Question

Conc. H2so4 is 98 persent by mass and has density of 1.84g/cm3. What volume of the conc. Acid is required to make 5L of 0.5 M H2so4 solution?

Answer 1

Answer:

Explanation:

Using equation. M¹=molarity=(%weight/weight×10×density)÷(Molecular weight). Substituting, %w/w as 98, density as 1.84, Molecular weight as 98 we get molarity as 18.4. Dilution eq M¹V¹=M²V². M²=0.5,V²=5lit=5000ml. Equatuating we get V¹=2500÷18.4=135.6=136ml=136cm³.

Answer 2

Answer:

136cm^3 will be the volume.

Explanation:

We know that equation of molarity is given by the formulae.

M=molarity=(%(weight/weight)×10×density)÷(Molecular weight).

We get that the %w/w as 98, again the density as 1.84,and the gram molecular weight as 98. Hence, the molarity as can be found by M1 = 98×1.84×10 / 98 =18.4.

So, we know that the dilution is having the equation as M1V1=M2V2. We know that the molarity is M2=0.5, and the volume is given as V2=5lit=5000ml. So, now on Equating we get V1=2500/18.4 which will be 135.6 or 136ml=136cm³.