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Chapter 15: Problem 62

Write all the species (except water) that are present in a phosphoric acid solution. Indicate which species can act as a Brønsted acid, which as a Brønsted base, and which as both a Brønsted acid and a Brønsted base.

Short Answer

Expert verified
The species present in the phosphoric acid solution are \(H_3PO_4\), \(H_2PO_4^-\), \(HPO_4^{2-}\), and \(PO_4^{3-}\). Out of these, \(H_3PO_4\), \(H_2PO_4^-\), and \(HPO_4^{2-}\) can act as a Brønsted acid. \(H_2PO_4^-\), \(HPO_4^{2-}\), and \(PO_4^{3-}\) can act as a Brønsted base. \(H_2PO_4^-\) and \(HPO_4^{2-}\) can act as both a Brønsted acid and a Brønsted base.

Step by step solution

01

Identify All the Species in a Phosphoric Acid Solution

Phosphoric acid (\(H_3PO_4\)) is a triprotic acid, meaning it has three protons it can donate. When phosphoric acid dissociates, it does so in stages, generating the following species: \(H_3PO_4\), \(H_2PO_4^-\), \(HPO_4^{2-}\), \(PO_4^{3-}\).
02

Determine Which Species Act as a Brønsted Acid

Brønsted acids are species that donate protons or \(H^+\). Thus, \(H_3PO_4\), \(H_2PO_4^-\) and \(HPO_4^{2-}\) can function as Brønsted acids, as they all have protons that they can donate.
03

Determine Which Species Act as a Brønsted Base

Brønsted bases are species that accept protons or \(H^+\). Hence, \(H_2PO_4^-\), \(HPO_4^{2-}\), and \(PO_4^{3-}\) can act as Brønsted bases because they can accept protons.
04

Determine Which Species Act as Both a Brønsted Acid and a Brønsted Base

A species that can both donate and accept a proton is called an amphoteric species. Hence, \(H_2PO_4^-\) and \(HPO_4^{2-}\) can act as both a Brønsted acid and a Brønsted base.

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Most popular questions from this chapter

A typical reaction between an antacid and the hydrochloric acid in gastric juice is \(\mathrm{NaHCO}_{3}(s)+\mathrm{HCl}(a q) \rightleftharpoons\) $$ \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g) $$ Calculate the volume (in L) of \(\mathrm{CO}_{2}\) generated from \(0.350 \mathrm{~g}\) of \(\mathrm{NaHCO}_{3}\) and excess gastric juice at 1.00 atm and \(37.0^{\circ} \mathrm{C}\).

Calculate the hydrogen ion concentration in \(\mathrm{mol} / \mathrm{L}\) for each of the following solutions: (a) a solution whose \(\mathrm{pH}\) is \(5.20,\) (b) a solution whose \(\mathrm{pH}\) is 16.00 , (c) a solution whose hydroxide concentration is \(3.7 \times 10^{-9} M\).

Give an example of the following: (a) a weak acid that contains oxygen atoms, (b) a weak acid that does not contain oxygen atoms, (c) a neutral molecule that acts as a Lewis acid, (d) a neutral molecule that acts as a Lewis base, (e) a weak acid that contains two ionizable \(\mathrm{H}\) atoms, (f) a conjugate acidbase pair, both of which react with \(\mathrm{HCl}\) to give carbon dioxide gas.

Classify each of the following species as a weak or strong acid: (a) \(\mathrm{HNO}_{3},\) (b) HF, (c) \(\mathrm{H}_{2} \mathrm{SO}_{4},\) (d) \(\mathrm{HSO}_{4}^{-}\), (e) \(\mathrm{H}_{2} \mathrm{CO}_{3},\) (f) \(\mathrm{HCO}_{3}^{-},(\mathrm{g}) \mathrm{HCl}\) (h) \(\mathrm{HCN}\), (i) \(\mathrm{HNO}_{2}\).

Malonic acid \(\left[\mathrm{CH}_{2}(\mathrm{COOH})_{2}\right]\) is a diprotic acid. Compare its two \(K_{\mathrm{a}}\) values with that of acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\left(K_{\mathrm{a}}\right),\) and account for the differences in the three \(K_{\mathrm{a}}\) values.
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