Question
Consider a titration of potassium dichromate solution with acidified Mohr's salt solution using diphenylamine as indicator. The number of moles of Mohr's salt required per mole of dichromate is
✓
Answer
The formula of Mohr's salt is $F eSO { }_4\left( NH _4\right)_2 SO _4$. It is a mixture of ferrous sulfate and ammonium sulfate. Ferrous sulfate is oxidized by potassium dichromate.
The reaction is as follows:
$K _2 Cr _2 O _7+6 F eSO _4+7 H _2 SO _4 \rightarrow K _2 SO _4+ Cr _2\left( SO _4\right)_3+3 Fe _2\left( SO _4\right)_3+7 H _2 O$
$1$ mole of potassium dichromate reacts with 6 moles of ferrous sulphate. Thus, the number of moles of Mohr's salt required per mole of dichromate is $6.$
Need a full question paper?
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
Explore more
Similar questions
Vapour pressure of a pure solvent at $90\,^oC$ is $1020\, torr$. A solution of $0.1\, m$ concentration has a vapour pressure of $1000\, torr$. What is the molecular weight of solvent ?
→$pH$ of a mixture of $1\ M\ HA (pK_a = 4.2)$ and $1\ M\ NaA$ is $4.5$ . In $300\ ml$ of buffer volume of $HA$ is.......$ml$ $[log\, 2 = 0.3]$
→For the reaction $\mathrm{N}_2 \mathrm{O}_4(\mathrm{~g}) \rightleftharpoons 2 \ \mathrm{NO}_2(\mathrm{~g})$, $\mathrm{K}_{\mathrm{p}}=0.492 \mathrm{~atm}$ at $300 \mathrm{~K} . \mathrm{K}_{\mathrm{c}}$ for the reaction at same temperature is_________ $\quad \times 10^{-2}$. (Given : $\mathrm{R}=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ )
→The number of possible isomers of an octahedral complex $[Co(C_2O_4)_2\,(NH_3)_2 ]^-$ is
→How many of given compounds show Tautomerism
In alkaline condition $KMn{O_4}$ reacts as $2KMn{O_4} + 2KOH \to 2{K_2}Mn{O_4} + {H_2}O + O$. The equivalent weight of $KMn{O_4}$ would be (Atomic mass of $K$ $= 39$, $Mn = 55$, $O = 16$)
→You are given $500\, mL$ of $2\,N\, HCl$ and $500\, mL$ of $5\,N\, HCl$. What will be the maximum volume of $3\, M\, HCl$ that you can make from these two sotutions ? .............. $\mathrm{mL}$
→A compound contains $2.8\%$ $Fe$ by mass. If the compound contains single $Fe$ atom in its one molecule, then the molar mass $(g/mol)$ of the compound is $(Fe = 56\, amu)$
→A solution of $Fe _{2}\left( SO _{4}\right)_{3}$ is electrolyzed for $'x'$ min with a current of $1.5\, A$ to deposit $0.3482\, g$ of $Fe$. The value of $x$ is $.......$. [nearest integer]
→Given : $1 \,F =96500\, C \,mol ^{-1}$
Atomic mass of $Fe =56\, g \,mol ^{-1}$
The number of meso form of the given compound is
→$\begin{array}{*{20}{c}}
{C{H_3} - CH - CH - CH - C{H_3}} \\
{|\,\,\,\,\,\,\,\,\,\,\,\,\,\,|\,\,\,\,\,\,\,\,\,\,\,\,|\,\,\,\,\,} \\
{OH\,\,\,\,\,\,\,OH\,\,\,\,\,OH\,\,}
\end{array}$