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.

A solution of ${\mathrm{H}}_2{\mathrm{O}}_2$​ is diluted to $10$ times of its initial volume. $20 \mathrm{mL}$ of this diluted solution requires $10 \mathrm{mL}$ of $0.2\mathrm{N} {\mathrm{KMnO}}_4$ for complete oxidation. The volume strength of original ${\mathrm{H}}_2{\mathrm{O}}_2$​ solution is

$10 \mathrm{mL}$ of a mixed solution of ${\mathrm{Na}}_2{\mathrm{CO}}_3$ and ${\mathrm{NaHCO}}_3$ required $2.5 \mathrm{mL}$ of $\frac{\mathrm{M}}{10} {\mathrm{H}}_2{\mathrm{SO}}_4$ when titrated with phenolphthalein as indicator. But when methyl orange was added, a second endpoint was observed on further addition of $2.5 \mathrm{mL}$ of $0.2\mathrm{M} {\mathrm{H}}_2{\mathrm{SO}}_4$. Calculate the amount of ${\mathrm{Na}}_2{\mathrm{CO}}_3$ and ${\mathrm{NaHCO}}_3$ in the one litre solution. 

$9.8 \mathrm{g}$ 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.

$1.5 \mathrm{gm}$ of $\mathrm{KI}$ is reacted with excess of ${\mathrm{KIO}}_3$ to produce ${\mathrm{I}}_2$ which is reacted with ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ in basic medium, where ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ converts to ${\mathrm{SO}}_4^{2-}$.  If the strength of ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ is $\frac{\mathrm{M}}{10}$, then the volume of ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ needed to reach equivalence point is:

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

Define titre value.

For a given reductant, ratio of volumes of $0.2\mathrm{M} {\mathrm{KMnO}}_4$ and $1\mathrm{M} {\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ in acidic medium will be

$31.26\mathrm{ml}$ of a $0.165\mathrm{M}$ solution of $\mathrm{Ca}{\left(\mathrm{OH}\right)}_2$ is required to just neutralise $25\mathrm{ml}$ of citric acid ${\mathrm{H}}_3{\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{O}}_7$. Then correct regarding this is/are

When ${\mathrm{l}}_2{\mathrm{O}}_5$ reacts with $50$ litre sample of $\mathrm{CO}$ gas, the $\mathrm{CO}$ gas converted into ${\mathrm{CO}}_2$ according to given reaction.

${\mathrm{I}}_2{\mathrm{O}}_5\left(\mathrm{s}\right)+5\mathrm{CO}\left(\mathrm{g}\right)\to 5{\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)$

The iodine distilled at this temperature and was collected in an absorber containing $10\mathrm{ml}$ of $0.025$ molar ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$. The excess hypo was back titrated with $10\mathrm{ml}$ of $0.002$ molar ${\mathrm{l}}_2$ solution. Then it is found that mass of ${\mathrm{l}}_2{\mathrm{O}}_5$ (solid) used for the reaction of sample of $50$ litre of $\mathrm{CO}$ gas is $\mathrm{a}\times {10}^{-3}$ grams. Then value of $2\mathrm{a}$ is (molar mass of ${\mathrm{l}}_2$ is$254 \mathrm{g}/\mathrm{mol}$)

$4\mathrm{mol}$ of a mixture of Mohr's salt and ${\mathrm{Fe}}_2{\left({\mathrm{SO}}_4\right)}_3$ required $400\mathrm{ml}$ of $0.5\mathrm{M}$ ${\mathrm{KMnO}}_4$ for complete oxidation in acidic medium. The mole $\%$ of Mohr's salt in the mixture is

$0.80 \mathrm{g}$ of sample of impure potassium dichromate was dissolved in water and made upto $500 \mathrm{mL}$ solution. $25 \mathrm{mL}$ of this solution treated with excess of $\mathrm{KI}$ in acidic medium and ${\mathrm{I}}_2$ liberated required $24 \mathrm{mL}$ of a sodium thiosulphate solution. $30 \mathrm{mL}$ of this sodium thiosulphate solution required $15 \mathrm{mL}$ of $\frac{\mathrm{N}}{20}$ solution of pure potassium dichromate. What was the percentage of ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ in given sample?

$0.6213 \mathrm{g}$ of sample contains an unknown amount of ${\mathrm{As}}_2{\mathrm{O}}_3$. The sample was treated with $\mathrm{HCl}$ resulting information of ${\mathrm{AsCl}}_3\left(\mathrm{g}\right)$ which was distilled into a beaker of water. The hydrolysis reaction is as follows:
${\mathrm{AsCl}}_3+2{\mathrm{H}}_2\mathrm{O}\to {\mathrm{HAsO}}_2+3{\mathrm{H}}^{+}+3{\mathrm{Cl}}^{-}$
The amount of ${\mathrm{HAsO}}_2$ was determined by titration with $0.04134 {\mathrm{MI}}_2$, requiring $23.04 \mathrm{mL}$ to reach the equivalence point. The redox products in the titration were ${\mathrm{H}}_3{\mathrm{AsO}}_4$ and $\mathrm{I}$. Find the amount of ${\mathrm{KMnO}}_4$ needed to oxidize $\mathrm{As}$ in ${\mathrm{As}}_2{\mathrm{O}}_3$ to its maximum possible oxidation state in acidic medium.

$1.2475 \mathrm{g}$ of crystalline copper sulphate was dissolved in water and excess of $\mathrm{KI}$ was added. The liberated iodine consumed $\frac{50 \mathrm{mL} \mathrm{N}}{10 {\mathrm{Na}}_2{ \mathrm{S}}_2{\mathrm{O}}_3}$ solution to reach the end point of the titration. Calculate the number of water molecules of hydration in crystalline copper sulphate salt.

Write the properties of secondary solution?

What is used as secondary standard for standardisation of $\mathrm{HCl}$?

Is $\mathrm{HCl}$ a primary standard and secondary standard explain?