Question

What volume of concentrated aquies sulphuric acid which is 98% H2SO4by mass and has density of 1.84gml-1 is required to prepare 10lof 0.2m.H2SO4 solution

Answer 1

Answer:

Volume of acid required to make one litre of 0.1M H_2SO_4H2SO4

solution is 5.5 ml.

Explanation: Given: H_2SO_4H2SO4 is labelled as 98% by weight means 98 gram of H_2SO_4H2SO4 is dissolved in 100 g of solution.

To calculate the moles, we use the equation:

Density of solution= 1.80 g/ml

Now we have to calculate the volume of solution.

Density=\frac{Mass}{Volume}Density=Volume Mass

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

Density mass = 1.80g/ml 100g =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}Molarity= Vs n×1000

where,

n= moles of solute

V_sV s = volume of solution in ml

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

Molarity= 55.5ml 1×1000 =18M

According to the neutralization law,

M_1V_1=M_2V_2M1

V1 =M2

V2 18\times V_2= 0.1\times 1000ml18×V2 =0.1×1000ml.....(1L=1000ml)

V_2=5.5mlV2 =5.5ml