Contact

For Study plan details

10:00 AM to 7:00 PM IST all days.

For Franchisee Enquiry

OR

or

Thanks, You will receive a call shortly.
Customer Support

You are very important to us

9321924448 / 9987178554

Mon to Sat - 10 AM to 7 PM

# 342g of 20% by mass of b a Ba(OH)2 solution (sp. gr.=0.57) is reacted with 1200 mL of 2M HNO3. If the final density of solution is same as pure water then molarity of the iron in resulting solution which decides the nature of the above solution is— (1)0.25M,(2)0.5M,(3)0.888M,(4)none of these.

Asked by patra04011965 24th May 2019, 8:52 AM
The mass of Ba(OH)2 is 342 g.
The molar mass of Ba(OH)2 is 171 gm
Hence,
1 mole of Ba(OH)2 is the molar mass of Ba(OH)is 171 gm
So, for 342 g. wil be x

We know 100% by mass is 2moles hence 20% will be x.

As given the molarity of HNO3 is 2M, So, the total moles=

Total acidic excess moles = 2.4 - 0.8 = 1.6

The total volume of Ba(OH)2 is

The volume of HNO3 is 1200ml

Hence the total volume of Ba(OH)2 = 1200+600 =1800 ml

Answered by Expert 24th May 2019, 11:02 AM
• 1
• 2
• 3
• 4
• 5
• 6
• 7
• 8
• 9
• 10

You have rated this answer 8/10