Weak Acids & Bases; Ka for Weak Acids (Oxford AQA International A Level Chemistry)

Revision Note

Alexandra Brennan

Written by: Alexandra Brennan

Reviewed by: Stewart Hird

Acid Dissociation Constant, Ka

Weak acids

  • A weak acid is an acid that partially (or incompletely) dissociates in aqueous solutions

    • Eg. most organic acids (ethanoic acid), HCN (hydrocyanic acid), H2S (hydrogen sulfide) and H2CO3 (carbonic acid)

  • The position of the equilibrium is more over to the left and an equilibrium is established

Equilibria Dissociation of a Weak Acid, downloadable AS & A Level Chemistry revision notes
The diagram shows the partial dissociation of a weak acid in aqueous solution
  • As this is an equilibrium we can write an equilibrium constant expression for the reaction

The acid dissociation constant, downloadable AS & A Level Chemistry revision notes
  • This constant is called the dissociation constant for a weak acid, Ka, and has the units mol dm-3

  • Values of Ka are very small, for example for ethanoic acid Ka = 1.74 x 10-5 mol dm-3 

  • When writing the equilibrium expression for weak acids, the following assumptions are made:

    • The concentration of hydrogen ions due to the ionisation of water is negligible

  • The value of Ka indicates the extent of dissociation

    • The higher the value of Ka the more dissociated the acid and the stronger it is

    • The lower the value of Ka the weaker the acid

Worked Example

Write the expression for the following acids:

  1. Benzoic acid, C6H5COOH

  2. Carbonic acid, H2CO3

Answer:

WE1 Writing Ka Expressions, downloadable AS & A Level Chemistry revision notes

pKa Calculations

Calculating pH from Ka

  • The pH of weak acids can be calculated when the following is known:

    • The concentration of the acid

    • The Ka value of the acid

  • From the Ka expression we can see that there are three variables:

The acid dissociation constant, downloadable AS & A Level Chemistry revision notes
  • However, the equilibrium concentration of [H+] and [A-] will be the same since one molecule of HA dissociates into one of each ion

  • This means you can simplify and re-arrange the expression to

Ka x [HA] = [H+]2

[H+]2 Ka x [HA] 

  • Taking the square roots of each side

[H+] = √(Ka x [HA])

  • Then take the negative logs

pH = -log[H+] = -log√(Ka x [HA])

Worked Example

Calculate the pH of 0.100 mol dm-3 ethanoic acid at 298 k with a Ka value of 1.74 × 10-5 mol dm-3.

Answer:

Ethanoic acid is a weak acid which ionises as follows:

CH3COOH (aq) ⇌ H+ (aq) + CH3COO- (aq)

Step 1: Write down the equilibrium expression to find Ka

Step 2: Simplify the expression

The ratio of H+ to CH3COO- ions is 1:1

The concentration of H+ and CH3COO- ions are therefore the same

The expression can be simplified to:

Step 3: Rearrange the expression to find [H+]

Step 4: Substitute the values into the expression to find [H+]

= 1.32 x 10-3 mol dm-3

Step 5: Find the pH

pH = -log[H+]

= -log(1.32 x 10-3)

= 2.88

Using pKa

  • The range of values of Ka is very large and for weak acids, the values themselves are very small numbers

Table of Ka values

Acid

Ka / mol dm-3

methanoic acid, HCOOH

1.77 x 10-4

ethanoic acid. CH3COOH

1.74 x 10-5

benzoic acid. C6H5COOH

6.46 x 10-5

carbnonic acid, H2CO3

4.30 x 10-7

  • For this reason it is easier to work with another term called pKa

  • The pKa is the negative log of the Ka value, so the concept is analogous to converting [H+] into pH values

pKa = -logKa

  • Looking at the pKa values for the same acids:

Table of pKvalues

Acid

Ka / mol dm-3

pKa*

methanoic acid, HCOOH

1.77 x 10-4

3.75

ethanoic acid. CH3COOH

1.74 x 10-5

4.75

benzoic acid. C6H5COOH

6.46 x 10-5

4.18

carbnonic acid, H2CO3

4.30 x 10-7

6.36

*The range of pKa values for most weak acids lies between 3 and 7

Worked Example

At 298 K, a solution of 0.100 mol dm-3 ethanoic acid has a hydrogen ion concentration of 1.32 x 10-3 mol dm-3.

Calculate the Ka & pKa of the acid.

Answer:

Step 1: Write down the equation for the partial dissociation of ethanoic acid

CH3COOH (aq) ⇌ H+ (aq) + CH3COO- (aq)

Step 2: Write down the equilibrium expression to find Ka

Calculating pH, Ka, pKA & Kw equation 2

Step 3: Simplify the expression

The ratio of H+ to CH3COO- is 1:1

The concentration of H+ and CH3COO- is, therefore, the same

The equilibrium expression can be simplified to:

Calculating pH, Ka, pKA & Kw equation 3

Step 4: Substitute the values into the expression to find Ka

Calculating pH, Ka, pKA & Kw equation 4
Calculating pH, Ka, pKA & Kw equation 5

= 1.74 x 10-5

Step 5: Determine the units of Ka

Calculating pH, Ka, pKA & Kw equation 6
Calculating pH, Ka, pKA & Kw equation 7

= mol dm-3

The value of Ka is therefore 1.74 x 10-5 mol dm-3

Step 6: Find pKa

pKa = - log10Ka

= - log10 (1.74 x 10-5)

= 4.76

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Alexandra Brennan

Author: Alexandra Brennan

Expertise: Chemistry

Alex studied Biochemistry at Newcastle University before embarking upon a career in teaching. With nearly 10 years of teaching experience, Alex has had several roles including Chemistry/Science Teacher, Head of Science and Examiner for AQA and Edexcel. Alex’s passion for creating engaging content that enables students to succeed in exams drove her to pursue a career outside of the classroom at SME.

Stewart Hird

Author: Stewart Hird

Expertise: Chemistry Lead

Stewart has been an enthusiastic GCSE, IGCSE, A Level and IB teacher for more than 30 years in the UK as well as overseas, and has also been an examiner for IB and A Level. As a long-standing Head of Science, Stewart brings a wealth of experience to creating Topic Questions and revision materials for Save My Exams. Stewart specialises in Chemistry, but has also taught Physics and Environmental Systems and Societies.