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Chapter 16: Problem 15

(a) Give the conjugate base of the following Bronsted- Lowry acids: (i) \(\mathrm{HIO}_{3}\), (ii) \(\mathrm{NH}_{4}^{+}\). (b) Give the conjugate acid of the following Bronsted-Lowry bases: (i) \(\mathrm{O}^{2-}\) (ii) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)

Short Answer

Expert verified
(a) The conjugate bases are: (i) \( IO_{3}^{-} \) for \( HIO_{3} \) (ii) \( NH_{3} \) for \( NH_{4}^{+} \) (b) The conjugate acids are: (i) \( OH^{-} \) for \( O^{2-} \) (ii) \( H_{3}PO_{4} \) for \( H_{2}PO_{4}^{-} \)

Step by step solution

01

Find the conjugate base of HIO3 (i)

To find the conjugate base of the Bronsted-Lowry acid HIO3, we need to remove one proton (H+) from its formula. So, HIO3 loses one proton to give the conjugate base IO3-. The balanced equation can be written as: HIO3 ⇆ H+ + IO3^-
02

Find the conjugate base of NH4+ (ii)

To find the conjugate base of the Bronsted-Lowry acid NH4+, we need to remove one proton (H+) from its formula. So, NH4+ loses one proton to give the conjugate base NH3. The balanced equation can be written as: NH4+ ⇆ H+ + NH3
03

Find the conjugate acid of O^2- (i)

To find the conjugate acid of the Bronsted-Lowry base O^2-, we need to add one proton (H+) to its formula. So, O^2- gains one proton to give the conjugate acid OH^-. The balanced equation can be written as: O^2- + H+ ⇆ OH^-
04

Find the conjugate acid of H2PO4^- (ii)

To find the conjugate acid of the Bronsted-Lowry base H2PO4^-, we need to add one proton (H+) to its formula. So, H2PO4^- gains one proton to give the conjugate acid H3PO4. The balanced equation can be written as: H2PO4^- + H+ ⇆ H3PO4 So, the conjugate bases are IO3^- for HIO3 and NH3 for NH4+, while the conjugate acids are OH^- for O^2- and H3PO4 for H2PO4^-.

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Most popular questions from this chapter

Complete the following table by calculating the missing entries. In each case indicate whether the solution is acidic or basic. $$ \begin{array}{llll} \hline\left[\mathrm{H}^{+}\right] & \mathrm{OH}^{-} \text {(aq) } && \mathrm{pH} & &\text { pOH }&& \text { Acidic or basic? } \\ \hline 7.5 \times 10^{-3} \mathrm{M} & & & & \\ & 3.6 \times 10^{-10} \mathrm{M} & & \\ & && 8.25 & & \\ & & &&& 5.70 & \end{array} $$

The amino acid glycine \(\left(\mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COOH}\right)\) can participate in the following equilibria in water: $$ \begin{aligned} \mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COOH}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \\ \mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COO}^{-}+\mathrm{H}_{3} \mathrm{O}^{+} \quad K_{a}=4.3 \times 10^{-3} \\ \mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COOH}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \\ +\mathrm{H}_{3} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COOH}+\mathrm{OH}^{-} \quad K_{b}=6.0 \times 10^{-5} \end{aligned} $$ (a) Use the values of \(K_{a}\) and \(K_{b}\) to estimate the equilibrium constant for the intramolecular proton transfer to form a zwitterion: $$ \mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COOH} \rightleftharpoons{ }^{+} \mathrm{H}_{3} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COO}^{-} $$ What assumptions did you need to make? (b) What is the pH of a \(0.050 \mathrm{M}\) aqueous solution of glycine? (c) What would be the predominant form of glycine in a solution with \(\mathrm{pH} 13 ?\) With \(\mathrm{mH}^{1} ?\)

How does the acid strength of an oxyacid depend on (a) the electronegativity of the central atom; (b) the number of nonprotonated oxygen atoms in the molecule?

Deuterium oxide \(\left(\mathrm{D}_{2} \mathrm{O},\right.\) where \(\mathrm{D}\) is deuterium, the hydrogen- 2 isotope) has an ion-product constant, \(K_{w^{+}}\) of \(8.9 \times 10^{-16}\) at \(20^{\circ} \mathrm{C}\). Calculate \(\left[\mathrm{D}^{+}\right]\) and \(\left[\mathrm{OD}^{-}\right]\) for pure (neutral) \(\mathrm{D}_{2} \mathrm{O}\) at this temperature.

Calculate the percent ionization of propionic acid \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{COOH}\right)\) in solutions of each of the following concentrations \(\left(K_{a}\right.\) is given in Appendix \(\left.D\right):\) (a) \(0.250 \mathrm{M}\), (b) \(0.0800 \mathrm{M}\), (c) \(0.0200 \mathrm{M}\).
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