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342g of 20% by mass of Ba(OH)2 solution (sp. g-0.57)is reacted with 1200ml of 2M HNO3. If the final density of the solution is same as that of pure water then the molarity of the ion in resulting solution which decides the nature of the above solution is : 1)0.25M 2)0.5M 3)0.888M?
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342g of 20% by mass of Ba(OH)2 solution (sp. g-0.57)is reacted with 12...
Ba(OH)2 Mass is 342 gr.
171gr is 1Mole
342gr is x
x=2 Moles
100% ------ 2moles
20% ....x
x=20*2/100=0.4moles
Ba(OH)2 Total moles 2*0.4=0.8
HNO3 Molarity is 2M
Total moles is M=n*1000/v
n=2*1200/1000=2.4moles
Total excess moles is acidic=2.4-0.8=1.6
Total volume of Ba(OH)2 is
d=w/v
v=342/0.57=600ml
HNO3 volume is 1200
total volume is 600+1200=1800
M=n*1000/v
M=1.6*1000/1800
M=0.88M
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Most Upvoted Answer
342g of 20% by mass of Ba(OH)2 solution (sp. g-0.57)is reacted with 12...

Calculation of Molarity of Ba(OH)2:
- Given mass of Ba(OH)2 solution = 342g, concentration = 20%
- Mass of Ba(OH)2 in solution = 0.20 * 342g = 68.4g
- Moles of Ba(OH)2 = 68.4g / (171.34g/mol) = 0.399 moles
- Volume of solution = 342g / 0.57g/mL = 600mL

Reaction of Ba(OH)2 with HNO3:
- Moles of HNO3 = 1200mL * 2M = 2.4 moles
- Ba(OH)2 + 2HNO3 -> Ba(NO3)2 + 2H2O
- Since 1 mole of Ba(OH)2 reacts with 2 moles of HNO3, all Ba(OH)2 will react.

Final Volume of Solution:
- Volume of Ba(OH)2 solution = 600mL
- Volume of HNO3 = 1200mL
- Total volume = 1800mL = 1.8L

Calculation of Molarity of Resulting Solution:
- Moles of Ba(NO3)2 in solution = 0.399 moles
- Molarity of Ba(NO3)2 = 0.399 moles / 1.8L = 0.222M

Determination of Ion's Molarity:
- Since Ba(NO3)2 dissociates into 3 ions (Ba2+ and 2NO3-), the molarity of ions = 3 * 0.222M = 0.666M

Therefore, the molarity of the ion in the resulting solution, which decides the nature of the solution, is 0.666M. This is not one of the options provided, so the closest option is 0.5M (option 2).
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342g of 20% by mass of Ba(OH)2 solution (sp. g-0.57)is reacted with 1200ml of 2M HNO3. If the final density of the solution is same as that of pure water then the molarity of the ion in resulting solution which decides the nature of the above solution is : 1)0.25M 2)0.5M 3)0.888M?
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342g of 20% by mass of Ba(OH)2 solution (sp. g-0.57)is reacted with 1200ml of 2M HNO3. If the final density of the solution is same as that of pure water then the molarity of the ion in resulting solution which decides the nature of the above solution is : 1)0.25M 2)0.5M 3)0.888M? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about 342g of 20% by mass of Ba(OH)2 solution (sp. g-0.57)is reacted with 1200ml of 2M HNO3. If the final density of the solution is same as that of pure water then the molarity of the ion in resulting solution which decides the nature of the above solution is : 1)0.25M 2)0.5M 3)0.888M? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 342g of 20% by mass of Ba(OH)2 solution (sp. g-0.57)is reacted with 1200ml of 2M HNO3. If the final density of the solution is same as that of pure water then the molarity of the ion in resulting solution which decides the nature of the above solution is : 1)0.25M 2)0.5M 3)0.888M?.
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