Analyzing SO42- and PO43- in Aqueous Solution

[leena19]

Homework Statement

An aqueous solution containing SO₄^2- and PO₄3- is provided.
Using this solution,dil.HNO₃ and dil NaOH only,outline a method to determine the concentration of SO₄^2- and PO₄^3- in the sample

Homework Equations

n/a

The Attempt at a Solution

Well,I'm not really sure how to do this 'cos I'm not very sure of the reactions.Anyway this is what I think,
first, find the initial volume of the solution.next we have to find the no. of moles of each ion present, to find the concentration.
To find the no. of moles,
we add excess dilute NaOH to the sample,then we get 2 colourless solutions of Na₂SO₄ and Na₃PO₄.
To this solution we then add,dil nitric acid,Im thinking one would give a gas and one wouldn't.The one that gives out a gas contains sulphate ions,
3Na₂SO₄ + 6HNO₃$$\rightarrow$$3SO₂+6NaNO₃+3H2O
Is the above equation correct?I know that a sulphite gives SO2 with an acid but does a sulphate also give the same products?

 

[chemisttree]

Don't think about generating a gas... think about the pKa of the two acids (one with a sulfate counterion and the other with a phosphate). How can you use titration to solve this problem?

 

[leena19]

Sulphuric acid is a strong acid,whereas phosphuric acid is a relatively weak acid ,so... the Ka of sulphuric is much higher than that of phosphuric acid,which means the pKa is lesser for sulphuric than for phosphuric?
And umm...are the two acids that you're referring to, the ones that we get after adding nitric acid to their Na salts ?or is it only after adding dil.HNO3 to the (initial) given solution of sulphate and phosphate ions?

 

[chemisttree]

Yep. Now devise the experiment...

 

[leena19]

Sulphuric acid is a strong acid,whereas phosphuric acid is a relatively weak acid ,so... the Ka of sulphuric is much higher than that of phosphuric acid,which means the pKa is lesser for sulphuric than for phosphuric?
And umm...are the two acids that you're referring to, the ones that we get after adding nitric acid to their Na salts ?or is it only after adding dil.HNO3 to the (initial) given solution of sulphate and phosphate ions?

Yep. Now devise the experiment...

I'm sorry,do you mean,we get phosphuric and sulphuric acid after we add HNO3 to the original solution?
SO₄^2- +2 HNO₃$$\rightarrow$$H2SO4 + 2NO₃^-

PO₄^3- + 3HNO₃$$\rightarrow$$H3PO4 + 3NO₃^-

Either way,
For the titration part,this is what I think,
Taking a known volume of the acid solution,( say 25cm3?) into a titration flask ,add few drops of phenolphthalein as an acid-base indicator,we titrate this using a known concentration of NaOH in the burette(say C).
but what happens now?
i know the reactions occur as follows,
NaOH + H2SO4 $$\rightarrow$$ Na2SO4 + H2O

3NaOH + H3PO4 $$\rightarrow$$ Na3PO4 + 3H2O
But what happens at the endpoint?
I know that when titrating with Na2CO3,there are 2 end points,with methyl orange as indicator,but does this apply here too ,for phosphuric acid?If so I don't know how and I can't help but feel like I 'm overthinking it.
Need some help here.please...
Thank you.