Problem: Calculate the pH at the following point in a titration of 40 mL (0.040 L) of 0.100 M barbituric acid (Ka = 9.8 × 10−5) with 0.100 M KOH.(a) no KOH added

🤓 Based on our data, we think this question is relevant for Professor Price's class at GVSU.

FREE Expert Solution

One Ka → monoprotic acid

let HA → barbituric acid


Equilibrium reaction:        HA(aq) + H2O(l)  A-(aq) + H3O+(aq) 


Step 1: Construct an ICE chart for the reaction.


Step 2: Write the Ka expression.

Ka=productsreactantsKa=[A-][H3O+]HA

Solids and liquids are not included in the expression



Step 3: Calculate the equilibrium concentrations.

Ka=xx0.100-x9.8×10-5=x20.100-x

[HA]initialKa>500; ignore -x

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Problem Details

Calculate the pH at the following point in a titration of 40 mL (0.040 L) of 0.100 M barbituric acid (Ka = 9.8 × 10−5) with 0.100 M KOH.

(a) no KOH added

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Acid Strong Base Titrations concept. You can view video lessons to learn Weak Acid Strong Base Titrations. Or if you need more Weak Acid Strong Base Titrations practice, you can also practice Weak Acid Strong Base Titrations practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Price's class at GVSU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.