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Chapter 43: Problem 4
Show that the pH reading in the model is correct (given that the hydronium ion concentration is \(5.0 \times 10^{-4} \mathrm{M}\) ) and explain why the value is not \(3.3\).
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Consider a neutral aqueous solution. a) What is \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in a neutral aqueous solution? b) What is the \(\mathrm{pH}\) of a neutral aqueous solution? c) What is the pOH of a neutral aqueous solution?
Based on the relationships given in the Information sections, what is the relationship between \(\mathrm{pH}, \mathrm{pOH}\), and \(\mathrm{p} K_{\mathrm{w} ?}\)
a) Show that \(\log \left(10^{5} \times 10^{-5}\right)=0\) without calculating a value for \(10^{5} \times 10^{-5}\). b) Identify which relationship you used from the Information to perform part a.
What is the value of each of the following expressions? a) \(\log \left(2.5 \times 10^{-5}\right)\) b) \(\log \left(2.5 \times 10^{5}\right)\) c) \(\log \left(5.0 \times 10^{-4}\right)\)
For a weak acid, HA: $$ \mathrm{HA}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{A}^{-}(\mathrm{aq}) $$ a) Write the equilibrium expression for \(K_{\mathrm{a}}\). b) Show that \(\mathrm{pH}=\mathrm{p} K_{\mathrm{a}}-\log \frac{[\mathrm{HA}]}{\left[\mathrm{A}^{-}\right]}\)
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