Volumetric Analysis

The reaction of  $H_{2}S$ with   $H_2{O}_2$ is an example of _____________ reaction

The reaction of ${\mathrm{H}}_2\mathrm{S}$ with ${\mathrm{H}}_2{\mathrm{O}}_2$ is an example of _____________ reaction.

$9.8 \mathrm{g}$ of ${\mathrm{FeSO}}_4{\left({\mathrm{NH}}_4\right)}_2{\mathrm{SO}}_4·{\mathrm{xH}}_2\mathrm{O}$ was dissolved in $250 \mathrm{mL}$ of its solution. $20 \mathrm{mL}$ of this solution required $20 \mathrm{mL}$ of ${\mathrm{KMnO}}_4$ solution, containing $3.53 \mathrm{g}$ of $90\%$ pure ${\mathrm{KMnO}}_4$ dissolved per litre. Calculate $\mathrm{x}$.

Round-off the answer to the nearest integer.

The volume used for a definite amount of unknown reagent at its equivalence point is known as _____.

Define titre value.

The $\mathrm{n}$ factor for dichromate ion in a redox reaction with Mohr's salt in an acidic medium is

${\mathrm{I}}_2$ obtained from $0.1 \mathrm{mol}$ of ${\mathrm{C}\mathrm{u}\mathrm{S}\mathrm{O}}_4$ required $100 \mathrm{ml} \text{of} 1 \mathrm{M}$ hypo solution, hence, mole percentage of pure $\mathrm{C}\mathrm{u}\mathrm{S}{\mathrm{O}}_4$ is

What mass of ${\mathrm{N}\mathrm{a}}_2{\mathrm{S}}_2{\mathrm{O}}_3.5{\mathrm{H}}_2\mathrm{O}$ is needed to make $500 \mathrm{c}{\mathrm{m}}^3$ of $0.200 \mathrm{N}$ solution for the reaction : $\mathrm{ }{2\mathrm{S}}_2\mathrm{ }{\mathrm{O}}_3^{2-}+\mathrm{ }{\mathrm{I}}_2\mathrm{ }⟶\mathrm{ }{\mathrm{S}}_4\mathrm{ }{\mathrm{O}}_6^{2-}\mathrm{ }+\mathrm{ }2{\mathrm{I}}^{-}$

${\mathrm{KMnO}}_4$ reacts with $\mathrm{KI}$, in basic medium to form ${\mathrm{I}}_2$ and ${\mathrm{MnO}}_2$ . When $250 \mathrm{ml}$ of $0.1 \mathrm{M} \mathrm{KI}$ solution is mixed with $250 \mathrm{ml}$ of $0.02 \mathrm{M} {\mathrm{KMnO}}_4$ in basic medium, what are the number of moles of ${\mathrm{I}}_2$ formed?

$0.1 \mathrm{N}{ \mathrm{K}}_2{\mathrm{C}}_2{\mathrm{O}}_4·3{\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4·4{\mathrm{H}}_2\mathrm{O}$ solution reacts completely with $20\mathrm{ml} 0.05\mathrm{M}$ of ${\mathrm{KMnO}}_4$ solution in acidic medium. Another sample of same solution of ${\mathrm{K}}_2{\mathrm{C}}_2{\mathrm{O}}_4. 3{\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4· 4{\mathrm{H}}_2\mathrm{O},$ having same volume is titrated with $\frac{1}{8}\mathrm{M}$ $\mathrm{NaOH}$ solution, then find volume of $\mathrm{NaOH}$ solution (in ml) required. [Give your answer as sum of digit and Fill OMR sheet]

The volume (in $\mathrm{mL}$ ) of $0.1 \mathrm{N} \mathrm{NaOH}$ required to neutralise $10 \mathrm{mL}$ of $0.1 \mathrm{N}$ phosphinic acid is __________ .

Consider titration of $\mathrm{NaOH}$ solution versus $1.25 \mathrm{M}$ oxalic acid solution. At the end point following burette readings were obtained.
(i) $4.5 \mathrm{ml}.$ (ii) $4.5 \mathrm{ml}.$ (iii) $4.4 \mathrm{ml}.$ (iv) $4.4 \mathrm{ml}$ (v) $4.4 \mathrm{ml}$
If the volume of oxalic acid taken was $10.0 \mathrm{ml}.$ then the molarity of the $\mathrm{NaOH}$ solution is ________ $\mathrm{M}$. (Rounded-off to the nearest integer)

$0.4 \mathrm{g}$ mixture of $\mathrm{NaOH}, {\mathrm{Na}}_2{\mathrm{CO}}_3$ and some inert impurities was first titrated with $\frac{\mathrm{N}}{10}\mathrm{HCl}$ using phenolphthalein as an indicator, $17.5 \mathrm{mL}$ of $\mathrm{HCl}$ was required at the end point. After this methyl orange was added and titrated. $1.5 \mathrm{mL}$ of same $\mathrm{HCl}$ was required for the next end point. The weight percentage of ${\mathrm{Na}}_2{\mathrm{CO}}_3$ in the mixture is_______ (Rounded-off to the nearest integer)

The volume, in $\mathrm{mL},$ of $0.02 \mathrm{M} {\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ solution required to react with $0.288 \mathrm{g}$ of ferrous oxalate in acidic medium is ________. (Molar mass of $\mathrm{Fe}=56 \mathrm{g} {\mathrm{mol}}^{-1}$)

A $20.0 \mathrm{mL}$ solution containing $0.2 \mathrm{g}$ impure ${\mathrm{H}}_2{\mathrm{O}}_2$ reacts completely with $0.316 \mathrm{g}$ of ${\mathrm{KMnO}}_4$ in acid solution. The purity of ${\mathrm{H}}_2{\mathrm{O}}_2(\mathrm{in} \%)$ is (mol. wt. of ${\mathrm{H}}_2{\mathrm{O}}_2={34}^{\text{'}}$ mole wt. of ${\mathrm{KMnO}}_4=158$)

Define "neutralisation".

In a titration experiment, $10 \mathrm{mL}$ of an ${\mathrm{FeCl}}_2$ solution consumed $25 \mathrm{mL}$ of a standard ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ solution to reach the equivalent point. The standard ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ solution is prepared by dissolving $1.225 \mathrm{g}$ of ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ in $250 \mathrm{mL}$ water. The concentration of the ${\mathrm{FeCl}}_2$ solution is closest to

[Given : molecular weight of ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7=294 \mathrm{g} {\mathrm{mol}}^{-1}$]

When $\left({\mathrm{NH}}_2{\mathrm{CH}}_2\mathrm{COOH}.\mathrm{HCl}\right)$ is treated with $\mathrm{NaOH},\mathrm{pH}$ at first half equivalence point is $2.4$ and the $\mathrm{pH}$ at second half equivalence point is $9.6$. The $\mathrm{pH}$ at first equivalence point is -

The concentration of ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3.5{\mathrm{H}}_2\mathrm{O}$ solution in grams per litre is $\mathrm{y}$, $10 \mathrm{mL}$ of which just de-colourised $15 \mathrm{mL}$ of $\frac{\mathrm{N}}{20}$ iodine solution, calculate $\frac{\mathrm{y}}{4.65}$ value?