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
1 answer:
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 = (p
+ logC)
pH = (1.8× + log0.05)
pH = [1.8× + (-1.30)]
pH = (1.8× -1.30)
pH = -0.64
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Answer:
8
Explanation:
Oxidation:
Reduction:
We have to equalise the number of moles of electrons gained and lost in a redox reaction in order to get a balanced reaction.
Hence we have to multiply the oxidation reaction throughout by 6.
and adding the two half-reactions we obtain:
Still the total charge and number of oxygen is not balanced.
Since the reaction takes place in acidic conditions, we will add required number of H+ to the appropriate side to balance the charge and add half the amount of H2O to balance the hydrogen atoms.
We add 14 H+ on LHS and 7H2O on RHS to obtain:
Sum of coefficients of product cations = 6+2 = 8