Click to Chat

1800-1023-196

+91-120-4616500

CART 0

• 0

MY CART (5)

Use Coupon: CART20 and get 20% off on all online Study Material

ITEM
DETAILS
MRP
DISCOUNT
FINAL PRICE
Total Price: Rs.

There are no items in this cart.
Continue Shopping
`        Commercially available sulphuric acid contains % 91 acid by mass and has a density of 1.83 g ML a ) calculate the molarity of the solution b ) volume of concentrated acid required to prepare 3.5 L of 0.50 M H2SO4`
2 years ago

Arun
23330 Points
```							Dear student 91 % acid by mass means 91 g acid in 100 g solution.Density = 1.83 g/mLVolume of solution = mass/density  = 91/1.83  = 49.73 mLMolar mass sulpuric acid, H2SO4  = 2 x 1 + 32 + 4 x 16 = 98 g/molNumber of moles of sulphuric acid = mass/molar mass  = 91/98  = 0.93Molarity = number of moles/ volume of solution in litres  = 0.93/0.0497  = 18.71 MApplying,M1V1= M2V218.71 x V = 0.5 x 3.5  V = 0.093 L    = 93 mLThus, 93 ml of concentrated acid is required to prepare 3.5L of 0.50 M H2SO4  RegardsArun (askIITians forum expert)
```
2 years ago
Think You Can Provide A Better Answer ?

## Other Related Questions on Physical Chemistry

View all Questions »

### Course Features

• 731 Video Lectures
• Revision Notes
• Previous Year Papers
• Mind Map
• Study Planner
• NCERT Solutions
• Discussion Forum
• Test paper with Video Solution

### Course Features

• 141 Video Lectures
• Revision Notes
• Test paper with Video Solution
• Mind Map
• Study Planner
• NCERT Solutions
• Discussion Forum
• Previous Year Exam Questions