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Chapter 16: Problem 78

The following very strong acids are formed by the reactions indicated: $$ \mathrm{HF}+\mathrm{SbF}_{5} \longrightarrow \mathrm{HSb} \mathrm{F}_{6} $$ (called "super acid," hexafluoroantimonic acid) $$ \mathrm{HF}+\mathrm{BF}_{3} \longrightarrow \mathrm{HBF}_{4} $$ (tetrafluoroboric acid) (a) Identify the Lewis acids and bases. (b) To which atom is the H atom bonded in each acid?

Short Answer

Expert verified
(a) Lewis Acids: \( \mathrm{SbF}_{5} \), \( \mathrm{BF}_{3} \); Lewis Bases: \( \mathrm{HF} \) (b) In \( \mathrm{HSbF}_{6} \), H is bonded to Sb; in \( \mathrm{HBF}_{4} \), H is bonded to B.

Step by step solution

01

Identify Lewis Acids And Bases

In the given reactions, \( \mathrm{HF} \) is the Lewis base in both reactions as it donates an electron pair. In the first reaction, \( \mathrm{SbF}_{5} \) is the Lewis acid as it accepts an electron pair. In the second reaction, \( \mathrm{BF}_{3} \) is the Lewis acid as it also accepts an electron pair.
02

Identify Atoms Bonded to Hydrogen

To find which atom is bonded to the H atom in each acid, analyze the molecular structure of the products from the initial reactions. In \( \mathrm{HSbF}_{6} \), the H atom is bonded to Sb atom. Similarly, in \( \mathrm{HBF}_{4} \), the H atom is bonded to the B atom.

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Most popular questions from this chapter

Explain why \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in a strong acid solution doubles as the total acid concentration doubles, whereas in a weak acid solution, \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) increases only by about a factor of \(\sqrt{2}\)

Write the formula of the conjugate base in the reaction of each acid with water. (a) \(\mathrm{HIO}_{3} ;\) (b) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\) (c) \(\mathrm{HPO}_{4}^{2-} ;\) (d) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\)

What are \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right],\left[\mathrm{OH}^{-}\right], \mathrm{pH},\) and \(\mathrm{pOH}\) of \(0.55 \mathrm{M}\) \(\mathrm{M} \mathrm{HClO}_{2} ?\)

A 28.2 L volume of \(\mathrm{HCl}(\mathrm{g}),\) measured at \(742 \mathrm{mmHg}\) and \(25.0^{\circ} \mathrm{C},\) is dissolved in water. What volume of \(\mathrm{NH}_{3}(\mathrm{g}),\) measured at \(762 \mathrm{mmHg}\) and \(21.0^{\circ} \mathrm{C},\) must be absorbed by the same solution to neutralize the HCl?

Use Lewis structures to diagram the following reaction in the manner of reaction (16.19) $$2 \mathrm{NH}_{3}+\mathrm{Ag}^{+} \longrightarrow\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}$$ Identify the Lewis acid and Lewis base.
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