Find the pH when 150 ml 1 M $\ce{NaOH}$ has been added to 100 ml 1 M $\ce{H3PO4}$. What I know: $$\ce{H3PO4 + NaOH -> NaH2PO4 + H2O}$$ $$\ce{NaH2PO4 + NaOH -> Na2HPO4 + H2O}$$ Finally 50 millimoles $\ce{Na2HPO4}$ and 50 millimoles $\ce{NaH2PO4}$ remains. Hence it will be =3×1+31+4×16=98 Add / Edited: 03.07.2015 / Evaluation of information: 5.0 out of 5 / number of votes: 1. 3NaOH + H3PO4 --> Na3PO4 + 3H2O b. The Questions and Answers of the total number of different kinds of buffers obtained during the titration of H3PO3 with NaOH are are solved by group of students and teacher of Class 11, which is also the largest student community of Class 11. Every 3 moles of NaOH … So for every 3 moles of NaOH, there needs to be 1 mole of H3PO4. The product of neutralisation of H3PO3 and 2NaOH will be :-H3PO3 + 2 NaOH -----> Na2H2PO3 + H2O. In this reaction 1g equivalent NaOH reacts with one mole H3PO4. When Phosphorous acid reacts with Sodium Hydroxide gives Sodium hypophosphite and Water. Should I apply acid buffer equation? pH, hydrogen ion concentration Calculator. But if it's what I think it is, here is the what I have: a. Please register to post comments. Become a Patron! I'm stuck with this question. pH calculation formula: pH = -log(1/H +) Where: H +: Hydrogen ion concentration in the solution H + concentration of acid is depended on its pKa, for strong acid like HCl, its pKa=1, thus H + concentration of 1 M HCl is also 1 M; for weak acid such as acetic acid, its pKa=0.0000175, thus H + concentration of 1 M acetic acid is: 1 * 0.0000175 = 0.0000175 M So molar mass of the acid is its equivalent mass. Сoding to search: H3PO3 + NaOH = NaH2PO3 + H2O. NaOH is monoacidic base. ChemiDay you always could choose go nuts or keep calm with us or without. 22.4g of Sodium Hydroxide Work: The balanced equation is the ratio of moles to each element. So its molar mass is same as equivalent mass. As we know that H3PO3 is a dibasic acid.