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Chapter 16: Problem 76
Predict the \(\mathrm{pH}(>7,<7, \approx 7)\) of a \(\mathrm{NaHCO}_{3}\) solution.
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Which of these statements is/are true regarding a 1.0 \(M\) solution of a strong acid HA? (a) \(\left[\mathrm{A}^{-}\right]>\left[\mathrm{H}^{+}\right]\) (b) The \(\mathrm{pH}\) is 0.00 . (c) \(\left[\mathrm{H}^{+}\right]=1.0 \mathrm{M}\) (d) \([\mathrm{HA}]=1.0 \mathrm{M}\).
Write all the species (except water) that are present in a phosphoric acid solution. Indicate which species can act as a Bronsted acid, which as a Bronsted base, and which as both a Bronsted acid and a Bronsted base.
Classify each of these species as a weak or strong acid: (a) \(\mathrm{HNO}_{3}\) (b) HF, (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (d) \(\mathrm{HSO}_{4}^{-}\) (e) \(\mathrm{H}_{2} \mathrm{CO}_{3},\) (f) \(\mathrm{HCO}_{3}^{-},(\mathrm{g}) \mathrm{HCl}\) (h) HCN, (i) \(\mathrm{HNO}_{2}\)
Which of the following solutions has the highest \(\mathrm{pH} ?\) (a) \(0.40 \mathrm{M} \mathrm{HCOOH},\) (b) \(0.40 \mathrm{M} \mathrm{HClO}_{4}\) (c) \(0.40 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}\).
Prove the statement that when the concentration of a weak acid HA decreases by a factor of 10 , its percent ionization increases by a factor of \(\sqrt{10}\). State any assumptions.
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