Question

What is the molarity of Sulphuric acid solution that had density = 1.84 at 35'celcius and contains 98% by weight
​

Answer 1

Answer:

as the given H2SO4 is 98%by wt, hence

100g solution contains 98g H2SO4 by mass

now density d=(m/v) ∴v=(m/d)

here, d=1.84g/c.c. m=100g, v=?

∴v=(100/1.84)mL=

 again molarity=

here weight taken W=98g, molecular weight of H2SO4 (M)=98g/mol,

volume (V)=

putting these values we get

∴molarity=(98*1.84*1000)/(98*100)=18.4as the given H2SO4 is 98%by wt, hence

100g solution contains 98g H2SO4 by mass

now density d=(m/v) ∴v=(m/d)

here, d=1.84g/c.c. m=100g, v=?

∴v=(100/1.84)mL=

 again molarity=

here weight taken W=98g, molecular weight of H2SO4 (M)=98g/mol,

volume (V)=

putting these values we get

∴molarity=(98*1.84*1000)/(98*100)=18.4(M)

Explanation:

please mark as brainliest answer