Question 15.9: Finding the Percent Ionization of a Weak Acid Find the perce...
Finding the Percent Ionization of a Weak Acid
Find the percent ionization of a 2.5 M HNO_{2} solution.
| To find the percent ionization, you must find the equilibrium concentration of H_{3}O^{+}. Follow the procedure in Example15.5, shown in condensed form here. | HNO_{2}(aq) + H_{2}O(l) \xrightleftharpoons[]{}H_{3}O^{+}(aq) + NO_{2}^{-}(aq)
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| K_{a} = \frac{[H_{3}O^{+}][NO_{2}^{-}]}{[HNO_{2}]} = \frac{x^{2}}{2.5 – \cancel{x}} (x is small) 4.6× 10^{-4} =\frac{ x^{2}}{2.5} x = 0.034 Therefore, [ H_{3}O{+} ] = 0.034 M. |
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| Use the definition of percent ionization to calculate it. (Since the percent ionization is less than 5%, the x is small approxi-mation is valid.) | % ionization = \frac{[H_{3}O^{+}]_{equil}}{[HA]_{init}}× 100% = \frac{0.034 \cancel{M}}{2.5 \cancel{M}}× 100% = 1.4% |
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