Equivalent Concept

Vapour density of a metal chloride is 66. Its oxide contains 53% metal. The atomic weight of the metal is

$1.1 \mathrm{g} {\mathrm{CH}}_3{\left({\mathrm{CH}}_2\right)}_{\mathrm{n}}\mathrm{COOH}$ was burnt in excess of air and the resultant gases $\left({\mathrm{CO}}_2+{\mathrm{H}}_2\mathrm{O}\right)$ were passed through a solution of $\mathrm{NaOH}$. The resulting solution is divided into two equal parts. One part required $75$m.e. of $\mathrm{HCl}$ for neutralisation using phenolphthalein as indicator. The other part required $100$ m.e. of $\mathrm{HCl}$ using methyl orange as indicator. Find $\mathrm{n}$.

$0.177\mathrm{g}$ of a monobasic acid required $30\mathrm{ml} \mathrm{of} \mathrm{N}/10 \mathrm{NaOH}$ solution for complete neutralization. Its molecular weight will be

The valency factor of ammonium sulphate is

The valecy factor of Aluminium sulphate is

${\mathrm{KMnO}}_4$ reacts with ${\mathrm{H}}_2{\mathrm{O}}_2$ in an acidic medium. The number of moles of oxygen produced per mole of ${\mathrm{KMnO}}_4$ is;

20 mL solution of 0.1 M ferrous sulphate was completely oxidised using a suitable oxidising agent. What is the number of electrons exchanged?

What are the number of moles of KMnO₄ that will be needed to react with one mole of ${\mathrm{SO}}_3^{2-}$ion  in acidic solution?

Molten ${\mathrm{AlCl}}_3$ is electrolysed with a current of $0.5 \mathrm{A}$ to produce $27.0 \mathrm{g}$ $\mathrm{Al}$.

How many litres of ${\mathrm{Cl}}_2$ at NTP were produced?(Report the answer in 2 significant numbers)

Upon heating a litre of a $\frac{\mathrm{N}}{2}\mathrm{HCl}$ solution, $2.675 \mathrm{g}$ of hydrogen chloride is lost and the volume of the solution shrinks to $750 \mathrm{mL}$. Calculate:

The normality of the resultant solution.(Express your answer up to three decimal places)

Find the equivalent weight of ${\mathrm{H}}_3{\mathrm{PO}}_4$, in the reaction,

$\left[\mathrm{Ca}(\mathrm{OH}{)}_2+{\mathrm{H}}_3{\mathrm{PO}}_4={\mathrm{CaHPO}}_4+2{\mathrm{H}}_2\mathrm{O}\right]$.

If $2 \mathrm{litres}$ of ammonia at $13 °\mathrm{C}$ and $0.90$ atmospheric pressure is neutralised by $134 \mathrm{ml}$ of ${\mathrm{H}}_2{\mathrm{SO}}_4$ solution, the normality value of the acid is A.

Report the value of A by multiplying with 100 and rounding off the value to two significant figures

How many gram of ${\mathrm{H}}_2\mathrm{S}$ will react with $63.2 \mathrm{g}$ of ${\mathrm{KMnO}}_4$ to produce ${\mathrm{K}}_2{\mathrm{SO}}_4$ and ${\mathrm{MnO}}_2?$ Give answer after rounding off to the nearest integer.

A certain amount of metal, whose equivalent weight is $28,$ displaces $0.7 \mathrm{litre}$ of hydrogen measured at NTP from an acid. Calculate the weight of the metal.

Give your answer to the nearest integer value after multiplying with 4.

If $6\times {10}^{-3} \mathrm{mole}$ of ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ reacts completely with $9\times {10}^{-3}$ mole of ${\mathrm{X}}^{\mathrm{n}+}$ to give ${\mathrm{XO}}_3^{-} \text{and} {\mathrm{Cr}}^{3+}$, then, the value of $\mathrm{n}$ is

The equivalent weight of an element is $4$. Its chloride has a vapour density $59.25$. Then the valency of the element is

Equivalent weight of an element is _____ proportional to its valency.