Question 11 (0.75 points) Consider a different 100.0 mL sample of 1.0 M acetic a

Question

Question 11 (0.75 points) Consider a different 100.0 mL sample of 1.0 M acetic acid, CH3COOH (Ka = 1.8 x 10.5). You titrate this sample at 25°C by gradually adding 0.50 mol/L NaOH solution Which of the following statements will be true about this titration? At the equivalence point, the concentration of acetate ions (CH3Coo) will be the same as the concentration of acetic acid at the start of the titration (i.e. 1.0 M). To reach the half-equivalence point, we must add a total of 200.0 mL of NaOH At the equivalence point, a small amount of acetic acid will be present since acetate is a weak base. At the start of the titration, the pH will be less than 7 When all of the acetic acid has been neutralized, the pH will be equal to 7

Explanation / Answer

The answer is D

at the start of the titration ,PH will be lessthan 7.

for weak acids,

[H+] = square root of KaxC

[H+] = sqaure root of (1.8x10^-5x1.0)

[H+] = 4.24x10^-3

-log(H+) = -log(4.24x10^-3)

PH=2.37.

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