Redox Reactions and Titration

${\mathrm{KMnO}}_4$ acts as an oxidising agent in alkaline medium. When alkaline ${\mathrm{KMnO}}_4$ is treated with $\mathrm{KI}$, iodide ion is oxidised to ${{\mathrm{IO}}_{\mathrm{X}}}^{-}$. The value of $\mathrm{X}$ is _____.

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+}$$?$

Volume ${\mathrm{V}}_1 \mathrm{mL}$ of $0.1\mathrm{M} {\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ is needed for complete oxidation of $0.678\mathrm{g} {\mathrm{N}}_2{\mathrm{H}}_4$ in acidic medium. The volume $\left(\mathrm{in} \mathrm{mL}\right)$ of $0.3 \mathrm{M} {\mathrm{KMnO}}_4$ needed for same oxidation in the acidic medium will be

$3.5 \mathrm{g}$ 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 $2{\mathrm{S}}_2{\mathrm{O}}_3^{2-}+{\mathrm{I}}_2⟶{\mathrm{S}}_4{\mathrm{O}}_6^{2-}+2{\mathrm{I}}^{-}:$

An aqueous solution of NaOH having density $1.1 \mathrm{kg} / \mathrm{dm}^{3}$ contains 0.02 mole fraction of $\mathrm{NaOH}$ :

The $10\mathrm{mL}, 1.193\mathrm{M} \mathrm{NaOH}$ solution is completely neutralized by $0.1 \mathrm{M} {\mathrm{H}}_2{\mathrm{SO}}_4$.The volume of ${\mathrm{H}}_2{\mathrm{SO}}_4$ needed is

Which of the following are correct about above observation?

$5 \mathrm{mL}$of $8 \mathrm{N}$ nitric acid, $4.8 \mathrm{mL}$ of $5 \mathrm{N}$ hydrochloric acid and a certain volume of $17 \mathrm{M}$ sulphuric acid are mixed together and made up to $2 \mathrm{L}$. $30 \mathrm{mL}$ of this acid mixture exactly neutralise $42.9 \mathrm{mL}$ of sodium carbonate solution containing one gram of ${\mathrm{Na}}_2{\mathrm{CO}}_3.10{\mathrm{H}}_2\mathrm{O}$ in $100 \mathrm{mL}$ of water. Calculate the amount in grams of the sulphate ions in solution. Report the answer after multiplying with 10 and round off to the nearest integer._​

An alkali is titrated against an acid with methyl orange as indicator, which of the following is a correct combination?

When I₂O₅ reacts with 50 litre sample of CO gas, the CO gas converted into CO₂ according to given reaction,
I₂O₅(s) + CO(g) $\to$ CO₂(g) + I₂(g)
The iodine distilled at this temperature and was collected in an absorber containing 10 ml of 0.025 molar Na₂S₂O₃. The excess hypo was back titrated with 10 ml of 0.002 molar I₂ solution. Then it is found that mass of I₂O₅ (solid) used for the reaction of sample of 50 litre of CO gas is x × 10^–3 gram. Then find value of 2x is (molar mass of I₂ is 254 g/mol).

I₂O₅ जब CO गैस के 50 लीटर नमूने के साथ क्रिया करती है, तो CO गैस निम्न अभिक्रिया के अनुसार CO₂ में परिवर्तित हो जाती है
I₂O₅(s) + CO(g) $\to$ CO₂(g) + I₂(g)
इस ताप पर आयोडीन आसवित की जाती है तथा 10 ml 0.025 मोलर Na₂S₂O₃ युक्त एक अवशोषक में एकत्रित कर ली जाती है। आधिक्य हाइपो का 10 ml 0.002 मोलर I₂ विलयन के साथ पश्च अनुमापन किया जाता है। तब यह पाया गया कि 50 लीटर CO गैस के नमूने की अभिक्रिया के लिए प्रयुक्त I₂O₅ (ठोस) का द्रव्यमान x × 10^–3 ग्राम है। 2x का मान ज्ञात कीजिए (I₂ का मोलर द्रव्यमान = 254 g/mol).

$25 mL$ of $HCl$ is titrated with $30 mL$ of $0.1M N{a}_{2}C{O}_3.$ How many $ml$ of the same $HCl$ solution will be consumed when it reacts with $30 mL 0.2 M NaO\mathrm{H?}$

If 10.00 g ${\mathrm{V}}_2{\mathrm{O}}_5$ is dissolved in acid and reduced to ${\mathrm{V}}^{2+}$ by treatment with $\mathrm{Z}\mathrm{n}\mathrm{ }$ metal, how many mole ${\mathrm{I}}_2$ could be reduced by the resulting $\mathrm{ }{\mathrm{V}}^{2+}$ solution as it is oxidised to ${\mathrm{V}}^{4+}$ . At weight of V = 51.

The equivalent masses of $\mathrm{N}{\mathrm{a}}_2\mathrm{C}{\mathrm{O}}_3$ when it is titrated with $\mathrm{H}\mathrm{C}\mathrm{l}$ using phenolphthalein and methyl orange separate experiments are

${\mathrm{I}}_2$ 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

$10 \mathrm{mL} \mathrm{of} {\mathrm{H}}_2{\mathrm{O}}_2$solution on treatment with KI and titration of liberated I₂, required $10 \mathrm{mL} \mathrm{of} 1\mathrm{N}$ hypo. Thus H₂O₂ is -

$10 \mathrm{m}\mathrm{L}$ of ${\mathrm{H}}_2{\mathrm{O}}_2$ Solution on treatment with $\mathrm{K}\mathrm{I}$ and titration of liberated ${\mathrm{I}}_2$, required $10\mathrm{ }\mathrm{m}\mathrm{L}$ of $1\mathrm{N}$ Hypo. Thus, ${\mathrm{H}}_2{\mathrm{O}}_2$ is:

2g of potassium ferrocyanide on boiling with conc. H₂SO₄ produces a gas. The gas is collected and then reacted with 3cc, 2 M ferric permanganate in acidic medium and the excess oxidant further requires 6cc, 3 M sodium oxalate for complete reaction in acidic medium. Calculate % purity of potassium ferrocyanide. Given, ${\text{M}}_{{\text{K}}_4\left[\text{Fe}{\left(\text{CN}\right)}_6\right]}=\text{368 g}/\text{mol}$

0.75 g sample containing ${\text{Fe}}_3{\text{O}}_4\left(\text{M}=232\right)$ and some inert impurity was dissolved in dilute ${\text{H}}_2{\text{SO}}_4$ solution and excess of Zn powder was added, so that all iron gets reduced to ferrous $\left({\text{Fe}}^{2+}\right)$ ions. The resulting solution was made free from unreacted zinc and then titrated against 0.1 M acidified KMnO₄ solution. A volume of 12 mL was required to reach the end point. Determine the mass percentage of Fe₃O₄ in the original sample.