Consider a different 100.0 mL sample of 1.0 M acetic acid, CH_3 COOH (K_a = 1.8

Question

Consider a different 100.0 mL sample of 1.0 M acetic acid, CH_3 COOH (K_a = 1.8 times 10^-5). You titrate this sample at 25 degree 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 (CH_3 COO^-) 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

we are titrating acitic acid. so at start of the titration more acid will be present so pH will be less than 7.

so answer = at the start of the titration the pH will be less than 7

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