An aqueous solution containing sulphate and phosphate ions provided.Using this solution,dil. nitric acid and dil.NaOH only,outline a method to determine the concentration of the sulphate and phosphate ions
I had posted this question on another forum and I was told to consider using titration to find the molar concentration of each ion present.
After adding dil. nitric acid to the above solution,we get 2 acids,namely phosphuric and sulphuric acid.
So.. to do the titration,this is what I thought,
Take a known volume of the acidic solution into a titraion flask and add phenolphalein as indicator.
In the burette we have a known concentration of the NaOH sol' provided to us,
Now... at the end point...this is where my problem starts,
what happens ? I know that titrating Na2CO3 with an acid gives 2 endpoints with methylorange as indicator,but is it relevant to this as well.
Does phosphuric acid act similar to Na2CO3 cause it'a weak acid just like Na2CO3 is a weak base?If so...I don't know how
On the other hand my whole method of titrating maybe completely wrong.
I'm looking for someone to guide me here.
A thorougly confused student seeking urgent help.