Question
0.189 gm of an organic compound gives 0.287 g of AgCl . The $\%$ of Cl in it is?(a) $18.75 \%$(b) $37.56 \%$(c) 55.25(d) $74 \%$
Step 1
The molar mass of Ag (Silver) is approximately 107.87 g/mol, and the molar mass of Cl (Chlorine) is approximately 35.45 g/mol. Thus, the molar mass of AgCl = 107.87 g/mol + 35.45 g/mol = 143.32 g/mol. Show more…
Show all steps
Your feedback will help us improve your experience
Narayan Hari and 57 other educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
When $0.25 \mathrm{~g}$ of an organic compounds is heated with $\mathrm{HNO}_{3}$ and $\mathrm{AgNO}_{3}$ in a carius tube, it gives $0.35 \mathrm{~g}$ of silver chloride. The percentage of chlorine in the compound is (a) $36.6 \%$ (b) $45.3 \%$ (c) $34.6 \%$ (d) $54.8 \%$
In Carius method of estimation of halogens, $250 \mathrm{mg}$ of an organic compound gave $141 \mathrm{mg}$ of $\mathrm{AgBr}$. The percentage of bromine in the compound is (At. mass $\mathrm{Ag}=108 ; \mathrm{Br}=80)$ (a) $24 \%$ (b) $36 \%$ (c) $48 \%$ (d) $60 \%$
The impure $6 \mathrm{~g}$ of $\mathrm{NaCl}$ is dissolved in water and then treated with excess of silver nitrate solution. The weight of precipitate of silver chloride is found to be $14 \mathrm{~g}$. The \% purity of $\mathrm{NaCl}$ solution would be: (a) $95 \%$ (b) $85 \%$ (c) $75 \%$ (d) $65 \%$
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD