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.

${\mathrm{I}}_2$ 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?

$25 \mathrm{mL}$ of a solution of ${\mathrm{Fe}}^{2+}$ ions require$32.45 \mathrm{mL}$ of $0.0153 \mathrm{M} {\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ solution. What is the molarity of the ${\mathrm{Fe}}^{2+}$ solution?

(Report the answer by multiplying the value with 100 and rounding off to three significant figures)

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 ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7=294 \mathrm{g} {\mathrm{mol}}^{-1}$]

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+}$$?$

$3.5 \mathrm{g}$ of a mixture of $\mathrm{NaOH}$ and $\mathrm{KOH}$ were dissolved and made up to $250 \mathrm{ml}. 25 \mathrm{mL}$ of this solution were completely neutralized by $17 \mathrm{mL}$ of $(\mathrm{N}/2) \mathrm{HCl}$solution. The percentage of $\mathrm{KOH}$ in mixture is:

In the reaction $\mathrm{Ca}(\mathrm{OH}{)}_2+{\mathrm{H}}_3{\mathrm{PO}}_4\cdots$ $\mathrm{Ca}$ ${}_3\left({\mathrm{PO}}_4\right)_2+{\mathrm{H}}_2\mathrm{O},$ the equivalent mass of ${\mathrm{H}}_2\mathrm{O}$ is: ($\mathrm{M}$ molecular mass)

Which compound decolourises iodine solution?

Consider the redox reaction $2{\mathrm{S}}_2{\mathrm{O}}_3^{2-}+{\mathrm{I}}_2⟶{\mathrm{S}}_4{\mathrm{O}}_6^{2-}+2{\mathrm{I}}^{-}:$

Which indicator will be most suitable for the titration of acetic acid vs $\mathrm{NaOH}$?

$25 \mathrm{ml}$  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  

Excess of acidified solution of KI was added to 8.4 mL ${\mathrm{H}}_2{\mathrm{O}}_2$. The iodine liberated needed 20 mL of 0.3 N ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ solution. What is the volume strength of ${\mathrm{H}}_2{\mathrm{O}}_2$ solution?

Find out the percentage purity of ${\mathrm{KMnO}}_4$ if $2\mathrm{g}$ impure sample of ${\mathrm{KMnO}}_4$ requires $40 \mathrm{ml}$ of $0.5 \mathrm{M}$ ferrous oxalate for complete reduction in acidic medium.