Question

If a buffer is composed of 34. 63 ml of 0. 139 m acetic acid and 36. 50 ml of 0. 182 m sodium acetate, how many ml of 0. 100 m hcl can be added before the buffer capacity is reached?

Answer 1

The volume is the product of the molar concentration and the moles of the substance. The volume of hydrochloric acid that can be added to the buffer is 0.066 L.

What is a buffer?

A buffer is a constant solution with a proton or hydrogen ion concentration with an acid, base, or salt dissolved in them.

The chemical reaction between hydrochloric acid and sodium acetate is given as,

HCl + CH₃Coo-Na → CH₃CooH + NaCl

From above the initials moles of acetic acid are given as,

Moles = molarity × volume

= 0.139 M × 0.0346 L

=  0.0048 moles

The initials moles of sodium acetate are given as,

M = 0.182 M × 0.0365 L

= 0.0066 moles

As it is known that the ratio of the buffer capacity is 10 for sodium acetate and acetic acid so,

Moles sodium acetate ÷ Moles Acetic acid = 10

(0.0066 moles + X) ÷ (0.0048 moles - X)  = 10

Here, X is the moles of HCl and is calculated as,

0.0066 moles + X = 0.048 moles - 10X

11 X = 0.048 ÷ 0.0066

11 X = 7.27

X = 0.66 moles  

The volume of 0.100 HCl with 0.66 moles is:

Volume = moles × molarity

= 0.100 × 0.66

= 0.066 L

Therefore, 0.066 L of 0.100 M HCl is required to reach the buffer capacity.

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