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An aqueous solution of 6.3g oxalic acid dihydrate is made up to 250 ml. the volume of 0.1N NaOH req to completely neutralize 10 ml of this solution is?
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An aqueous solution of 6.3g oxalic acid dihydrate is made up to 250 ml...
Calculation of Volume of NaOH Required to Neutralize the Solution


Given:

Mass of oxalic acid dihydrate = 6.3g

Volume of solution = 250 ml

Concentration of NaOH = 0.1N

Volume of solution to be neutralized = 10 ml


Formula:

Moles of oxalic acid dihydrate = (mass of oxalic acid dihydrate) / (molar mass of oxalic acid dihydrate)

Moles of NaOH = (concentration of NaOH) x (volume of NaOH used in liters)

Moles of oxalic acid dihydrate = moles of NaOH (at equivalence point)


Calculation:

Molar mass of oxalic acid dihydrate = molar mass of oxalic acid + 2 x molar mass of water

Molar mass of oxalic acid dihydrate = (2 x 1) + (2 x 16) + 2 x [1 + (2 x 16)]

Molar mass of oxalic acid dihydrate = 126 g/mol


Moles of oxalic acid dihydrate = (6.3g) / (126 g/mol) = 0.05 mol


At equivalence point, moles of NaOH = moles of oxalic acid dihydrate

Therefore, moles of NaOH = 0.05 mol


Moles of NaOH = (concentration of NaOH) x (volume of NaOH used in liters)

Volume of NaOH used in liters = moles of NaOH / concentration of NaOH

Volume of NaOH used in liters = 0.05 mol / 0.1N = 0.5 L


Volume of NaOH used in 10 ml of solution = (0.5 L / 250 ml) x 10 ml = 0.02 ml


Therefore, the volume of NaOH required to completely neutralize 10 ml of this solution is 0.02 ml.
Community Answer
An aqueous solution of 6.3g oxalic acid dihydrate is made up to 250 ml...
Equivalent mass of C2H2O4.2H2O = 126/2 = 63 Normality of oxalic acid = 6.3/63 * 1000/250 = 0.4 N =>N1V1 = N2V2 N1 =>normality of oxalic acid V1 = volume of oxalic acid N2 =normality of sodium hydroxide V2 =volume of sodium hydroxide =>0.4 * 10 = 0.1 * V2 =>V2 = 40 ml.
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An aqueous solution of 6.3g oxalic acid dihydrate is made up to 250 ml. the volume of 0.1N NaOH req to completely neutralize 10 ml of this solution is?
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