Redox titrations

In order to oxidise a mixture of 1 mole each of $\ce{FeC2O4}$, $\ce{Fe2(C2O4)3}$, $\ce{FeSO4}$ and $\ce{Fe2(SO4)3}$ in acidic medium, the number of moles of $\ce{KMnO4}$ required is

500 mL of 0.2 M $\ce{MnO4-}$ solution in basic medium when mixed with 500 mL of 1.5 M KI solution, oxidises iodide ions to liberate molecular iodine. This liberated iodine is then titrated with a standard $x$ M thiosulphate solution in presence of starch till the end point. If 300 mL of thiosulphate was consumed, then the value of $x$ is ________.

The treatment of an aqueous solution of 3.74 g of $\ce{Cu(NO3)2}$ with excess KI results in a brown solution along with the formation of a precipitate. Passing $\ce{H2S}$ through this brown solution gives another precipitate X. The amount of X (in g) is _____.

[Given: Atomic mass of H = 1, N = 14, O = 16, S = 32, K = 39, Cu = 63, I = 127]

Acidified potassium permanganate solution oxidises oxalic acid. The spin-only magnetic moment of the mangenese product formed from the above reaction is ______ B.M. (Nearest Integer)

A 2.0 g sample containing $\mathrm{MnO_2}$ is treated with HCl liberating $\mathrm{Cl_2}$. The $\mathrm{Cl_2}$ gas is passed into a solution of KI and 60.0 mL of 0.1 M $\mathrm{Na_2S_2O_3}$ is required to titrate the liberated iodine. The percentage of $\mathrm{MnO_2}$ in the sample is ______. (Nearest integer)

[Atomic masses (in u) Mn = 55; Cl = 35.5; O = 16, I = 127, Na = 23, K = 39, S = 32]

0.01 M $\mathrm{KMnO_4}$ solution was added to 20.0 mL of 0.05 M Mohr's salt solution through a burette. The initial reading of 50 mL burette is zero. The volume of $\mathrm{KMnO_4}$ solution left in the burette after the end point is ______ mL. (nearest integer)

The dark purple colour of $\mathrm{KMnO_4}$ disappears in the titration with oxalic acid in acidic medium. The overall change in the oxidation number of manganese in the reaction is :

20 mL of 0.02 M hypo solution is used for the titration of 10 mL of copper sulphate solution, in the presence of excess of KI using starch as an indicator. The molarity of $\mathrm{Cu^{2+}}$ is found to be ______ $\times10^{-2}$ M. [nearest integer]

Given : $\mathrm{2Cu^{2+}+4I^-\rightarrow Cu_2I_2+I_2}$

$\mathrm{I_2+2S_2O_3^{2-}\rightarrow2I^-+S_4O_6^{2-}}$

20 mL of 0.02 M $\mathrm{K_2Cr_2O_7}$ solution is used for the titration of 10 mL of $\mathrm{Fe^{2+}}$ solution in the acidic medium.

The molarity of $\mathrm{Fe^{2+}}$ solution is ______ $\times10^{-2}$ M. (Nearest Integer)

In the titration of $\mathrm{KMnO_4}$ and oxalic acid in acidic medium, the change in oxidation number of carbon at the end point is ______

Given below are two statements : One is labelled as Assertion A and the other is labelled as Reason R

Assertion A : Permanganate titrations are not performed in presence of hydrochloric acid.

Reason R : Chlorine is formed as a consequence of oxidation of hydrochloric acid.

In the light of the above statements, choose the correct answer from the options given below

The value of $\mathbf x$ is ____.

The value of $\mathbf y$ is ____.

To measure the quantity of $\mathrm{MnCl_2}$ dissolved in an aqueous solution, it was completely converted to $\mathrm{KMnO_4}$ using the reaction,

$$\mathrm{MnCl_2 + K_2S_2O_8 + H_2O \rightarrow KMnO_4 + H_2SO_4 + HCl} \quad \text{(equation not balanced)}.$$

Few drops of concentrated HCl were added to this solution and gently warmed. Further, oxalic acid (225 mg) was added in portions till the colour of the permanganate ion disappeared. The quantity of $\mathrm{MnCl_2}$ (in mg) present in the initial solution is ____.

(Atomic weights in g mol$^{-1}$: Mn = 55, Cl = 35.5)

25 mL of household bleach solution was mixed with 30 mL of 0.50 M KI and 10 mL of 4 N acetic acid. In the titration of the liberated iodine, 48 mL of 0.25 N $\ce{Na2S2O3}$ was used to reach the end point. The molarity of the household bleach solution is

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