Titration

$9.8 \mathrm{g}$ 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.

$25 \mathrm{mL}$ 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)

Which of the following halogen oxides is used for the estimation of carbon monoxide in automobile exhaust gases?

$0.1 \mathrm{N}{ \mathrm{K}}_2{\mathrm{C}}_2{\mathrm{O}}_4·3{\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4·4{\mathrm{H}}_2\mathrm{O}$ 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 $0.02 \mathrm{M} {\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ 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 ${\mathrm{KMnO}}_4=158$)

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

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?

$100 \mathrm{mL}$ of $0.05 \mathrm{M} {\mathrm{CuSO}}_4$ (aq.) solution was electrolysed using inert electrodes by passing current till the $\mathrm{pH}$ of the resulting solution was $2$. The solution after electrolysis was neutralized and then treated with excess $\mathrm{KI}$ and formed ${\mathrm{I}}_2$ was titrated with $0.04 \mathrm{M} {\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$. Calculate the required volume (in $\mathrm{mL}$) of ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$.

A $100 \mathrm{ml}$ solution of $0.1 \mathrm{N} \mathrm{HCl}$ was titrated with $0.2 \mathrm{N} \mathrm{NaOH}$ solution. Find the volume of $\mathrm{KOH} \left(0.25 \mathrm{N}\right)$ that will be required for completing the titration, if the titration was discontinued after adding another $30 \mathrm{ml}$ of $\mathrm{NaOH}$ solution. 

A unit litre solution has a oxalic acid and carbonic acid dissolved in water. To neutralise 100 mL of  0.1M NaOH solution completely, 200 mL of the given solutuon is required.Another 200 mL of the same sample required 40 mL of 0.1 N of ${{\mathrm{KMnO}}_4}_{}$. Which amongh the given statement is wrong?

What will be the molar mass of the dibasic acid if $1.575\mathrm{ }\mathrm{g}$ of a dibasic acid is neutralized by $25\mathrm{ }\mathrm{mL}$ of $1\mathrm{ }\mathrm{M}\mathrm{ }\mathrm{NaOH}$ solution.?

What is the amount of $\mathrm{NaOH}$ required to neutralise $200\mathrm{ }\mathrm{ml}$ of $0.5\mathrm{M}\mathrm{ }{\mathrm{H}}_2{\mathrm{SO}}_4$ solution?

Find out the volume of $1\mathrm{M}\mathrm{ }\mathrm{HCl}$ required to react with a solution containing 0.5 mole of $\mathrm{KOH}$ and 1 mole of ${\mathrm{Na}}_2{\mathrm{CO}}_3$ in presence of phenolphthalein indicator.

What will be the value of X if - $40\mathrm{ }\mathrm{ml}$ of 1 M ${\mathrm{H}}_{\mathrm{x}}\mathrm{A}$ it required to completely react with $20 \mathrm{ml}$ of 1 M ${\mathrm{Ca}\left(\mathrm{OH}\right)}_2.$ 

What is the molecular weight of acid if 10 mL of 0.1 M solution $\mathrm{NaOH}$ is completely neutralized by 25 mL of 3 g of dibasic acid in one litre solution?

A 50 mL 0.015 M Sodium Sulfite​ solution require 12 mL of an acidified potassium manganate solution for complete reaction. Volume of same permanganate solution that would be required to oxidize completely 0.12 g of Iron Oxalate is (Molecular weight of Fe = 56)

Excess of KI is allowed to react with a sample consisting of chocolate-brown powder of PbO₂ and iodine liberated is reacted with N₂H₄ in another container. 1.12 litre of gas was liberated from this second container at STP .What is the volume of decimolar NaOH (in litres) required to dissolve PbO₂ completely? (Assume all reactions are 100% complete)