All your burette readings (initial and final) as well as the size size of your pipette, must be recorded but no account of experimental procedure is required. All calculations must be done in your answer book. 

Xg of pure potassium trioxocarbonate (IV) was treated with 1dm\(^3\) of 0. 25M tetraoxosulphate (VI) acid to obtain solution A which contains excess acid. B is a solution containing 2.8g of potassium hydroxIde per 250cm\(^3\) solution.

(a) Put A into the burette and titrate with 20cm\(^3\) or 25cm\(^3\) portions of B. using methyl orange as indicator. Record the volume of your pipette. Tabulate your burette readings and calculate the average volume of acid used.

(b) From your results and the information given. Calculate the;

(i) concentration of the excess acid in A in mol dm\(^3\)

(iii) value of X. The equation for the reaction between the excess acid the potassium hydroxide is H\(_2\)SO\(_4\) + 2KOH \(\to\) K\(_2\)SO\(_4\) [H = 1. C = 12, O = 16. S = 32, K = 39]

Credit will be given for strict adherence to the instructions, for observations precisely recorded, and for accurate inferences. All tests, Observations, and inferences must be clearly entered in your answer book, in ink, at the time they are made. Carry out the following exercises on sample C.

Record your observations and identify any gases evolved 

(a) Put all of C into a test tube and add about 5cm\(^3\) of water. Shake the mixture and filter. Keep both the residue and the filtrate

(b) Divide the filtrate into two portions;

(i)  To the first portion, add a few drops of dilute trioxonitrate (V) acid followed by about 1cm\(^3\) of silver trioxonitrate (V) solution 

(ii) Add excess aqueous ammonia to the mixture in (i) above

(iii) To the second portion, add about 2cm\(^3\) of dilute sodium hydroxide solution and warm gently

(c) Add about 2cm\(^3\) of dilute hydrochloric acid to the residue from (a) above and warm gently. Filter if necessary and divide the resulting solutio into two portions.

(i) To the first portion add dilute sodium hydroxide solution in drops until it is in excess

(ii) To the second portion, add aqueus ammonia in drops until it is in excess.

(a)(i) Give one laboratory use of activated charcoal

(ii) A piece of phosphorus and some magnesium ribbon were burnt in two separate jars of oxygen. Water was then added to dissolve the product. State the action of litmus on each of the resulting solutions

(b) Give one chemical test to distinguish between CH\(_3\)CH\(_2\)OH and CH\(_3\)COOH.

(c) Describe how you would dilute accurately a solution containing 0.10 mole of the solute per dm\(^3\) of solution to 0.010M. 

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. 

Credit will be given for strict adherence to instructions, for observations precisely recorded, and for accurate inferences. All tests, observations, and inferences must be clearly entered in your answer book, in ink, at the time they are made.

Carry out the following exercises on sample F. Record your observations and identify any gases evolved. State the conclusion you draw from the result of each test.

(a) Put all of F into a beaker and add about 10cm\(^3) of water. Stir the mixture and filter. Keep both the residue and the filtrate.

(b)(i) Test the filtrate with litmus paper.

(ii) Add a few drops of the fehling's solution provided to about 2cm\(^3\) of the filtrate in a test tube. Boil the mixture.

(c) Put the residue from (a) above into a test tube and add about 5cm\(3\) of hydrochloric acid. Identify the gas evolved.

(d) To about 2cm\(^3\) of the clear solution from (c) above add dilute sodium into hydroxide solution dropwise and then in excess.

(e) From your results deduce what F is and its constituent