Determine the Enthalpy of Neutralisation for the following there Acids, H2SO4, HNO3 and H2SO4

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A level coursework

Determine the Enthalpy of Neutralisation for the following there Acids, H2SO4, HNO3 andH2SO4

Introduction

Acid and bases have a very important property that is that they are able to cancel each other out when mixed together in the right proportions, this reaction is called a neutralisation reaction, which can be an exothermic reaction .

The standard enthalpy of neutralisation is the heat absorbed per mole when an acid and a base react to form water under standard conditions.

In this experiment I will be investigating the values for enthalpy of neutralisation of the three strong acids (HCl, HNO3 andH2SO4)

Scientific Background information

As explained before, neutralisation happens between an acid and a base. Neutralisation is the formation of water from hydrogen and hydroxide ions

H30+(aq) + OH-(aq) --> 2H20(aq)

According to Arrhenius' theory 'neutralisation occurs because equal mols of hydrogen ions in the acid are equal to the mols of hydroxide ions in the base so the two react completely to form water'*1.

Neutralisation of HCl and NaOH:

NaOH(aq) + HCl(aq) --> NaCl(aq) + H2O(l).

Neutralisation of HNO3 and NaOH

NaOH(aq) + HNO3(aq)