Redox Reactions as the Basis for Titrations

How many grams of potassium dichromate are required to oxidise $20.0 \mathrm{g}$ of ${\mathrm{Fe}}^{2+}$ in ${\mathrm{FeSO}}_4$ to ${\mathrm{Fe}}^{3+}$ if the reaction is carried out in an acidic medium ? (Molar mass of ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ and ${\mathrm{FeSO}}_4$ are $294$ and $152$ respectively)

Round off your answer to the nearest integer.

Reaction of ${\mathrm{Br}}_2$ with ${\mathrm{Na}}_2{\mathrm{CO}}_3$ in aqueous solution gives sodium bromide and sodium bromate with evolution of ${\mathrm{CO}}_2$ gas. The number of sodium bromide molecules involved in the balanced chemical equation is 

How many moles of iodine are liberated when $2$ moles of potassium permanganate react with potassium iodide?

Ceric ammonium sulphate and potassium permanganate are used as oxidising agents in acidic medium for oxidation of ferrous ammonium sulphate to ferric sulphate. The ratio of number of moles of cerium ammonium sulphate required per mole of ferrous ammonium sulphate to the number of moles of ${\mathrm{KMnO}}_4$ required per mole of ferrous ammonium sulphate is

${\mathrm{MnO}}_4^{-}$ ions are reduced in acidic condition to ${\mathrm{Mn}}^{2+}$ions whereas they are reduced in neutral condition to ${\mathrm{MnO}}_2$. The oxidation of $25 \mathrm{mL}$ of a solution $\mathrm{X}$ containing ${\mathrm{Fe}}^{2+}$ ions required in acidic condition $20 \mathrm{mL}$ of a solution $\mathrm{Y}$ containing ${\mathrm{MnO}}_4^{-}$ ions. What volume of solution $\mathrm{Y}$ would be required to oxidise $25 \mathrm{mL}$ of solution $\mathrm{X}$ containing ${\mathrm{Fe}}^{2+}$ ions in neutral condition? 

$3.92 \mathrm{g}$ of ferrous ammonium sulphate are dissolved in $100 \mathrm{mL}$ water. $20 \mathrm{mL}$ of this solution requires $18 \mathrm{mL}$ of potassium permanganate during the titration for complete oxidation. The weight of ${\mathrm{KMnO}}_4$ present in one litre of the solution is (acidic medium)

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+}$$?$

Assuming complete ionization, the same moles of the following compounds will require the least amount of acidified ${\mathrm{KMnO}}_4$ for complete oxidation? 

Number of moles of ${\mathrm{MnO}}_4^{-}$ required to oxidize one mole of ferrous oxalate completely in acidic medium will be

Consider the titration of potassium dichromate solution with acidified Mohr's salt solution using diethylamine as indicator. The number of moles of Mohr's salt required per mole of dichromate is 

The number of moles of ${\mathrm{KMnO}}_4$ needed to react with one mole of ${\mathrm{SO}}_3^{2-}$ in acidic solution is

The number of moles of ${\mathrm{KMnO}}_4$ reduced by one mole of $\mathrm{KI}$ in alkaline medium is

For decolourization of $1 \mathrm{mole}$ of ${\mathrm{KMnO}}_4$, the moles of ${\mathrm{H}}_2{\mathrm{O}}_2$ required is

${\mathrm{KMnO}}_4$ acts as an oxidising agent in alkaline medium. When alkaline ${\mathrm{KMnO}}_4$ is treated with $\mathrm{KI}$, iodide ion is oxidised to

Discuss briefly the function of the salt bridge in an electrochemical cell.

Draw a labelled diagram for the Daniel cell. Discuss its working.

Both ${\mathrm{Cr}}_2{\mathrm{O}}_7^{2–}$ (aq) and ${\mathrm{MnO}}_4^{–}$(aq) can be used to titrate ${\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)$. If in a given titration, $24.50 {\mathrm{cm}}^3$ of $0.1 \mathrm{M}$ ${\mathrm{Cr}}_2{\mathrm{O}}_7^{2–}$ were used, than what volume of $0.1 \mathrm{M}$ ${\mathrm{MnO}}_4^{–}$ solution would have been used for the same titration?

$50 \mathrm{mL}$ of an aqueous solution of ${\mathrm{H}}_2{\mathrm{O}}_2$ was reacted with excess of $\mathrm{KI}$ solution and dilute ${\mathrm{H}}_2{\mathrm{SO}}_4$. The liberated iodine required $20 \mathrm{mL} 0.1 \mathrm{N}$ ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ solution of complete interaction. Calculate the concentration of ${\mathrm{H}}_2{\mathrm{O}}_2$ in ${\mathrm{gL}}^{–1}$.

$2.48 \mathrm{g}$ of ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3.{\mathrm{xH}}_2\mathrm{O}$ was dissolved per litre of the solution. $20 \mathrm{mL}$ of this solution required $10 \mathrm{mL}, 0.01 \mathrm{M}$ iodine solution. Find out the value of x.

How many millimoles of potassium dichromate is required to oxidise $24 \mathrm{mL}$ of $0.5 \mathrm{M}$  Mohr's salt solution in acidic medium?