Question

you want to titrate a 0.10 l of 0.20 m naoh. However, you are given a 0.50 l solution of h3po4 of unknown concentration. It takes 0.25 l solution of 0.25 L solution of 0.25 m Ca(oh)2 to neutralize the H3Po4 solution. Find the concentration of the h3po4 solution and then calculate how many litres of the original h3po4 solution is needed to fully neutralize the naoh solution

Answer 1

Qale or DATE S Lelution 0.10 lite of 0.20 M Naion_ 0.50 litre of unknown H₂Pou solution 0.25 litre of 0.25 M Calt), solutions Wed to completely neutralize this Hapou Molarity defination - It su defined as the no. of Now moles of Salute' in 1 litre seleffonat - I litse 0.25M Cdotis falution have a 0.25 Male 0.95_life folution contain = 0d 5x0.25 — of Goн, CaCOH)2 +2H₂PO4 = 0.0625 moles of Cloty (az flow, 16H2O Balanced chemical equation from this equation we com see that . 2 mole of H₂ Pou reacts with 3 male of Caloty 3 mole of CaOH react, with a moleff H₂P04 t - Imole of Castly will react with of male 0.0625 mole of CalHjg deact with or neutrilze _ * 0.0625 = 0.042 Molero Hz.POCA It means o.042 males of H₂PO4 present in 6.50 litet Solution of 43 Pou Solution typen -0.50 litre & contain 0.042 Males of H₂ pou 1 litre will have a 0.049 0.084 males 6.50 of 43 POL This Malarity of ty for solution ite 0.089 M .

DATE: Non tilation with NaOhne 3 Na oH f H₂ pou Na₃PO4 + 30 Concentsation of H.pou solution 0.084 M Concentration Non Solution Q20M - Volume used No OH solution - 2.10 litre Volume required of M₂ Pou solution ? for a.20 M solution of Nach I litre of NaOH solution have 0.20 moles of elocitne will have = 0.20x010-_0.02 Mala ---of Naotte according to balanced equation e-meloof H3f04-hentized by 3moleg Naoh. Carol I 3 mole of NaOH neutraze = Imole of H₂PO4 0.02_mole of Noofl_will noutaize- xorog 1 01007 moter for 0.084 M solution of Hylow of H₂ply 0.084 molo of H₂ pon = I lite Rootmole Hapon 0.00750.083 - 0.084__ Homee volume of HzpOy solution Unfumeda 0.08? - litre. OOR3clike_HypOy solution needed