Question

According to the label on a bottle of concentrated hydrochloric acid, the contents are 36.0% HCl by mass and have a density of 1.18 g/mL.
1.What is the molarity of concentrated HCl?
2.What volume of it would you need to prepare 853 mL of 1.80 M HCl?
3.What mass of sodium bicarbonate would be needed to neutralize the spill if a bottle containing 1.75 L of concentrated HCl dropped on a lab floor and broke open?

Answer 1

1.Let the volume of solution be 1000 ml.

Mass of the solution is 1180 gm.

Mass of HCl is $36/100×1180=424.8$ gm

No of moles of $HCl =424.8/36.46=11.65 moles$

$Molarity=11.65M$ (Answer)

2.1000ml contains 1.8 mole of HCl.

1 ml contains 1.8/1000 mole of HCl.

853 ml contains $1.8×853/1000 mole=1.5354 moles$

Mass of HCl is $1.5354×36.46=55.98$ gm

Density of HCl is 1.18 g/mL.

1.18 gm has a volume of 1 ml

1 gm has a volume of 1/1.18ml

55.98 gm has a volume of 1/1.18× 55.98=47.44ml$1/1.18× 55.98=47.44ml$ (Answer)

3.$no of moles =11.65×1.75 moles=20.3875moles$

No of $Moles=20.3875moles$

Mass of $NaHCO_3=20.3875×84.007=1712.69 gm$

(Answer)