College Chemistry

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I need help with this question!!

a sample of pure KHP weighing .8097g dissolved in water and titrated with 40.25 mL of NaOH solution. The same NaOH solution was used to titrate a solution of a weak diprotic acid H2X. A sample of 0.18694g of the weak acid was first dissolved in water in a 100 mL volumetric flask creating a solution of 100.00 mL. A 25.00 mL portion of this solution was tuitrated with the sodium hydroxide solution. The titration required 28.02 mL of the basic solution. What is the molar mass of the weak acid H2X?

I know that the KHP and the NaOH have a 1:1 mole ratio, and then using that you can substitute it to the formula H2X+NaOh=Na2X+H2O, and then make a IRF table...? PLEASE help!!!

• College Chemistry - ,

the species of H3o+ can be called which of the following?

• College Chemistry - ,

Emily there are two reactions of H2X with NaOH ,as of what I've learned..

H2X+NaOH ---> NaHX + H2O

when there's excess NaOH,
H2X+ 2NaOH ---> Na2X +2H2O

• College Chemistry - ,

First find the moles of H2X with the help of the NaOH moles.Now you get the moles of H2X in 25ml.Multiply it by 4 to find the moles in 100ml.

Find the concentration of NaOH with the given data in the titration of KHP.

Find the molar mass of H2X by dividing the no.of H2X moles by the given mass of H2X

n=m/M)

n=no.of moles
m=given mass
M=molar mass