In this method, we are finding the concentration of sulfuric acid by volumetry.
For that the first standardization of the titrant. Since sulfuric acid is a strong acid it is better to use a strong base. Thus the given base is NaOH.
The whole titration works under the principle acidimetry and alkalimetry
The reaction between NaOH and oxalic acid is
H2C2O4(aq) + 2 NaOH (aq) --> Na2C2O4(aq) + 2 H2O (l)
That is one oxalic acid consumes 2 moles of NaOH
Given that 0.0855 g of oxalic acid took 25.28 mL of Na OH for neutralization.
Molecular weight of oxalic acid is 90.03 g/mol
Thus 25.28 mL of NaOH took 0.0855/90.03 moles of oxalic acid
25.28 mL of NaOH took 9.46 x 10-4moles of oxalic acid. Which means 25.28 mL contains twice 9.46 x 10-4moles of NaOH (since one oxalic acid consumes two NaOH molecules)
Thus 25.28 mL contains 0.001899 moles. For converting into molarity (number of moles per liter) 0.001899 x 1000/25.28 =0.075 M (molarity and normality are same for NaOH since it is monoprotic base)
Standardization of NaOH is over. Now we have to estimate the unknown sulfuric acid. Reaction between sulfuric acid and NaOH is
H2SO4(aq) + 2 NaOH (aq) --> Na2SO4(aq) + 2 H2O (l)
In this case also, one-mole sulfuric acid consumes 2 moles NaOH.
Given that 10 mL (volume (H2SO4)) of this sulfuric acid consumes 32.34 mL of NaOH (volume (NaOH))
For finding concentration
Normality (NaOH)x volume (NaOH)= Normality (H2SO4) x volume (H2SO4)
thus normality of sulfuric acid = 32.34 x 0.075/10 = 0.2425 N.
Since sulfuric acid is diprotic acid (it can react with 2 base molecules) = normality/2 = 0.2425/2
= 0.1212 M
An unknown sample of sulfuric acid was determined by the method used in this experiment. The...
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