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Chapter 14: Q14.1-14 E (page 765)
Is the self ionization of water endothermic or exothermic? The ionization constant for water \(\left( {{K_W}} \right)\)is 2.9* \({10^{ - 14}}\)at \({40^ \circ }{\rm{C}}\)and 9.3 x \({10^{ - 14}}\)at \({60^ \circ }{\rm{C}}\)
Self ionization of water is endothermic process.
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Calculate the concentration of each species present in a \(0.010M\) solution of phthalic acid, \({C_6}{H_4}{\left( {C{O_2}H} \right)_2}\).
\(\begin{array}{*{20}{c}}{{C_6}{H_4}{{\left( {C{O_2}H} \right)}_2}(aq) + {H_2}O(l) \rightleftharpoons {H_3}{O^ + }(aq) + {C_6}{H_4}\left( {C{O_2}H} \right){{\left( {C{O_2}} \right)}^ - }(aq)}&{{K_a} = 1.1 \times 1{0^{ - 3}}} \\ {{C_6}{H_4}\left( {C{O_2}H} \right)\left( {C{O_2}} \right)(aq) + {H_2}O(l) \rightleftharpoons {H_3}{O^ + }(aq) + {C_6}{H_4}{{\left( {C{O_2}} \right)}_2}^{2 - }(aq)}&{{K_a} = 3.9 \times 1{0^{ - 6}}} \end{array}\)
Nicotine, \({C_{10}}{H_{14}}\;{N_2}\), is a base that will accept two protons \(\left( {{K_1} = 7 \times 1{0^{ - 7}},{K_2} = 1.4 \times 1{0^{ - 11}}} \right)\). What is the concentration of each species present in a \(0.050 - M\) solution of nicotine?
What do we represent when we write
\(C{H_3}C{O_2}H(aq) + {H_2}O(l) \rightleftharpoons{H_3}{O^ + }(aq) + C{H_3}CO_2^ - (aq)?\)
From the equilibrium concentrations given, calculate \({K_a}\)for each of the weak acids and \({K_b}\)for each of the weak bases.
\(\begin{aligned}(a)N{H_3}:\left( {O{H^ - }} \right) = 3.1 \times 1{0^{ - 3}}M\left( {NH_4^ + } \right) = 3.1 \times 1{0^{ - 3}}M;\left( {N{H_3}} \right) = 0.533M;\\(b)HN{O_2}:\left( {{H_3}{O^ + }} \right) = 0.011M;\left( {NO_2^ - } \right) = 0.0438M;\left( {HN{O_2}} \right) = 1.07M;\\(c){\left( {C{H_3}} \right)_3}\;N:\left( {{{\left( {C{H_3}} \right)}_3}\;N} \right) = 0.25M;\left( {{{\left( {C{H_3}} \right)}_3}N{H^ + }} \right) = 4.3 \times 1{0^{ - 3}}M;\left( {O{H^ - }} \right) = 4.3 \times 1{0^{ - 3}}M;\\(d)N{H_4} + :\left( {N{H_4} + } \right) = 0.100M;\left( {N{H_3}} \right) = 7.5 \times 1{0^{ - 6}}M;\left( {{H_3}{O^ + }} \right) = 7.5 \times 1{0^{ - 6}}M\end{aligned}\)
\(\begin{aligned}\left( {N{H_3}} \right) = 7.5 \times 1{0^{ - 6}}M\\\left( {{H_3}{O^ + }} \right) = 7.5 \times 1{0^{ - 6}}M\end{aligned}\)
Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the following equations:
\({\rm{\;(a)\;NO}}_2^ - + {{\rm{H}}_2}{\rm{O}} \to {\rm{HN}}{{\rm{O}}_2} + {\rm{O}}{{\rm{H}}^ - }\).
\({\rm{\;(b)\;HBr}} + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_3}{{\rm{O}}^ + } + {\rm{B}}{{\rm{r}}^ - }\)
\({\rm{\;(c)\;H}}{{\rm{S}}^ - } + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_2}{\rm{S}} + {\rm{O}}{{\rm{H}}^ - }\)
\({\rm{\;(d)\;}}{{\rm{H}}_2}{\rm{PO}}_4^ - + {\rm{O}}{{\rm{H}}^ - } \to {\rm{HP}}{{\rm{O}}_4}^{2 - } + {{\rm{H}}_2}{\rm{O}}\)
\({\rm{\;(e)\;}}{{\rm{H}}_2}{\rm{PO}}_4^ - + {\rm{HCl}} \to {{\rm{H}}_3}{\rm{P}}{{\rm{O}}_4} + {\rm{C}}{{\rm{l}}^ - }\)
\({\rm{\;(f)\;}}{\left( {{\rm{Fe}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_5}({\rm{OH}})} \right)^{2 + }} + {\left( {{\rm{Al}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}} \right)^{3 + }} \to {\left( {{\rm{Fe}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}} \right)^{3 + }} + {\left( {{\rm{Al}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_5}({\rm{OH}})} \right)^{2 + }}\)
\({\rm{\;(g)\;C}}{{\rm{H}}_3}{\rm{OH}} + {{\rm{H}}^ - } \to {\rm{C}}{{\rm{H}}_3}{{\rm{O}}^ - } + {{\rm{H}}_2}\)
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