Mole ConceptHard
Question
A human patient suffering from a duodenal ulcer may show a concentration of HCl of 80 × 10−3 molar in gastric juice. If his stomach receives 3 L of gastric juice per day, how much medicine (antacid syrup) containing 2.6 g of Al(OH)3 per 100 ml must he consumes per day to neutralize the acid?
Options
A.27 ml
B.80 ml
C.240 ml
D.120 ml
Solution
3HCl + Al(OH)3 → AlCl3 + 3H2O
3 mole 78 g
∴3 × 80 × 10−3 mole $\frac{78}{3} \times 3 \times 80 \times 10^{- 3}$ = 7.8 × 0.8 g
∴ Volume of antacid syrup needed = $\frac{100}{2.6} \times (7.8 \times 0.8)$= 240 mL
Create a free account to view solution
View Solution FreeMore Mole Concept Questions
A quantity of 10 g of a mixture of C2H6 and C5H10 occupy 4480 ml at 1 atm and 273 K. The percentage of C2H6 by mass in t...Which of the following statement is correct :...An amount of 2 moles of KClO3 is decomposed completely to produce O2 gas. How many moles of butene C4H8 can be burnt com...H3PO4 (98 g mol-1) is 98% by mass of solution. If the density is 1.8 gm/ml, the molarity is...10 g of CaCO3 contains :-...