1.

A metal weighing 0.43 g was dissolved in 50 mL of 1 N H_(2)SO_(4). The unreacted H_(2)SO_(4) required 14.2 mL of 1 N NaOH for neutralisation. Calculate the equivalent weight of the metal?

Answer»

Solution :`H_(2)SO_(4)" LEFT unreacted "-=NaOH" reacted= 14.2 mL of 1 N"`
`therefore"1 N "H_(2)SO_(4)" reacted with the metal "=(50-14.2)mL=35.8mL`
`"35.8 mL of 1 N "H_(2)SO_(4)="35.8 MILLIEQUIVALENTS"`
If E is the EQUIVALENT wt. of the metal, milliequivalents of the metal reacted `"=(0.43)/(E)xx1000=(430)/(E)`
As metal and the acid will react in equivalent amounts,
`(430)/(E)=35.8 or E=(430)/(35.8)=12.01`


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