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Chapter 16: Problem 6

Give the conjugate acid of each of these bases: (a) \(\mathrm{HS}^{-}\) (b) \(\mathrm{HCO}_{3}^{-}\) (c) \(\mathrm{CO}_{3}^{2-}\) (d) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (e) \(\mathrm{HPO}_{4}^{2-}, \quad\) (f) \(\mathrm{PO}_{4}^{3-}\) (g) \(\mathrm{HSO}_{4}^{-}\) (h) \(\mathrm{SO}_{4}^{2-}\) (i) \(\mathrm{NO}_{2}^{-}\) (j) \(\mathrm{SO}_{3}^{2-}\)

Short Answer

Expert verified
The conjugate acids are: (a) \(H_{2}S\), (b) \(H_{2}CO_{3}\), (c) \(HCO_{3}^{-}\), (d) \(H_{3}PO_{4}\), (e) \(H_{2}PO_{4}^{-}\), (f) \(HPO_{4}^{2-}\), (g) \(H_{2}SO_{4}\), (h) \(HSO_{4}^{-}\), (i) \(HNO_{2}\), and (j) \(HSO_{3}^{-}\).

Step by step solution

01

Identifying the conjugate acid of \(HS^{-}\)

Adding a proton (\(H^{+}\)) to \(HS^{-}\) forms the conjugate acid \(H_{2}S\), as the negative charge is neutralized by the proton.
02

Identifying the conjugate acid of \(HCO_{3}^{-}\)

Adding a proton to \(HCO_{3}^{-}\) leads to \(H_{2}CO_{3}\), which is the matching conjugate acid.
03

Identifying the conjugate acid of \(CO_{3}^{2-}\)

In this case, adding a proton to \(CO_{3}^{2-}\) results in \(HCO_{3}^{-}\), balancing, and reducing the negative charge by one.
04

Identifying the conjugate acid of \(H_{2}PO_{4}^{-}\)

Add a proton to \(H_{2}PO_{4}^{-}\) to form \(H_{3}PO_{4}\), thereby neutralizing the negative charge and forming the conjugate acid.
05

Identifying the conjugate acid of \(HPO_{4}^{2-}\)

Adding a proton to \(HPO_{4}^{2-}\) forms \(H_{2}PO_{4}^{-}\), reducing the negative charge by one.
06

Identifying the conjugate acid of \(PO_{4}^{3-}\)

Adding a proton to \(PO_{4}^{3-}\) forms \(HPO_{4}^{2-}\), reducing the charge by one.
07

Identifying the conjugate acid of \(HSO_{4}^{-}\)

By adding a proton to \(HSO_{4}^{-}\), \(H_{2}SO_{4}\) is formed, neutralizing the negative charge.
08

Identifying the conjugate acid of \(SO_{4}^{2-}\)

Adding a proton to \(SO_{4}^{2-}\) results in \(HSO_{4}^{-}\), reducing the negative charge by one.
09

Identifying the conjugate acid of \(NO_{2}^{-}\)

Adding a proton to \(NO_{2}^{-}\) results in \(HNO_{2}\), neutralizing the negative charge.
10

Identifying the conjugate acid of \(SO_{3}^{2-}\)

If a proton is added to \(SO_{3}^{2-}\), \(HSO_{3}^{-}\) is created, reducing the charge by one.

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Most popular questions from this chapter

Prediet the \(\mathrm{pH}(>7,<7,\) or \(\approx 7)\) of the aqueous solutions containing the following salts: (a) \(\mathrm{KBr}\) (b) \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) (c) \(\mathrm{BaCl}_{2}\) (d) \(\mathrm{Bi}\left(\mathrm{NO}_{3}\right)_{3}\).

In terms of orbitals and electron arrangements, what must be present for a molecule or an ion to act as a Lewis acid (use \(\mathrm{H}^{+}\) and \(\mathrm{BF}_{3}\) as examples)? What must be present for a molecule or ion to act as a Lewis base (use \(\mathrm{OH}^{-}\) and \(\mathrm{NH}_{3}\) as examples)?

A solution is made by dissolving \(18.4 \mathrm{~g}\) of \(\mathrm{HCl}\) in 662 \(\mathrm{mL}\) of water. Calculate the \(\mathrm{pH}\) of the solution. (Assume that the volume of the solution is also \(662 \mathrm{~mL} .)\)

Give the conjugate base of each of these acids: (a) \(\mathrm{CH}_{2} \mathrm{ClCOOH},\) (b) \(\mathrm{HIO}_{4}\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{4},\) (d) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (e) \(\mathrm{HPO}_{4}^{2-},\) (f) \(\mathrm{H}_{2} \mathrm{SO}_{4},(\mathrm{~g}) \mathrm{HSO}_{4}^{-}\) (h) \(\mathrm{HCOOH}\) (i) \(\mathrm{HSO}_{3}^{-},(\mathrm{j}) \mathrm{NH}_{4}^{+},(\mathrm{k}) \mathrm{H}_{2} \mathrm{~S},\) (l) \(\mathrm{HS}^{-},(\mathrm{m}) \mathrm{HClO}\).

Write the equation relating \(K_{\mathrm{a}}\) for a weak acid and \(K_{\mathrm{b}}\) for its conjugate base. Use \(\mathrm{NH}_{3}\) and its conjugate acid \(\mathrm{NH}_{4}^{+}\) to derive the relationship between \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\).
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