0.66 g of H3PO2 will require 'X' ml of 0.1 M NaOH for complete neutralisation. Then x =
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The value of x is 1000 mL.
Explanation:
The chemical reaction follower in neutralization of H₃PO₂ is:
H₃PO₂ + NaOH → NaH₂PO₂
The equivalent weight is given by the formula:
Equivalent weight = (Weight of acid)/(Normality × Volume)
Since, Equivalent weight = Molar mass
The molar mass of H₃PO₂ = 66
Weight of acid = 0.66 g
Normality = 0.1 M
Volume = x
66 = (0.66)/(0.1 × x)
0.1 × x = 0.66/66 = 0.01
x = 0.01/0.1 = 0.1 L
∴ X = 1000 mL
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