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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
Answered by Expert
Answer:
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
 
straight x equals 342 over 171 equals space 2 space moles
We know 100% by mass is 2moles hence 20% will be x.
 
straight x space equals space fraction numerator 20 cross times 2 over denominator 100 end fraction space 0.4 space moles
 
The space total space moles space of space Ba left parenthesis OH right parenthesis subscript 2 space equals space 2 space cross times space 0.4 space equals space 0.8
 
As given the molarity of HNO3 is 2M, So, the total moles=
 
 straight M space equals space fraction numerator straight n cross times 1000 over denominator straight V end fraction

straight n space equals space fraction numerator 2 cross times 1200 over denominator 1000 end fraction

straight n space equals space 2.4 space moles
 
 
Total acidic excess moles = 2.4 - 0.8 = 1.6
 
The total volume of Ba(OH)2 is straight d space equals space straight w over straight v
straight v space equals space fraction numerator 342 over denominator 0.57 end fraction space equals space 600 ml
 
The volume of HNO3 is 1200ml
 
Hence the total volume of Ba(OH)2 = 1200+600 =1800 ml
 
straight M space equals fraction numerator straight n cross times 1000 over denominator straight V end fraction
straight M space equals space fraction numerator 1.6 cross times 1000 over denominator 1800 end fraction
straight M space equals space 0.88 straight M
Answered by Expert 24th May 2019, 11:02 AM
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