Question

What is the ph of a solution which is 0. 023 m in weak base and 0. 037 m in the conjugate weak acid ( a = 7. 1 × 10^−6)?

Answer 1

The pH of a solution which is 0.023 m in weak base and 0 037 m in the conjugate weak acid whose Ka= 7.1 × 10⁻⁶ is 4.93.

pH determines the amount of hydrogen and hydroxide ions in a solution. It is the negative logarithm of hydrogen ion concentration.

Given,

Ka= 7.1 × 10⁻⁶

Weak base = 0.023M

Acid = 0.037M

Using base dissociation constant, Ka we can calculate pKa by:

pKa = -log [Ka]

pKa = -log [7.1 × 10⁻⁶]

pKa = 5.15

A weak base and its conjugate acid are present in equal proportions in buffer solution. Using the Henderson-Hasselbalch equation, we can find out the pH of a buffer solution that constitutes a weak base and its conjugate acid.

Using Henderson-Hasselbalch equation,

pH = pKa + log [Weak base / acid]

pH = 5.15 + log [0.023 / 0.037]

pH = 5.15 + log[0.6]

pH = 5.15 - 0.22

pH = 4.93

Therefore, the pH of the solution is 4.93.

Learn more about pH here, brainly.com/question/22390063

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