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Chemistry Question on Solutions

Concentrated aqueous sulphuric acid is 98% H2SO498 \% \,H _{2} SO _{4} by mass and has a density of 1.80 g. mL−11.80 \,g .\, mL ^{-1} Volume of acid required to make 11 litre of 0.1 M H2SO40.1\, M \,H _{2} SO _{4} solution is:

A

11.10 mL

B

5.55 mL

C

16.65 mL

D

22.20 mL

Answer

5.55 mL

Explanation

Solution

w2=98 g,w1=100 g,d=1.8 g mL−1w_2 = {98\, g}, w_1 ={ 100\, g}, d = {1.8\, g\, mL^{-1}}
Volume of solution=MassDensity=1001.8=55.55ML{ Volume\, of\, solution = \frac{ Mass}{Density} = \frac{100}{1.8} = 55.55 ML}
Molarity=w2×1000M2×V(in mL){Molarity = \frac{w_2 \times 1000}{M_2 \times V (in \, mL)}}
=98×100098×55.55=18 M= {\frac{98 \times 1000}{98 \times 55.55} = 18 \, M}
Now, M1V1=M2V2M_1V_1 = M_2V_2
18×V1=0.1×100018 \times V_1 = 0.1 \times 1000
⇒V1=0.1×100018=5.55 mL\Rightarrow V_1 = \frac{0.1 \times 1000}{18} = {5.55 \, mL}