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23 Nov 2019

100 mL of a 0.2351 M solution of the weak base acetate (Ac-) istitrated to the equivalence point with a 0.1674 M solution of thestrong acid HCL. For acetic acid, (HAc) Ka=1.8 x 10^-5.

a. Find the volume of HCL required to reach the equivalencepoint.

b. Find the concentrations of Ac-, HAc, OH- and H+ at theequivalence point.

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Trinidad Tremblay
Trinidad TremblayLv2
10 Oct 2019

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Related questions

(a) 0.002 M acetic acid (HAc) (pKa = 4.7) is added to solution. Determine the final pH and [HAc] and [Ac-] in the solution?

(b) How does pH and [HAc] and [Ac-] change when 0.00035 M NaOH, a strong base, is titrated into the solution described in part (a)? Note: NaOH is added from a concentrated stock solution, so the volume change is negligible.

(c) What is the pH and [HCl] and [Cl-] when 2 mM hydrochloric acid (pKa = 0) is added to water?

(d) Discuss whether your results in (a) and (c) are consistent with our assumptions about the dissociation of weak and strong acids.

calculate the pH of a solution of 0.25 M acetic acid and 0.34 M sodium acetate before and after 0.036 M NaOH is added to the solution. Ka of HAc=1.8*10^-5

A solution is made of 10^-2.7 M sodium acetate and 10^-3.7 M NaHCO3.

a. Find the pH of this solution. Assume the solution is initally closed to the atmosphere.

b. This solution is then equilibrated with atmospheric CO2 where Pco2= 400ppm. Find the new pH after the system has reached equilibrium.

HAc= H+ + Ac- Ka, Ac= 10^-4.76

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