Could someone please answer this question urgently, please answer all parts, will like and rate highly

The ionic compound ammonium sulphate is an important fertilizer. Aqueous solutions of ammonium sulphate and sodium hydroxide react according to the following equation: (NH4)2SO4(aq)+2NaOH(aq)2NH3(g)+Na2SO4(aq)+2H2O(l) (a) (i) Write the full ionic equation for this reaction ( 2 marks) (ii) Write the net ionic equation for the reaction in part (i) and identify the Brnsted-Lowry conjugate acid-base pairs. (4 marks) (b) A 3.00g sample of fertilizer containing ammonium sulphate was made up to 250.0cm3 of aqueous solution. A 25.0cm3 sample of this solution was added to an excess of sodium hydroxide solution and the ammonia gas produced passed into a solution of 50.0cm3 of 0.100moldm3 hydrochloric acid. The residual acid was then titrated with 0.100moldm3 potassium hydroxide; 25.4cm3 of KOH was required to achieve an end point. (i) Write an equation for the reaction of ammonia gas with hydrochloric acid. (2 marks) (ii) Write an equation for the reaction of hydrochloric acid with potassium hydroxide. (2 marks) (iii) What amount of HCl was present in the 50.0cm3 of 0.100molm3 hydrochloric acid before the ammonia gas was passed through it? (1 mark) (iv) How many moles of HCl remained in the 50.0cm3 of 0.100moldm3 hydrochloric acid after the ammonia gas was passed through it? (4 marks) (v) Thus determine the number of moles of HCl that were used in the reaction with ammonia. (2 marks) (vi) Use your answers to part (i) and (v) above to deduce the number of moles of ammonia formed from 25.0cm3 of diluted sample of fertilizer. (1 mark) (vii) Thus calculate the amount of ammonium sulphate in the 25.0cm3 of diluted sample of fertilizer. (2 marks) (viii) What amount ammonium sulphate, in moles, was present in the 3.00g sample of fertilizer? (2 marks) (ix) What is the percentage by mass of ammonium sulphate in the fertilizer? Mt((NH4)2SO4)=132.1