The equivalent weight of an acid is equal to
- AMolecular weight $\times$ acidity
- BMolecular weight $\times$ basicity
- CMolecular weight / basicity
- DMolecular weight / acidity
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$8 \ g$ of a metal reacted with oxygen to form $9 \ g$ of its oxide. What is the weight (in $g$) of the metal required to react with $8 \ g$ of hydrogen? $(H=1.0)$
The amount of $K_2Cr_2O_7$ (equivalent weight $49.04$) required to prepare $100 \ mL$ of its $0.05 \ N$ solution is ........ $g$.
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View SolutionThe equivalent mass of an element $X$ is $9$. If the vapor density of its chloride salt is $66.75$,determine the valency of element $X$.
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View SolutionCalculate the molar mass of naturally occurring argon from the data given in the following table:
Isotope Molar Mass $(g \ mol^{-1})$ Abundance $^{36}Ar$ $35.96755$ $0.337 \%$ $^{38}Ar$ $37.96272$ $0.063 \%$ $^{40}Ar$ $39.9624$ $99.600 \%$
| Isotope | Molar Mass $(g \ mol^{-1})$ | Abundance |
| $^{36}Ar$ | $35.96755$ | $0.337 \%$ |
| $^{38}Ar$ | $37.96272$ | $0.063 \%$ |
| $^{40}Ar$ | $39.9624$ | $99.600 \%$ |
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View SolutionAssuming chlorine element has two isotopes as $Cl^{35}$ and $Cl^{37}$ with their percentage abundance as $25\%$ and $75\%$ respectively. Find the average atomic weight.
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