Equivalent Concept

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

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

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

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

Arsenic forms two oxides, one of which contains $65.2\%$ and the other $75.7\%$ of the element. Hence, equivalent masses of arsenic are in the ratio :

Explain Equivalent mass of element.

Carbon forms two oxides, namely carbon monoxide and carbon dioxide. The equivalent mass of which element remains constant? 

Volume ${\mathrm{V}}_1 \mathrm{mL}$ of $0.1\mathrm{M} {\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ is needed for complete oxidation of $0.678\mathrm{g} {\mathrm{N}}_2{\mathrm{H}}_4$ in acidic medium. The volume $\left(\mathrm{in} \mathrm{mL}\right)$ of $0.3 \mathrm{M} {\mathrm{KMnO}}_4$ needed for same oxidation in the acidic medium will be

In alkaline medium,${\mathrm{KMnO}}_4$ reacts as follows (Atomic weights $\mathrm{K}=39.09, \mathrm{Mn}=54.94, \mathrm{O}=16.00$)

$2{\mathrm{KMnO}}_4+2\mathrm{KOH}\to 2{\mathrm{K}}_2{\mathrm{MnO}}_4 +{\mathrm{H}}_2\mathrm{O}+\left[\mathrm{O}\right]$

Hence, its equivalent weight is

Equivalent weight of chlorine molecule in the equation is : $3{\mathrm{Cl}}_2+ 6\mathrm{NaOH} \to 5\mathrm{NaCl}+ {\mathrm{NaClO}}_3+3{\mathrm{H}}_2\mathrm{O}$

An aqueous solution of $6.3 \mathrm{g}$ of oxalic acid dihydrate is made up to $250 \mathrm{mL}$. The volume of $0.1 \mathrm{N} \mathrm{NaOH}$ required to completely neutralize $10 \mathrm{mL}$ of this solution is