D is 2.00M ethanoic acid.  E is 2.00M potassium hydroxide solution.

(a) Using a 50cm\(^3\) measuring cylinder, measure 50cm\(^3\) of D and transfer the solution into plastic cup.Record the temperature T\(_1\) of the solution. Rinse the cylinder distilled water and allow to dry.

 

(b) Using the dry measuring cylinder from (a) above, measure 50cm of E. Record the temperature, T\(_2\) of the solution.

 

(c) Find the average temperature T\(_3\) of the two solutions and record the value.

 

(d) Pour the measured quantity of solution E quickly from the measuring cylinder into the plastic cup containing solution D. Stir the mixture with the thermometer. Record the highest temperature T\(_4\) attained.

(e)(i) Find the rise in temperature (T\(_4\) - T\(_3\) ad record the value 

(ii) Calculate the mass of the reaction mixture, given that during the reaction 1cm\(^3\) of the mixture weighs 1g

 

(f) From your results in (a) to (e) above, calculate the;

 (i) Heat evolved during the reaction, giving that the specific heat capacity of water is 4.2Jg\(^{-1}\)C \(^{-1}\) and using the formula; heat evolved = mass x specific heat capacity x rise in temperature

(ii) Heat of neutralization of one mole of ethanoic acid by potassium hydroxide

(g) List two sources of error in the method used for determining the heat of neutrailzation and suggest how their effect can be minimized.