02

Suitable net ionic equations which shows that given species act as Bronsted-Lowry acid

So, it is observed that each of the species donates a proton (\({H^ + }\)) to another molecule. So. all the above species are Bronsted-Lowry acid.

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Most popular questions from this chapter

What two common assumptions can simplify calculation of equilibrium concentrations in a solution of a weak acid?

Which base in Table 14.3 is most appropriate for preparation of a buffer solution with a pH of 10.65? Explain your choice.

Calculate the concentration of each species present in a \(0.010M\) solution of phthalic acid, \({C_6}{H_4}{\left( {C{O_2}H} \right)_2}\).

\(\begin{array}{*{20}{c}}{{C_6}{H_4}{{\left( {C{O_2}H} \right)}_2}(aq) + {H_2}O(l) \rightleftharpoons {H_3}{O^ + }(aq) + {C_6}{H_4}\left( {C{O_2}H} \right){{\left( {C{O_2}} \right)}^ - }(aq)}&{{K_a} = 1.1 \times 1{0^{ - 3}}} \\ {{C_6}{H_4}\left( {C{O_2}H} \right)\left( {C{O_2}} \right)(aq) + {H_2}O(l) \rightleftharpoons {H_3}{O^ + }(aq) + {C_6}{H_4}{{\left( {C{O_2}} \right)}_2}^{2 - }(aq)}&{{K_a} = 3.9 \times 1{0^{ - 6}}} \end{array}\)

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?

Which of the following will increase the percentage of HF that is converted to the fluoride ion in water?

(a) Addition of \(NaOH\)

(b) Addition of \(HCl\)

(c) Addition of \(NaF\)
See all solutions

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