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Chapter 16: Problem 65

Predict which is the stronger acid: (a) \(\mathrm{HClO}_{2}\) or \(\mathrm{HClO}_{3} ;(\mathrm{b}) \mathrm{H}_{2} \mathrm{CO}_{3}\) or \(\mathrm{HNO}_{2} ;(\mathrm{c}) \mathrm{H}_{2} \mathrm{SiO}_{3}\) or \(\mathrm{H}_{3} \mathrm{PO}_{4}\) Explain.

Short Answer

Expert verified
The stronger acids are HClO3, HNO2, and H3PO4.

Step by step solution

01

Compare the conjugate bases of HClO2 and HClO3

The conjugate base of HClO2 is ClO2-, and of HClO3 is ClO3-. Due to the extra oxygen in ClO3-, it is more stable than ClO2-. This is because an extra oxygen atom allows the negative charge to be spread across more atoms, stabilizing the ion.
02

Compare the conjugate bases of H2CO3 and HNO2

The conjugate base of H2CO3 is HCO3-, and of HNO2 is NO2-. The conjugate base NO2- is more stable than HCO3-, since it has an extra oxygen atom to stabilize the negative charge. Also, nitrate ions are generally more stable than carbonate ions due to the superior electronegtivity of nitrogen.
03

Comparing the conjugate bases of H2SiO3 and H3PO4

The conjugate base of H2SiO3 is HSiO3-, and of H3PO4 is H2PO4-. The H2PO4- ion is more stable than HSiO3-, since phosphorus is in the third period of the periodic table and can expand its octet to accommodate the negative charge better than silicon. Additionally, the conjugate base of H3PO4 has an additional hydrogen atom, which can also help to balance the negative charge.

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Most popular questions from this chapter

Propionic acid, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH},\) is \(0.42 \%\) ionized in \(0.80 \mathrm{M}\) solution. The \(K_{\mathrm{a}}\) for this acid is (a) \(1.42 \times 10^{-5}\) (b) \(1.42 \times 10^{-7} ;\) (c) \(1.77 \times 10^{-5} ;\) (d) \(6.15 \times 10^{4}\) (e) none of these.

A saturated aqueous solution of \(o\) -nitrophenol, \(\mathrm{HOC}_{6} \mathrm{H}_{4} \mathrm{NO}_{2},\) has \(\mathrm{pH}=4.53 .\) What is the solubility of \(o\) -nitrophenol in water, in grams per liter? $$\begin{aligned} &\mathrm{HOC}_{6} \mathrm{H}_{4} \mathrm{NO}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+-\mathrm{OC}_{6} \mathrm{H}_{4} \mathrm{NO}_{2}\\\ &&\mathrm{p} K_{\mathrm{a}}=7.23 \end{aligned}$$

You are asked to prepare a 100.0 mL sample of a solution with a pH of 5.50 by dissolving the appropriate amount of a solute in water with \(\mathrm{pH}=7.00 .\) Which of these solutes would you use, and in what quantity? Explain your choice. (a) \(15 \mathrm{M} \mathrm{NH}_{3}(\mathrm{aq}) ;\) (b) \(12 \mathrm{M} \mathrm{HCl}(\mathrm{aq})\) (c) \(\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s}) ;\) (d) glacial (pure) acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH}\)

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?

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?
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