MCQ
A commercially sold conc. $HCl$ is $35 \% HCl$ by mass. If the density of this commercial acid is $1.46$ $g / mL$, the molarity of this solution is ....$M$
(Atomic mass : $Cl =35.5 \,amu , H =1\, amu$ )
- A$10.2$
- B$12.5$
- ✓$14.0$
- D$18.2$
✓
Answer
Correct option: C.
$14.0$
c
Let total volume $=1000 \,mL =1 \,L$
Let total volume $=1000 \,mL =1 \,L$
total mass of solution $=1460 \,g$
mass of $HCl =\frac{35}{100} \times 1460$
moles of $HCl =\frac{35 \times 1460}{100 \times 36.5}$
So molarity $=\frac{35 \times 1460}{100 \times 36.5}=14 \,M$
Need a full question paper?
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
Explore more
Similar questions
What is relation between following molecules
The crystalline form of borax has
→($A$) tetranuclear $\left[\mathrm{B}_4 \mathrm{O}_5(\mathrm{OH})_4\right]^{2-}$ unit
($B$) all boron atoms in the same plane
($C$) equal number of $s p^2$ and $s p^3$ hybridized boron atoms
($D$) one terminal hydroxide per boron atom
Among the given structure which can exhibit tautomerism ?
The product $(A)$ of given alkoxymercuration de-mercuration is
→Compound $(P)$ is
→Oxidation number of $C$ in $HNC$ is
→Which is correct
In Duma's method of estimation of nitrogen, $0.1840 \,g$ of an organic compound gave $30 \,mL$ of nitrogen collected at $287\, K$ and $758\, mm$ of $Hg$ pressure. The percentage composition of nitrogen in the compound is ...... . (Round off to the Nearest Integer). [Given : Aqueous tension at $287\, K =14 \,mm$ of $Hg$ ]
→A reaction between methyl magnesium bromide and ethyl alcohol gives
As the alkaline earth metals $($except Be$)$ tend to lose their valence electrons readily. They act as:
→