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?

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

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 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?

The required volume (in litres) of $30$ volume ${\mathrm{H}}_2{\mathrm{O}}_2$ in acidified medium required for decolourization of one mole of ${\mathrm{KMnO}}_4$ is:

Calculate the moles of ${\mathrm{I}}^{-}$ ion that are required to react with $1 \mathrm{mole}$ of ${\mathrm{MnO}}_4^{-}$ in acidic medium?

What volume of $\mathrm{1 }\mathrm{M}\mathrm{ }\mathrm{HCl}$ is 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.

Find out the volume of $0.154 \mathrm{M} {\mathrm{CrO}}_4^{-2}$ required in basic medium, to react with $40 \mathrm{mL}$ of $0.246,{\mathrm{S}}_2{\mathrm{O}}_3^{-2},$ and oxidise it to ${\mathrm{SO}}_4^{-2}?$

$1.2 \mathrm{g}$ sample of ${\mathrm{Na}}_2{\mathrm{CO}}_3$ and ${\mathrm{K}}_2{\mathrm{CO}}_3$ was dissolved in water to form $100 \mathrm{mL}$of a solution, $20 \mathrm{mL}$ of this solution required $40 \mathrm{mL}$ of $0.1\mathrm{N}$ $\mathrm{HCl}$ for complete neutralisation. $20 \mathrm{mL}$ of this solution is treated with excess of $\mathrm{BaCl}$₂. Calculate the weight of the precipitate.

Regarding the primary standards, how many statement(s) is/are correct?

i.  Primary standards have high purity.

ii. Primary standard solution can be directly prepared by dissolving in solvent.

iii.$ \mathrm{NaOH}$ and $\mathrm{KMnO}_{4}$ are examples of primary standards.

iv. Some hydrate salts are also used as primary standards.

$60 \mathrm{mL}$ of $\mathrm{NaOH}$ solution is completely neutralised by $0.98 \mathrm{g}$ of ${\mathrm{H}}_3{\mathrm{PO}}_4$. The concentration of $\mathrm{NaOH}$ solution is:

If $10$ volume of ${\mathrm{H}}_2{\mathrm{O}}_2$ reacts completely with $100 \mathrm{ml}$ of $2 \mathrm{N} {\mathrm{KMnO}}_4$, calculate the volume of ${\mathrm{H}}_2{\mathrm{O}}_2$ used in $\mathrm{mL}$.

A certain volume of $17\mathrm{M}$ sulphuric acid, $5 \mathrm{mL}$ of $8 \mathrm{N}$ nitric acid and $4.8 \mathrm{mL}$ of hydrochloric acid are mixed together and made up to a volume of $2 L. 42.9 \mathrm{mL}$ of sodium carbonate solution containing one gram of ${\mathrm{Na}}_2{\mathrm{CO}}_3$ $.10{\mathrm{H}}_2\mathrm{O}$ is neutralised by exactly $30 \mathrm{mL}$ of this acid mixture in $100 \mathrm{mL}$ of water. Find out the amount in grams, of the sulphate ions in the solution.

To measure the quantity of manganese chloride $\left({\mathrm{MnCl}}_2\right)$ dissolved in an aqueous solution, it was completely converted to ${\mathrm{KMnO}}_4$ using the reaction, ${\mathrm{MnCl}}_2+{\mathrm{K}}_2{\mathrm{S}}_2{\mathrm{O}}_8+{\mathrm{H}}_2\mathrm{O}\to {\mathrm{KMnO}}_4+\mathrm{HCl}$ (equation not balanced). Few drops of concentrated $\mathrm{HCl}$ ware added to this solution and gently warmed. Further, oxalic acid $\left(225 \mathrm{mg}\right)$ was added in proportions until the colour of the permanganate ion disappeared. The quantity of ${\mathrm{MnCl}}_2$ (in mg) present in the initial solution will be:

$\left(\mathrm{Atomic} \mathrm{weights} \mathrm{is} \mathrm{g} {\mathrm{mol}}^{-1}: \mathrm{Mn}=55, \mathrm{Cl}=35.5\right)$

1 g of a mixture of Na₂ CO₃ and K₂ CO₃ was made upto 250 mL in  aqueous solution. 25 mL of this solution was neutralized by 20 mL of HCl of unknown concentration. The neutralized solution required 16.24 mL of 0.1 N AgNO₃ for precipitation. Calculate
 the % K₂CO₃ in mixture

A mixture of H₂C₂O₄ (oxalic acid) and NaHC₂O₄ weighing 2.02 g was dissolved in water and the solution made up to one litre. Ten millilitres of the solution required 3.0 mL of 0.1 N sodium hydroxide solution for complete neutralization. In another experiment, 10.0 mL of the same solution, in hot dilute sulphuric acid medium, required 4.0 mL of 0.1 N potassium permanganate solution for complete reaction. Calculate the ratio of mass of NaHC₂O₄ to H₂C₂O₄ in the original mixture.