Question

Concentrated aqueous sulphuric acid is 98% H2SO4 by mass and has density 1.80g/ml volume of acid required to make one litre of 0.1M H2SO4 solutions

Answer 1

By the formula M1 = density × 10 × % by mass / atomic mass
A/c to question ,,
M1 = 98×1.80×10 / 98 =18
Now from formula , M1V1 = M2V2
M1=18, V1=?, M2=0.1, V2=1L
So, V1= M2V2 / M1
V1 =0.1×1 /18 =0.0055
So
Ans is 0.0055

Answer 2

Answer: Volume of acid required to make one litre of 0.1M $H_2SO_4$ solution is 5.5 ml.

Explanation: Given: $H_2SO_4$ is labelled as 98% by weight means 98 gram of $H_2SO_4$ is dissolved in 100 g of solution.

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\textMolar mass}}=\frac{98g}{98g/mol}=1mole$

Density of solution= 1.80 g/ml

Now we have to calculate the volume of solution.

$Density=\frac{Mass}{Volume}$  

$Volume=\frac{mass}{Density}=\frac{100g}{1.80g/ml}==55.5ml$

Molarity : It is defined as the number of moles of solute present per liter of the solution.

Formula used :

$Molarity=\frac{n\times 1000}{V_s}$

where,

n= moles of solute

$V_s$ = volume of solution in ml

$Molarity=\frac{1\times 1000}{55.5ml}=18M$

According to the neutralization law,

$M_1V_1=M_2V_2$

$18\times V_2=0.1\times 1000ml$     (1L=1000ml)

$V_2=5.5ml$