Answer:
We know
\[m=\frac{{{x}_{B}}\times
1000}{(1-{{x}_{B}}){{m}_{A}}}\] (i)
\[{{x}_{B}}=\] Mole fraction of solute
= 0.04
\[{{m}_{A}}=\]
Molar mass of solvent = 18
Putting
these values in Eqn. (i), we get
\[m=\frac{0.04\times
1000}{(1-0.04)\times 18}=2.31\]
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