Question

A solution contains 410.3 g of h2so4 per litre

Answer 1

Molar mass of H2SO4:

= 1x2 + 32 + 16x4

= 98g/mol


Number of moles = Given mass/Molar mass

                             = 410.3/98

                             = 4.19 moles


Molarity =  Number of moles per litre



Molarity of the solution = 4.19M

Answer 2

Answer:

Step-by-step explanation:

Quantity of H2SO4 = 410.3g (Given)

One liter of solution weights = Density = 1243g  (Given)

Temperature = 20° C (Given)

Since, 410.3 g of the solution is H2SO4 then the rest of the weight will be -

= 1243 - 410

= 833 g ( which must be water)  

Molar mass -

H = 2 x 1= 2  

S = 1 x 32=32  

O = 4 x 16= 64

Thus, the molar mass of H2SO4 = 98.078 g/mol  ( 64+32+2)

Moles of H2SO4 = 410.3 g/ 98.078 = 4.183  

Now, m = moles solute / Kg solvent

= 4.183 / 0.833

= 5.027

Thus, the molarity of the solution is 5.027.