Calculate the ph of the solution formed when 3.5 g of impure NaOH (98.7 purity) is dissolved in water and is made up to 100cm3 and then 25cm3 of 0.35 mol dm3 of diprotic acid is added
I calculated the moles of the diprotic acid and NaOH but I don’t know what to do after What would represent the diprotic acid
I'm stuck on another question again. Calculate the ph of the solution formed when 3.5g of impure NaOH ( 98.7 purity) is disolved in water and is made up to 100cm3 and then 25cm3 of 0.35 mol dm3 of diprotic acid us added i calculated the moles of the diprotic acid and NaOH but i don't know what to do after. what would represent the diprotic acid?
I'm stuck on another question again. Calculate the ph of the solution formed when 3.5g of impure NaOH ( 98.7 purity) is disolved in water and is made up to 100cm3 and then 25cm3 of 0.35 mol dm3 of diprotic acid us added i calculated the moles of the diprotic acid and NaOH but i don't know what to do after. what would represent the diprotic acid?
I'm stuck on another question again. Calculate the ph of the solution formed when 3.5g of impure NaOH ( 98.7 purity) is disolved in water and is made up to 100cm3 and then 25cm3 of 0.35 mol dm3 of diprotic acid us added i calculated the moles of the diprotic acid and NaOH but i don't know what to do after. what would represent the diprotic acid?
You could represent the diprotic acid as H2X
Then your equation becomes:
2NaOH + H2X ==> Na2X + 2H2O
So that 2 mol of sodium hydroxide reacts with 1 mol of acid.