Redox Reactions and Titration

${\mathrm{KMnO}}_4$ acts as an oxidising agent in alkaline medium. When alkaline ${\mathrm{KMnO}}_4$ is treated with $\mathrm{KI}$, iodide ion is oxidised to ${{\mathrm{IO}}_{\mathrm{X}}}^{-}$. The value of $\mathrm{X}$ is _____.

How many $\mathrm{ml}$ of $0.125$ $\mathrm{M}$ ${\mathrm{Cr}}^{3+}$ must be reacted with $12.00 \mathrm{ml}$ of $0.200 \mathrm{M}$ ${{\mathrm{MnO}}_4}^{-}$ if the redox products are ${\mathrm{Cr}}_2{{\mathrm{O}}_7}^{2-}$and ${\mathrm{Mn}}^{2+}$$?$

$25 \mathrm{ml}$  of household bleach solution was mixed with $30 \mathrm{ml}$ of  $0.50$ $\mathrm{M}$ $\mathrm{KI}$ and $10 \mathrm{ml}$ of  $4 \mathrm{N}$ acetic acid. In the titration of the liberated iodine, $48 \mathrm{ml}$ of $0.25 \mathrm{N}$ ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ was used to reach the end point. The molarity of the household bleach solution is  

$5 \mathrm{mL}$of $8 \mathrm{N}$ nitric acid, $4.8 \mathrm{mL}$ of $5 \mathrm{N}$ hydrochloric acid and a certain volume of $17 \mathrm{M}$ sulphuric acid are mixed together and made up to $2 \mathrm{L}$. $30 \mathrm{mL}$ of this acid mixture exactly neutralise $42.9 \mathrm{mL}$ of sodium carbonate solution containing one gram of ${\mathrm{Na}}_2{\mathrm{CO}}_3.10{\mathrm{H}}_2\mathrm{O}$ in $100 \mathrm{mL}$ of water. Calculate the amount in grams of the sulphate ions in solution. Report the answer after multiplying with 10 and round off to the nearest integer._​

Conductometric titration curve of an equimolar mixture of HCl and HCN with NaOH (aq) is

$10 \mathrm{mL} \mathrm{of} {\mathrm{H}}_2{\mathrm{O}}_2$solution on treatment with KI and titration of liberated I₂, required $10 \mathrm{mL} \mathrm{of} 1\mathrm{N}$ hypo. Thus H₂O₂ is -

Acidified ${\mathrm{K}\mathrm{M}\mathrm{n}\mathrm{O}}_4$ oxidises oxalic acid to ${\mathrm{C}\mathrm{O}}_2.$ What is the volume (in litres) of ${10}^{-4}\mathrm{M}\mathrm{ }{\mathrm{K}\mathrm{M}\mathrm{n}\mathrm{O}}_4$ required to completely oxidise $0.5 \mathrm{L}$ of ${10}^{-2}$ $\mathrm{M}$ oxalic acid in acid medium?

Amount of oxalic acid present in a solution can be determined by its titration with ${\mathrm{K}\mathrm{M}\mathrm{n}\mathrm{O}}_4$ solution in the presence of ${\mathrm{H}}_2{\mathrm{S}\mathrm{O}}_4.$ The titration given unsatisfactory result when carried out in the presence of HCl because HCl

The oxidation state of chromium in the final product formed by the reaction between KI and acidified potassium dichromate solution is

A mixture of $\mathrm{FeO}$ and ${\mathrm{Fe}}_2{\mathrm{O}}_3$ is completely reacted with $100 \mathrm{mL}$ of $0.25 \mathrm{M}$ acidified ${\mathrm{KMnO}}_4$ solution. The resultant solution was then titrated with zinc dust which converted ${\mathrm{Fe}}^{3+}$ of the solution to ${\mathrm{Fe}}^{2+}$. The ${\mathrm{Fe}}^{2+}$ required $1000 \mathrm{mL}$ of $0.1 \mathrm{M} {\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ solution. Find out the percentage weight of ${\mathrm{Fe}}_2{\mathrm{O}}_3$ in the mixture.

Iodine oxidises ${\mathrm{S}}_2{\mathrm{O}}_3^{2-}$ ion to

1.2 g of a salt with its empirical formula K_xH_y(C₂O₄)_z was dissolved in 50 mL of water and its 10 mL portion required 11 mL of a 0.1 M HCl solution to reach the equivalence point. In a separate titration, 15 mL of the stock solution required 20 mL 0.2475 M KOH to reach the equivalence point. Determine the empirical formula of salt.

1 M NaOH solution was slowly added into 1000 mL of 183.75 g impure H₂SO₄ solution and the following plot was obtained. The percentage purity of  H₂SO₄ sample and slope of the curve respectively are :