A titration is carried out and 0.04dm^3 of sulphuric acid neutralises 0.08dm^3 sodium hydroxide of concentration 1mol/dm^3. Calculate the concentration of the sulphuric acid.

The first thing to do with this titration calculation is write the balanced symbol equation for the reaction. Using the knowlege that when an acid and base react a salt and water is produced we can write:

H2SO4 (aq)+ 2NaOH (aq) ---> Na2SO4 (aq)+ 2H2(l)

From the balanced symbol equation we can see that 1 mole of H2SO4 neutralises 2 moles of NaOH

The next thing to do is calculate the number of moles of sodium hydroxide that were used up in the reaction.

We use the equation: number of moles = concentration x volume

N =    1 mol/dm3   x 0.08dm3 = 0.08 moles of NaOH

The number of moles of H2SO4 used up in the reaction is therefore half of this (0.04 moles) since we established from the symbol equation that 1 mole of H2SO4 neutralises 2 moles of NaOH.

Finally we can calculate the concentration of H2SO4 by using the equation :

concentration = number of moles/ volume

c = 0.04mol/ 0.04dm3 = 1mol/dm3
 

VA
Answered by Victor A. Chemistry tutor

4033 Views

See similar Chemistry GCSE tutors

Related Chemistry GCSE answers

All answers ▸

Describe the differences in properties between diamond and graphite.


Describe and Explain the trend in Volatility of Group 7 Elements


Ethanol, CH3CH2OH, can be converted into a carboxylic acid with two carbon atom. Name the carboxylic acid formed from ethanol and draw its structure. Show all bonds between atoms.


What is the empirical formula of a compound with the following composition by mass, 48.0g C, 4.0g H and 48.0g O?


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

MyTutor is part of the IXL family of brands:

© 2025 by IXL Learning