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calculate the ph of the following two buffer solutions: (a) 1.0 m ch3coona/2.0 m ch3cooh. (b) 0.1 m ch3coona/0.2 m ch3cooh. which is the more effective buffer? a. 1.0 m ch3coona/2.0 m ch3cooh b. 0.1 m ch3coona/0.2 m ch3cooh

Sagot :

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pH of (a) = 5.081 and  pH of (b) = 4.479. The effective buffer is  1.0M CH3COONa / 2.0 m CH3COOH.

What is buffer solution?

Buffer Solution is a water-based solvent-based solution composed of a weak acid and its conjugate base, or a weak base and its conjugate acid.

We know that,

pH = pKa + log[salt] / [acid]

For  1.0M CH3COONa / 2.0 m CH3COOH

Given,

[Salt] = CH3COONa = 1.0M

[Acid] = CH3COOH = 2.0M

pKa of CH3COOH = 4.78

Subsituting the values,

pH = 4.78 + log[1.0] / [2.0]

pH = 4.78 + 0.3010

pH = 5.081

For  0.1M CH3COONa / 0.2M CH3COOH

Given,

[Salt] = CH3COONa = 0.1M

[Acid] = CH3COOH = 0.2M

Subsituting the values,

pH = 4.78 + log[0.1] / [0.2]

pH = 4.78 + (-0.3010)

pH = 4.479

The effective buffer is  1.0M CH3COONa / 2.0 m CH3COOH because the higher the concentrations, the bigger the total buffer capacity.

To know more about buffer solutions, check out:

https://brainly.com/question/27371101

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