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Chapter 45: Problem 11
To 2 significant figures, predict the \(\mathrm{pH}\) of a \(1.00\) molar solution of \(\mathrm{NaBr}\). Explain your reasoning carefully.
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Indicate which of the following are potential acids, potential bases, or both (potential acid and potential base). a) \(\mathrm{Al}^{3+}\) b) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) c) \(\mathrm{HPO}_{4}{ }^{2-}\) d) \(\quad \mathrm{F}^{-}\) e) \(\mathrm{NH}_{4}^{+}\) f) \(\mathrm{H}_{2} \mathrm{O}\)
\(\mathrm{HNO}_{3}\) is considered to be the weakest of the strong acids. Explain why the conjugate bases of all strong acids do not produce basic solutions when dissolved in water.
Describe how to determine the value of \(K_{\mathrm{b}}\) for a base-given the value of \(K_{\mathrm{a}}\) for its conjugate acid.
For each of the following, describe the common features: a) all \(K_{\mathrm{a}}\) expressions b) all \(K_{\mathrm{b}}\) expressions c) all \(K_{\mathrm{a}} \times K_{\mathrm{b}}\) products
Provide an expression relating \(K_{\mathrm{w}}\) to \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) of a conjugate acid-base pair.
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