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What is the ph of a solution which is 0. 025 m in weak base and 0. 039 m in the conjugate weak acid ( a = 7. 1 × 10−6)?

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The pH of the solution is 4.96.

pH measures the amount of hydrogen and hydroxide ions in a solution and shows how acidic or alkaline it is.

Weak bases are the solutions to substances that do not dissociate completely in water. Conjugate acids are the product formed by the base and have a difference of one proton.

Using the base dissociation constant, Ka

pKa can be calculated as,

[tex]pKa = - log (Ka)[/tex]

       [tex]= - log (7.1 * 10^-6)[/tex]

       [tex]= 5.15[/tex]

0. 025 M in the weak base and 0. 039 M in the conjugate weak acid.

Therefore, a weak base and its conjugate acid are present in equal proportions in buffer solution. As we are aware, the Henderson-Hasselbalch equation can be used to determine the pH of a buffer solution that comprises a weak base and its conjugate acid.

[tex]pH = pK + log [\frac{A^-}{HA} ]\\[/tex]

     [tex]= 5.15 + log( \frac{0.025}{0.037})[/tex]

     [tex]=5.15 + log 0.64[/tex]

     [tex]=5.15-0.19[/tex]

     [tex]=4.96[/tex]

Therefore, the pH of the solution is 4.96.

Learn more about pH here:

https://brainly.com/question/22390063

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