If 8.7 g of butanoic acid, c4h8o2, is dissolved in enough water to make 1.0 l of solution, what is the resulting ph? a table with ka values can be found here.

Question

George

Chemistry

1 May, 04:57

If 8.7 g of butanoic acid, c4h8o2, is dissolved in enough water to make 1.0 l of solution, what is the resulting ph? a table with ka values can be found here.

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Answers (1)

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Tasha · Answer 1

Hello! Such questions are answered by using concept from chemical equilibrium and pH formulas. First, you are required to find the concentration of H + or H3O + ions at concentration by using chemical equilibrium secondly you will calculate pH for particular H + concentration by using - log [H+] formula. Below the equation shows the reaction of butanoic acid with water producing butyrate and hydronium ions. Initially when the reaction is at time = 0 no H3O + is produced, then, reaction starts and equilibrium is attained at which unknown (x) amount of H3O + is formed. This unknown concentration is calculated as shown below (i don't know much maths so, i use online calculator). When concetration of H3O + is in hand then you can simply calculate pH.

Also, before starting the calculation you should find out Molarity of given acid by following method,

Molarity = moles : dm³

Molarity = (mass : M. Mass) : dm³

M. Mass of Butyric acid = 88 g/mol

So, Molarity = (8.7 g : 88 g/mol) : 1 dm³

Molarity = 0.0988 mol/dm³