1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

# A solution is made by mixing equal volumes of 30% by weight of H2SO4 (density = 1.218 g/mL) and 70% by weight of H2SO4 (density = 1.610 g/mL). Then which of the following statement(s) is/are correct?

A
Weight of H2O (solvent) is 133.56 g
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
Molarity of the final solution is 7.6 M
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
C
Molality of the final solution is 11.4 m
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
D
Molarity of the final solution is 5.4 M
No worries! Weâ€˜ve got your back. Try BYJUâ€˜S free classes today!
Open in App
Solution

## The correct option is C Molality of the final solution is 11.4 mSuppose that the solution contains 100 mL of each variety of H2SO4. Total volume is, therefore, 200 mL or 0.2 L Weight of 100 mL of H2SO4 solution (30%)=1.218×100 =121.8 g and weight of 100 mL of H2SO4 solution (70%) =1.610×100 =161 g Weight of H2SO4 (30%)=121.8×30100=36.54g Weight of H2SO4(70%)=161×70100=112.7 g Total weight of H2SO4 (solute) =36.54+112.7=149.24 g ∴ Weight of H2O (solvent) = weight of solution - weight of solute =(121.8+161)−149.24 =133.56 g Moles of H2SO4=149.2498=1.5228 (molecular weight of H2SO4=98) Molality=1.5228133.56×1000=11.4 m Molarity=1.52280.2=7.6 M

Suggest Corrections
1
Join BYJU'S Learning Program
Related Videos
Reactions in Solutions
CHEMISTRY
Watch in App
Join BYJU'S Learning Program