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vivado [14]
2 years ago
6

Suppose that 25. 0 ml of 0. 10 m ch3cooh(aq) ( ka =1. 8 x 10-5) is titrated with 0. 10 m naoh(aq). (a)what is the initial ph of

the 0. 10 m ch3cooh (aq) solution?
Chemistry
1 answer:
liberstina [14]2 years ago
7 0

The initial ph of the 0. 10M ch3cooh  (aq) solution is  -0.64.

The salt sodium acetate is present at the equivalency point. It is a salt of a strong base and a weak acid. The expression "its pH" provides the information.

pH = 7 + 0.5p + 0.5logC

where C is the salt concentration. Monobasic acid is Acetic acid here.

25 ml of 0.10 M NaOH solution are needed for the titration of 25 ml of 0.10 M acetic acid.

Total volume = 25 + 25 = 50ml

The salt concentration = C = 0.10×  = 0.05

The pH for weak acid is given by,

pH = \frac{1}{2} (pK_{a} + logC)

pH =  \frac{1}{2} (1.8× + log0.05)

pH =  \frac{1}{2} [1.8× + (-1.30)]

pH =  \frac{1}{2} (1.8× -1.30)

pH = -0.64

Learn more about pH here;

brainly.com/question/15192160

#SPJ4

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