Chemistry help

Posted on 2015-12-01 07:08:00 in Chemistry by ALEXI

One beaker contains 10.0 mL of acetic acid/sodium acetate buffer at maximum buffer capacity (equal concentrations of acetic acid and sodium acetate), and another contains 10.0 mL of pure water. Calculate the hydronium ion concentration and the pH after the addition of 0.25 mL of 0.10 M HCl to each one. What accounts for the difference in the hydronium ion concentrations? Explain this based on equilibrium concepts; in other words, saying that one solution is a buffer is not sufficient. H3 O+ (aq) + C2 H3 O2 - (aq) ? HC2 H3 O2(aq) +H2 O Ka of acetic acid = 1.8 x 10-5 Acetic acid/sodium acetate buffer: Acetic acid = 0.1M, Sodium acetate = 0.1M

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