$0.126 \ g$ of an acid requires $20 \ mL$ of $0.1 \ N$ $NaOH$ for complete neutralization. The equivalent weight of the acid is:

An alloy of metals $X$ and $Y$ weighs $12 \ g$ and contains atoms $X$ and $Y$ in the ratio of $2:5$. The percentage of metal $X$ in the alloy is $20$ by mass. If the atomic mass of $X$ is $40$,what is the atomic mass of metal $Y$ (in $amu$)?

Assuming 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.

The weight of a molecule of the compound $C_{60}H_{122}$ is

An element,$X$ has the following isotopic composition:
$^{200}X: 90\%$,$^{199}X: 8.0\%$,$^{202}X: 2.0\%$
The weighted average atomic mass of the naturally occurring element $X$ is closest to......$amu$.

If $0.228 \, g$ of silver salt of a dibasic acid gave a residue of $0.162 \, g$ of silver on ignition,then the molecular weight of the acid is: