A student is asked to prepare a buffer solution with the pH of 4.95, using one of the following weak acids and its conjugate base. | acid | HA | HB | HC | | :--- | :--- | :--- | :--- | | Ka | 4.7 x 10^-4 | 4.4 x 10^-6 | 5.0 x 10^-7 | Which acid and its conjugate base should the student choose? none of the three acids HA HB HC
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A buffer solution is a mixture of a weak acid and its conjugate base (or a weak base and its conjugate acid) that can resist changes in pH upon the addition of small amounts of acid or base. The effectiveness of a buffer is greatest when the pH of the solution is Show more…
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A student is asked to prepare a buffer solution at pH = 8.60 using one of the following weak acids HA (kA = 2.7 * 10^-3), HB (Ka = 4.4 * 10^-6), and HC (Ka = 2.6 * 10^-9). Which acid should you choose? Why?
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A student is asked to prepare a buffer solution at $\mathrm{pH} 8.60,$ using one of the following weak acids: $\mathrm{HA}\left(K_{\mathrm{a}}=2.7 \times 10^{-3}\right), \mathrm{HB}$ $\left(K_{\mathrm{a}}=4.4 \times 10^{-6}\right), \mathrm{HC}\left(K_{\mathrm{a}}=2.6 \times 10^{-9}\right) .$ Which acid should the student choose? Why?
A student is asked to prepare a buffer solution at pH $8.60,$ using one of the following weak acids: $\mathrm{HA}\left(K_{a}=2.7 \times 10^{-3}\right), \mathrm{HB}$ $\left(K_{\mathrm{a}}=4.4 \times 10^{-6}\right), \mathrm{HC}\left(K_{\mathrm{a}}=2.6 \times 10^{-9}\right) .$ Which acid should the student choose? Why?
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