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Chapter 14: Problem 133

Identify the Lewis acid and the Lewis base in each of the following reactions. a. \(\mathrm{B}(\mathrm{OH})_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{B}(\mathrm{OH})_{4}^{-}(a q)+\mathrm{H}^{+}(a q)\) b. \(\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q)\) c. \(\mathrm{BF}_{3}(g)+\mathrm{F}^{-}(a q) \rightleftharpoons \mathrm{BF}_{4}^{-}(a q)\)

Short Answer

Expert verified
In conclusion, for each reaction: a. \( B(OH)_3 \) is the Lewis acid and \( H_2O \) is the Lewis base. b. \( Ag^+ \) is the Lewis acid and \( NH_3 \) is the Lewis base. c. \( BF_3 \) is the Lewis acid and \( F^- \) is the Lewis base.

Step by step solution

01

Identify electron pair donor and acceptor

In the reaction, B(OH)3 accepts an electron pair from H2O to form B(OH)4^-. At the same time, H2O donates a proton H^+. \( \mathrm{B}(\mathrm{OH})_{3} + \mathrm{OH}^{-} \rightleftharpoons \mathrm{B}(\mathrm{OH})_{4}^{-} \)
02

Determine Lewis acid and base

B(OH)3 is the Lewis acid as it accepts an electron pair from the water molecule. H2O is the Lewis base as it donates an electron pair to the B(OH)3. #b. Ag^+(aq) + 2 NH3(aq) 鈬� Ag(NH3)2^+(aq)#
03

Identify electron pair donor and acceptor

Ag^+ accepts an electron pair from two NH3 molecules to form the complex ion Ag(NH3)2^+. \( \mathrm{Ag}^{+} + 2 \mathrm{NH}_{3} \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+} \)
04

Determine Lewis acid and base

Ag^+ is the Lewis acid as it accepts an electron pair from the NH3 molecules. NH3 is the Lewis base as it donates an electron pair to the Ag^+. #c. BF3(g) + F^-(aq) 鈬� BF4^-(aq)#
05

Identify electron pair donor and acceptor

BF3 accepts an electron pair from F^- to form BF4^-. \( \mathrm{BF}_{3} + \mathrm{F}^{-} \rightleftharpoons \mathrm{BF}_{4}^{-} \)
06

Determine Lewis acid and base

BF3 is the Lewis acid as it accepts an electron pair from the F^- ion. F^- is the Lewis base as it donates an electron pair to the BF3. In conclusion, for each reaction: a. B(OH)3 is the Lewis acid and H2O is the Lewis base. b. Ag^+ is the Lewis acid and NH3 is the Lewis base. c. BF3 is the Lewis acid and F^- is the Lewis base.

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Most popular questions from this chapter

A certain acid, HA, has a vapor density of \(5.11 \mathrm{~g} / \mathrm{L}\) when in the gas phase at a temperature of \(25^{\circ} \mathrm{C}\) and a pressure of \(1.00 \mathrm{~atm}\). When \(1.50 \mathrm{~g}\) of this acid is dissolved in enough water to make \(100.0 \mathrm{~mL}\) of solution, the \(\mathrm{pH}\) is found to be \(1.80\). Calculate \(K_{\mathrm{a}}\) for the acid.

Arsenic acid \(\left(\mathrm{H}_{3} \mathrm{AsO}_{4}\right)\) is a triprotic acid with \(K_{\mathrm{a}_{1}}=5 \times 10^{-3}\) \(K_{\mathrm{a}_{2}}=8 \times 10^{-8}\), and \(K_{\mathrm{a}_{3}}=6 \times 10^{-10} \cdot\) Calculate \(\left[\mathrm{H}^{+}\right],\left[\mathrm{OH}^{-}\right]\) \(\left[\mathrm{H}_{3} \mathrm{AsO}_{4}\right],\left[\mathrm{H}_{2} \mathrm{AsO}_{4}^{-}\right],\left[\mathrm{HAsO}_{4}^{2-}\right]\), and \(\left[\mathrm{AsO}_{4}^{3-}\right]\) in a \(0.20 \mathrm{M}\) arsenic acid solution.

Formic acid \(\left(\mathrm{HCO}_{2} \mathrm{H}\right)\) is secreted by ants. Calculate \(\left[\mathrm{H}^{+}\right]\) and the \(\mathrm{pH}\) of a \(0.025 M\) solution of formic acid \(\left(K_{\mathrm{a}}=1.8 \times 10^{-4}\right)\).

Consider \(1000 . \mathrm{mL}\) of a \(1.00 \times 10^{-4} M\) solution of a certain acid HA that has a \(K_{\mathrm{a}}\) value equal to \(1.00 \times 10^{-4} .\) How much water was added or removed (by evaporation) so that a solution remains in which \(25.0 \%\) of HA is dissociated at equilibrium? Assume that HA is nonvolatile.

A solution is prepared by dissolving \(0.56 \mathrm{~g}\) benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2} \mathrm{H}, K_{\mathrm{a}}=6.4 \times 10^{-5}\right)\) in enough water to make \(1.0 \mathrm{~L}\) of solution. Calculate \(\left[\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2} \mathrm{H}\right],\left[\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2}^{-}\right],\left[\mathrm{H}^{+}\right],\left[\mathrm{OH}^{-}\right]\), and the \(\mathrm{pH}\) of this solution.
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