 ## Enthalpy changes involving solutions

### A coffee cup calorimeter Many reactions in we study in chemistry take place in solution, for example neutralisation of an acid using an alkali is a chemical reaction that takes place in solution. In this case the reactants and the product are the system. The water and the calorimeter are part of the surroundings. If the reactants undergo an exothermic reaction then the heat produced will heat the water and as long as the calorimeter is well insulated we can use the temperature change to calculate the enthalpy change for the reaction taking place. A simple but effective calorimeter is shown opposite.

Here a polystyrene coffee cup is used to hold the solutions that are reacting. Polystyrene is an excellent insulator but this simple calorimeter can be improved if we simply place the polystyrene cup inside another cup to further insulate the reaction and prevent heat from leaving or entering the solution. The cork lid will also prevent heat loss by evaporation if the reaction is exothermic and also prevent heat from the surrounding entering the solution if the reaction is endothermic.

### Calculating enthalpy of neutralisation

Neutralisation reactions are exothermic. When an acid and an alkali react they form a salt and water.

##### Acid(aq) + alkali(aq) → salt(aq) + water(l)

A defintion you should learn is:

The standard enthalpy of neutralisation is defined as: The enthalpy change when an acid is neutralised by a alkali or base to form one mole of water under standard conditions (298K, 100 kPa).

Consider the neutralisation reaction between the strong acid; hydrochloric and the strong alkali sodium hydroxide. HCl(aq) + NaOH(aq)

##### HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
Here the acid and alkali react in a molar ratio of 1:1. We can use the simple coffee cup calorimeter to measure the enthalpy of neutralisation here. Method.
• Rinse out a 25ml pipette using a dilute hydrochloric acid solution. Clean a second pipette but this time rinse it out using a dilute sodium hydroxide solution.
• Using a clean pipette measure out 25ml of 1M HCl and 25ml of 1M NaOH and place each of the solutions in two separate expanded polystyrene cup. Each cup should be sitting on a working magnetic stirrer.
• Using an accurate thermometer (one that measures to at least 0.10C) measure the temperature of each solution every minute for at least 5 minutes to ensure both solutions are at room temperature. Record the temperature of each solution in a table.
• Place the coffee cup containing 25ml of hydrochloric acid into another coffee cup so that you have one cup sitting inside another as shown in the diagram above. Put the calorimeter on top of a magnetic stirrer and ensure the solution is being well stirred.
• Record the temperature of the acid in a table every 30 seconds for 4 minutes.
• On the fourth minute pour the 25ml of sodium hydroxide (NaOH) into the acid. do not record the temperature at the time of mixing but start recording the temperature again at 5 minutes. Continue to record the temperature of the solution every minute for a further 10 minutes, or until the temperature reaches room temperature. Neutralisation reactions are very exothermic and can release large amounts of heat enery. We are also recording temperature changes over a fairly long period of time and despite our best efforts with insulation and using double polystyrene cups some heat loss to the surrounding will take place, especially if the reaction is very exothermic and releases large amounts of heat energy. However it is possible to compensate for SOME of this heat loss by using an extrapolation method as shown in the graph opposite.

Here you can see a set of results obtained by a student, they have plotted their results on a graph and extrapolated to find the maximum temperature reached, to try and compensate for heat loss to the surroundings:

### Example 1:

Let's use the example above to calculate the enthalpy of neutralisation when 25ml of 1M hydrochloric acid is neutralised by a 25ml of a 1M sodium hydroxide solution. Let's assume that the temperature rise in the example above was 70C. Solution -

• Total volume of solution is 50ml. The mass will be therefore be 50g, since the density of water is 1gcm3 (1ml of water has a mass of 1g). We will assume that solution formed has the same density as water.
• The specific heat capacity of water is 4.2 kJ kg-1 K-1 or 4.2 J g-1 K-1.
• Simply use the equation below to calculate the enthalpy change:
##### q = m x c x ΔT

Substituting in the values we have:
##### = 1470J or 1.47kJ

To calculate the molar enthalpy change we simply need to scale up.
First calculate the number of moles of acid used:

So :
##### = -58.8 kJ mol-1
(The answer is negative since it is an exothermic reaction).

### Example 2 - Displacement reactions.

Displacement reactions occur when a more reactive metal removes or displaces a less reactive metal from a compound or solution. Displacement reactions can be very exothermic, especially if the two metals involved are far apart in the reactivity series. For example zinc will displace copper from a copper sulfate solution according to the equation below|:

##### 1mol    1mol           1mol           1mol ### Example

50 ml of 0.75M copper sulfate solution was pipetted into a coffee cup calorimeter and the temperature was recorded every 30 seconds for 4 minutes. 5g of zinc powdered was then added to the copper sulfate solution and the temperature was recorded every 30 seconds until a maximum temperature was reached, then the temperature was recorded for a further 4 minutes. The initial temperature of the solution was 24oC and the final temperature was 540C. This reaction is slow and the student obtained the final temperatur by extrapolation as in the previous example.
Moles of copper sulfate present Moles of zinc present
Number of moles = concentration x volume
= 0.75 mol dm-3 x 50/1000
= 0.0375 mol
Number of moles = mass/Ar
=5g/65
= 0.077 mol
The zinc is in excess, which is what we need. This will ensure that the reaction goes to completion and all the copper sulfate will react. In order to calculate the enthalpy change we only take into account the mass of the solution as this is what we are measuring the temperature of.
So enthalpy change is calculated from:
##### = 6300J or 6.3kJ
To calculate the enthalpy change per mole of copper sulfate we simply scale up and use the formula below:

## Key Points

• A simple coffee cup calorimeter can used to measure enthalpy changes for reactions which take place in solutions.
• we use the equation below to calculate these enthalpy changes:
• q = m x c x ΔT
Here:
• q=the heat energy released or taken in by the system. This will obviously depend on whether the reaction is exothermic or endothermic.
• m= the mass of the substance, this is usually water. Recall that the density of water is 1g/cm3, this means that 1g of water has a volume of 1cm3 or 1ml.
• c= specfic heat capacity. For reactions taking place in aqueous solutions the specific heat capacity of water is 4.18kJK-1kg-1. This simply means taht it takes 4.18kJ of heat energy to raise 1kg of water by 1 degree Kelvin or 1 degree Celsius.
• ΔT = This is simply the change in temperataure that takes place during the reaction.
• The main source of error in the calorimeter is lilely to be heat loss to the surroundings if the reaction is exothermic. You should be able to describe how to use the extroplation method discussed above to compensate for some of this heat loss.
• You shoukld be able to Descruibe a method to measure the enthalpy change for a reaction in solution or combustion.