Ch.16 - Aqueous Equilibria: Acids & Bases
Chapter 16, Problem 143
Which would you expect to be the stronger Lewis acid in each of the following pairs? Explain. (a) BF3 or BH3
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Related Practice
Textbook Question
The hydrated cation M1H2O26
3 + has Ka = 10-4, and the
acid HA has Ka = 10-5. Identify the principal reaction in
an aqueous solution of each of the following salts, and classify
each solution as acidic, basic, or neutral.
(a) NaA
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Textbook Question
Calculate the pH and the percent dissociation of the hydrated
cation in the following solutions. See Appendix C for
the value of the equilibrium constant.
(a) 0.010 M Cr1NO323
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Textbook Question
Classify each of the following as a Lewis acid or a Lewis
base.
(e) OH-
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Textbook Question
Calculate the pH and the concentrations of all species present
(H3O+ , F-, HF, Cl-, and OH-) in a solution that contains
0.10 M HF 1Ka = 3.5 * 10-42 and 0.10 M HCl.
736
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Textbook Question
When NO2 is bubbled into water, it is completely converted
to HNO3 and HNO2:
2 NO21g2 + H2O1l2S HNO31aq2 + HNO21aq2
Calculate the pH and the concentrations of all species present
(H3O+ , OH-, HNO2, NO2
-, and NO3
-) in a solution
prepared by dissolving 0.0500 mol of NO2 in 1.00 L of
water. Ka for HNO2 is 4.5 * 10-4.
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Textbook Question
Acid and base behavior can be observed in solvents other
than water. One commonly used solvent is dimethyl
sulfoxide (DMSO), which can be treated as a monoprotic
acid 'HSol.' Just as water can behave either as an acid or a
base, so HSol can behave either as a Brønsted–Lowry acid
or base.
(b) The weak acid HCN has an acid dissociation constant
Ka = 1.3 * 10-13 in the solvent HSol. If 0.010 mol of
NaCN is dissolved in 1.00 L of HSol, what is the equilibrium
concentration of H2Sol + ?
922
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