A solution of ethanoic acid in water has a concentration of 3 g/dm^3. Given that the pKa of ethanoic acid is 4.76, calculate the pH of this solution.
Key facts to be noted by student:
Molar mass of ethanoic acid = 60 g/mol.
pKa = -log(Ka)
pH =-log([H+])
Concentration of acid solution = 3/60 = 0.05 moldm-3
ka = [H+]2 / [CH3COOH] therefore
[H+]2 = 10-4.76 / 0.05 --> [H+] = 0.0186 moldm-3
ph = -log(0.0186) ---> pH =1.73
TC
Related Chemistry A Level answers
All answers ▸20cm3 of 0.5moldm-3 of HCL is diluted by adding 15cm3 of water. This diluted solution is titrated against a 0.3moldm-3 solution of NaOH. What is the volume of the NaOH in cm3 required to reach the endpoint of the titration?
Predict the boiling points (lowest to highest) of Butan-1-ol, 2-methylpropane and Butane
Describe the trend in ionisation energies down group 1.
State the relative charge and relative mass of a proton, of a neutron and of an electron. In terms of particles, explain the relationship between two isotopes of the same element. Explain why these isotopes have identical chemical properties.