Question
Asked Dec 9, 2019
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Enough of a monoprotic weak acid is dissolved in water to produce a 0.0164 M solution. The pH of the resulting solution is
2.54. Calculate the Ka for the acid.
Ka =
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Enough of a monoprotic weak acid is dissolved in water to produce a 0.0164 M solution. The pH of the resulting solution is 2.54. Calculate the Ka for the acid. Ka =

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Expert Answer

Step 1

An acid dissociation constant which is denoted by ‘Ka’ can be defined as the quantitative measure of the strength of a given acid in the solution.

 

Step 2

The pH of a given solution can be defined as the measure of the molar concentration of the hydrogen ions present in the solution and is a measure of its basicity or the acidity. The mathematical formula is as follows:

 

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pH=-log[H*]

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Step 3

The pH of the resultant solution is given to be 2.54.

The concentration of the resultant solution is giv...

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pH=-log[H"] 2.54=-log[H*] [H]=0.00288M

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