Question

1) Calculate the pH of a 0.026 M solution of NH4NO3. Kb of NH3= 1.8x10^-5. include both the dissociation and hydrolysis equations in the set up

2)calculate the pH of a 75 ml buffer solution containing 0.20 M of citric acid(C6H8O7, Ka= 3.2x10^-7) and 0.30 M sodium citrate. and what is the pH after adding 3.0 mlbof 1.5 M HCl to the buffer solution in that question?

3) what is the pH of 20.00 ml of 0.40 M nitrous acid( Ka= 4.0x10^-4) titrated with 10.00 ml of 0.50 M sodium hydroxide? including a balanced chemical equation.

4) will precipitate form when 0.012 M Ba(NO3)2 is combined with 0.023 M Na2SO4? Ksp of BaSO4=2.3 x10^-8.

PLEASE help me answering the 4 questions i am have a trouble working these problems out i appreciate it

Answer 1

for precipitation Q must be greater than Ksp and in this solution first we calculate Q which is greater tha Ksp i.e., precipitate forms. Thanku and have a nice day