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Chapter 13: Problem 20
Solution \(\mathrm{X}\) has \(\mathrm{pH}\) 11.7. Solution \(\mathrm{Y}\) has \(\left[\mathrm{OH}^{-}\right]=4.5 \times 10^{-2}\). Which solution is more basic? Which has the higher \(\mathrm{pOH}\) ?
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Consider the diprotic acid \(\mathrm{H}_{2} \mathrm{~A}\). For the first dissociation of \(\mathrm{H}_{2} \mathrm{~A}, K_{\mathrm{al}}=\) \(2.7 \times 10^{-4} .\) For its second dissociation, \(K_{\mathrm{a} 2}=8.3 \times 10^{-7} .\) What is the \(\mathrm{pH}\) of a \(0.20 \mathrm{M}\) solution of \(\mathrm{H}_{2} \mathrm{~A}\) ? Estimate \(\left[\mathrm{HA}^{-}\right]\) and \(\left[\mathrm{A}^{2-}\right]\).
Uric acid, \(\mathrm{HC}_{5} \mathrm{H}_{3} \mathrm{O}_{3} \mathrm{~N}_{4}\), can accumulate in the joints. This accumulation causes severe pain and the condition is called gout. \(K_{\mathrm{a}}\) for uric acid is \(5.1 \times 10^{-6} .\) For a \(0.894 M\) solution of uric acid, calculate (a) \(\left[\mathrm{H}^{+}\right]\) (b) \(\left[\mathrm{OH}^{-}\right]\) (c) \(\mathrm{pH}\) (d) \% ionization
For each of the following reactions, indicate the Brønsted-Lowry acids and bases. What are the conjugate acid/base pairs? (a) \(\mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{H}_{2} \mathrm{O}\) (b) \(\mathrm{HNO}_{2}(a q)+\mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{NO}_{2}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{HCHO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{CHO}_{2}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)\)
Using the Brønsted-Lowry model, write an equation to show why each of the following species produces a basic aqueous solution. (a) \(\mathrm{NH}_{3}\) (b) \(\mathrm{NO}_{2}^{-}\) (c) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\) (d) \(\mathrm{CO}_{3}{ }^{2-}\) (e) \(\mathrm{F}^{-}\) (f) \(\mathrm{HCO}_{3}^{-}\)
Butyric acid, \(\mathrm{HC}_{4} \mathrm{H}_{7} \mathrm{O}_{2}\), is responsible for the odor of rancid butter and cheese. Its \(K_{\mathrm{a}}\) is \(1.51 \times 10^{-5} .\) Calculate \(\left[\mathrm{H}^{+}\right]\) in solutions prepared by adding enough water to the following to make \(1.30 \mathrm{~L}\). (a) \(0.279 \mathrm{~mol}\) (b) \(13.5 \mathrm{~g}\)
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