Redox Reaction

A $5.0 \mathrm{~cm}^3$ solution of $\mathrm{H}_2 \mathrm{O}_2$ liberates 1.27 g of iodine from an acidified KI solution. The percentage strength of $\mathrm{H}_2 \mathrm{O}_2$ is close to

A compound $(\mathrm{X})$ when treated with $\mathrm{CuSO}_4$ solution yields a brown precipitate．On adding hypo solution the precipitate turns white．The compound $(\mathrm{X})$ is

What is the four-electron reduced form of $\mathrm{O}_2$ ?

How many electrons are needed to reduce $\mathrm{N}_2$ to $\mathrm{NH}_3 ?$

The equivalent weight of \(\mathrm{Na}_2 \mathrm{S}_2 \mathrm{O}_3(\mathrm{Gram}\) molecular weight \(=\mathrm{M})\) in the given reaction is
$$\mathrm{I}_2+2 \mathrm{Na}_2 \mathrm{~S}_2 \mathrm{O}_3=2 \mathrm{NaI}+\mathrm{Na}_2 \mathrm{~S}...

The equivalent weight of KIO\(_3\) in the given reaction is (M = molecular mass):
\(\mathrm{2Cr{(OH)_3} + 4O{H^ - } + KI{O_3} \to 2CrO_4^{2 - } + 5{H_2}O + KI}\)

Oxidation states of Cr in K2Cr2O7 and CrO5 are respectively

N2H4 and H2O2 show similarity in

A given amount of Fe2+ is oxidised by x mol of \(MnO_4^ -\) in acidic medium. The number of moles of \(C{r_2}O_7^{2 - }\) required to oxidise the same amount of Fe2+ in acidic medium is

What will be the normality of the salt solution obtained by neutralising x mL y (N) HCl with y mL x(N) NaOH, and finally adding (x + y) mL distilled water

You are supplied with 500 mL each of 2N HCl and 5N HCl. What is the maximum volume of 3M HCl that you can prepare using only these two solutions?

0.126 g of an acid is needed to completely neutralise 20 mL 0.1 (N) NaOH solution. The equivalent weight of the acid is