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Chapter 14: Q14.3-46 E (page 830)
What do we represent when we write
\(C{H_3}C{O_2}H(aq) + {H_2}O(l) \rightleftharpoons{H_3}{O^ + }(aq) + C{H_3}CO_2^ - (aq)?\)
\(C{H_3}C{O_2}H(aq) + {H_2}O(l) \rightleftharpoons{H_3}{O^ + }(aq) + C{H_3}CO_2^ - (aq)?\) represents the dissociation of a weak acid in water.
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What two common assumptions can simplify the calculation of equilibrium concentrations in a solution of a weak base?
A \({\bf{5}}{\bf{.36 g}}\) sample of \({\bf{N}}{{\bf{H}}_{\bf{4}}}{\bf{Cl}}\) was added to \({\bf{25}}.{\bf{0}}{\rm{ }}{\bf{mL}}\) of \({\bf{1}}{\bf{.00 M NaOH}}\) and the resulting solution diluted to\({\bf{0}}.{\bf{100}}{\rm{ }}{\bf{L}}\).
(a) What is the pH of this buffer solution?
(b) Is the solution acidic or basic?
(c) What is the pH of a solution that results when \({\bf{3}}.{\bf{00}}{\rm{ }}{\bf{mL}}\) of \({\bf{0}}.{\bf{034}}{\rm{ }}{\bf{M}}{\rm{ }}{\bf{HCl}}\) is added to the solution?
Which of the following concentrations would be practically equal in a calculation of the equilibrium concentrations in a \(0.134 - M\) solution of \({H_2}C{O_3}\), a diprotic acid: \(\left( {{H_3}{O^ + }} \right),\left( {O{H^ - }} \right),\left( {{H_2}C{O_3}} \right),\left( {HCO_3^ - } \right)\left( {CO_3^{2 - }} \right)?\) No calculations are needed to answer this question.
The ionization constant for water\(({K_w})\) is\(2.9 \times 1{0^{ - 14}}\;at\;4{0^o}C\). Calculate\(\left( {{H_3}{O^ + }} \right),\left( {O{H^ - }} \right),pH,\;and\;pOH\) for pure water at \(4{0^o}C\).
The hydronium ion concentration of vinegar is approximately 4×10−3 M. What are the corresponding values of pOH and pH?
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