Question

40 ml of CH3COOH solution was titrated with 20 ml of 0.15 M Ca (OH) 2 solution.
The concentration of CH3COOH solution is ...
A. 0.1
B. 0.15
C. 0.2
D. 0.25
E. 0.30

Answer 1

Explanation:

You are dealing with a neutralization reactionthat takes place between acetic acid, CH3COOH, a weak acid, and sodium hydroxide, NaOH, a strong base.

Now, the pH of the resulting solution will depend on whether or not the neutralization is completeor not.

If the neutralization is not complete, more specifically if the acid is not completely neutralized, you will have a buffer solution that will contain acetic acid and its conjugate base, the acetate anion..

It's important to note that at complete neutralization, the pH of the solution will not be equal to 7. Even if you neutralize the weak acid completely, the solution will be left with its conjugate base, which is why you can expect its pH to be greater than 7.

So, the balanced chemical equation for this reaction is - I'll show you the ionic equation

CH3COOH(aq]+OH−(aq]→CH3COO−(aq]+H2O(l]

Notice that 1 mole of acetic acid will react with 1mole of sodium hydroxide, shown here as hydroxide anions, OH−, to produce 1 mole of acetate anions, CH3COO−.

Use the molarities and volumes of the two solutions to determine how many moles of each you're adding

c=nV⇒n=c⋅V

nacetic=0.20 M⋅25.00⋅10−3L=0.0050 moles CH3COOH

and

nhydroxide=0.10 M⋅40.00⋅10−3L=0.0040 moles OH−

Since you have fewer moles of hydroxide anions, the added base will be completely consumed by the reaction.

As a result, the number of moles of acetic acid that remain in solution will be

nacetic remaining=0.0050−0.0040=0.0010 moles

The reaction will also produce 0.0040 moles of acetate anions.

This means that you're now dealing with a buffer. Use the Henderson-Hasselbalch equation to find its pH

pH=pKa+log([conjugate base][weak acid])

Use the total volume of the solution to find the new concentrations of the acid and of its conjugate base

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