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Solve! - Physical and Chemical Equilibria - BITSAT

The density of NH_{4}OH solution is 0.6 g/ml. It contains 35% by weight of NH_{4}OH. Calculate the normality of the solution

  • Option 1)

    4.8N

  • Option 2)

    10N

  • Option 3)

    0.5N

  • Option 4)

    6.0N

 
Answers (1)
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As we learned in concept

Molarity -

Molarity = \frac{Moles \: of \: solute}{V\! ol.of\: solution(L)}

=> 1 mol \:of \:NH_{4}OH\rightarrow 100g\: of \: sol -

 

 for NH4OH, Molarity =normality

 

35 \% \:weight \:of \:NH_{4}OH means 35g NH4OH in  100g of solution

=> 1 mol \:of \:NH_{4}OH\rightarrow 100g\: of \: sol

100g\: of\: sol \rightarrow \frac{100}{0.6}=\frac{1000}{6}mol

\therefore N=M\frac{moles/equivalnts}{vol}

=\frac{1\times 1000}{1000/6}

=6N

 


Option 1)

4.8N

Option is incorrect

Option 2)

10N

Option is incorrect

Option 3)

0.5N

Option is incorrect

Option 4)

6.0N

Option is correct

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