What quantity of ammonium sulphate is necessary for the production of ammonia gas sufficient to neutralize a solution containing $$292$$ g of HCl?
Let, the amount of $$(NH_{4})_{2}SO_{4}$$ needed is $$x$$ g. Then, $$\displaystyle \frac{x}{132/2}=\frac{292}{36.5}$$.Hence, $$\mathrm{x}=528$$ g.
Open in App Suggest Corrections 0 Text Solution 272 g403 g528 g1056 g Answer : C Solution : 1 moles of `NH_(3)` neutralizes one mole of HCl , Now, moles of `Hcl = (292)/(36.5) = 8` <br> `rArr` Moles of `NH_(3)` required `= 8 rArr` Moles of `(NH_(4))_(2)SO_(4)` required = 4 <br> `rArr` Mass of `(NH_(4))_(2)SO_(4)` required `= 4 xx 132 = 528 g` |