$0.16 \ g$ of dibasic acid required $25 \ mL$ of decinormal $NaOH$ solution for complete neutralization. The molecular weight of the acid will be:

$2 \ g$ of metal carbonate is neutralized completely by $100 \ mL$ of $0.1 \ N$ $HCl$. The equivalent weight of metal carbonate is:

In a reaction,the ferrous $(Fe^{2+})$ ion is oxidized to ferric $(Fe^{3+})$ ion. The equivalent weight of the ion in the above reaction is equal to:

$A$ metal $M$ (specific heat $0.16 \ J \ g^{-1} \ K^{-1}$) forms a metal chloride with $65\%$ chlorine present in it. The formula of the metal chloride will be:

Naturally occurring boron consists of two isotopes with atomic masses $10.01 \ (I)$ and $11.01 \ (II)$. The average atomic mass of natural boron is $10.81$. Find the percentage abundance of isotopes $(I)$ and $(II)$ respectively.

$74.5 \ g$ of a metallic chloride contains $35.5 \ g$ of chlorine. What is the equivalent mass of the metal?