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02-26-2008, 04:48 PM
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| CHEMISTRY problem?
In titration, 25.10 mL of a monoprotic weak acid HA(aq) is neutralized with 25.10 mL of 0.502M NaOH(aq). a)Calculate the ratio of [A-] to [HA] after 12.55 mL of the 0.502 M NaOH(aq) had been added to the initial amount of HA(aq). b)At the equivalance point, you have a solution of what salt?      |
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02-26-2008, 04:48 PM
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Moles NaOH = moles HA = 0.02510 L x 0.502 =0.0126 [HA] = 0.0126 / 0.02510 L = 0.502 M Moles NaOH = 0.01255 L x 0.502 = 0.00630 Moles HA = 0.0126 - 0.00630 = 0.0063 Moles A- = 0.0063 total volume = 25.10 + 12.55 = 37.65 mL = 0.03765 L [HA] = [A-] = 0.0063 / 0.03765 =0.167 M ratio = 1 at equivalence point we have only A- |
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