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Chapter 14: Problem 112

Arrange the following \(0.10 M\) solutions in order from most acidic to most basic. See Appendix 5 for \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) values. \(\mathrm{CaBr}_{2}, \quad \mathrm{KNO}_{2}, \quad \mathrm{HClO}_{4}, \quad \mathrm{HNO}_{2}, \quad \mathrm{HONH}_{3} \mathrm{ClO}_{4}\).

Short Answer

Expert verified
The order of the given solutions from most acidic to most basic is: \(\mathrm{HClO}_4\), \(\mathrm{HNO}_2\), \(\mathrm{HONH}_3 \mathrm{ClO}_4\), \(\mathrm{CaBr}_2\), \(\mathrm{KNO}_2\).

Step by step solution

01

Identify acidic and basic compounds

We have to identify the acidic and basic nature of each compound: 1. CaBr2: Neutral 2. KNO2: Basic 3. HClO4: Acidic (strong acid) 4. HNO2: Acidic (weak acid) 5. HONH3ClO4: Acidic (weak base + strong acid)
02

Comparing acidic strengths

We need to compare the acidic strengths of HClO4, HNO2, and HONH3ClO4. We know that HClO4 is a strong acid, so it will have the lowest pH compared to the weak acidic solutions. Comparison of weak acids HNO2 and HONH3ClO4 can be done based on the Ka values: - HNO2: Ka = \(5.1 \times 10^{-4}\) - HONH3ClO4: Ka (NH4+) = \(5.6 \times 10^{-10}\) HNO2 has a higher Ka value (larger acidic dissociation constant); thus, it is more acidic than HONH3ClO4.
03

Comparing basic strengths

Now, we will compare the basic strengths of KNO2 and CaBr2. Since CaBr2 is neutral and KNO2 is a basic solution, KNO2 will be more basic.
04

Arrange solutions

Arrange the solutions from most acidic to most basic based on the comparisons of their acidic and basic strengths: 1. HClO4 (strong acid) 2. HNO2 (weak acid with higher Ka) 3. HONH3ClO4 (weak acid with lower Ka) 4. CaBr2 (neutral) 5. KNO2 (basic) Therefore, the order from most acidic to most basic is: \(\mathrm{HClO}_4\), \(\mathrm{HNO}_2\), \(\mathrm{HONH}_3 \mathrm{ClO}_4\), \(\mathrm{CaBr}_2\), \(\mathrm{KNO}_2\).

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Most popular questions from this chapter

Identify the Lewis acid and the Lewis base in each of the following reactions. a. \(\mathrm{Fe}^{3+}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q)\) b. \(\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{OH}^{-}(a q)\) c. \(\mathrm{HgI}_{2}(s)+2 \mathrm{I}^{-}(a q) \rightleftharpoons \mathrm{HgI}_{4}{ }^{2-}(a q)\)

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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. \(\mathrm{BF}_{3}(g)+\mathrm{F}^{-}(a q) \rightleftharpoons \mathrm{BF}_{4}^{-}(a q)\)
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