Tell only one difference between a potentiometric acid-base titration and a conv

Question

Tell only one difference between a potentiometric acid-base titration and a conventional acid-base Titration? B) Tell the difference between equivalence point and endpoint in an acid-base titration? C) Having 21.44 mL of 0.1250 M NaOH neutralizes 25.00mL of an unknown monoprotic acid solution. Determine the concentration of the unknown acid solution? D) Having the value of pH is a 0.1500M weak monoprotic acid solution is 2.00. Find the Ka of the Acid? E) Having the pH at the half-equivalence point is 3.15 in an acid-base titration. Find is the Ka of the acid? F) Find are the components of an acid-base buffer? What do these buffers do?

Explanation / Answer

A)

pontentiometric acid base titration = require voltimeter, will have a change in current measurement whereas the coventional titration requiers a change in pH so the indicator Changes color (visual)

B)

equivalence point: the point in which acid = base ONLY

endpoint : the point in which we assume the equivalence point is achieved, but it is measured via indirect method such as indicator color change

C)

M1*V1 = M2*V2

21.44*0.125 = M2*25

M2 = 21.44*0.125 /25 = 0.1072 M of acid

D)

HA <-> H+ + A-

Ka = [H+][A-]/[HA]

[H+] = 10^-pH = 10^-2

[A-] = [H+] = 10^-2

[HA] = 0.15 - 10^-2

Ka = (10^-2)^2 / (0.15 - 10^-2) = 0.0007142

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