List of top Chemistry Questions on Equilibrium asked in AIEEE

If $K_{sp}$ of $CaF_2$ at $25^??$ is $1.7 \times 10^{-10}$, the combination amongst the following which gives a precipitate of $CaF_2$ is

The equilibrium constant $\left(K_{c}\right)$ for the reaction $N_{2}$$_{(g)}$ + $O_{2}$ $_{(g)} \to 2NO \left(g\right)$ at temperature T is $4 � 10^{-4}$. Thevalue of Kc for the reaction $NO$$_{(g)} \to \frac{1}{2} N_{2}$$_{(g)} + \frac{1}{2} O_{2}$$_{(g)}$ at the same temperature is :

An acid HA ionises as $HA {\rightleftharpoons} H^{+} + A^{-}$ The pH of 1.0 M solution is 5. Its dissociation constant would be:

A vessel at 1000 K contains $CO_2$ with a pressure of 0.5 atm. Some of the $CO_2$ is converted into CO on the addition of graphite. It the total pressure at equilibrium is 0.8 atm, the value of K is

At $25^{\circ}C$, the solubility product of $Mg\left(OH\right)_{2} $ is $1.0 \times 10^{-11}$. At which pH, will $Mg^{2+}$ ions start precipitating in the form of $Mg\left(OH\right)_{2}$ from a solution of $0.001 \,M \,Mg^{2+}$ ions ?

In aqueous solution the ionization constants for carbonic acid are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$ Select the correct statement for a saturated 0.034 M solution of the carbonic acid.

Solid $Ba\, (NO_3)_2$ is gradually dissolved in a $1.0 ? 10^{-4}M\,Na_2CO_3$ solution. At what concentration of $Ba^{2+}$ will a precipitate begin to form ?($K_{sp}$ for $Ba\, CO_3 = 5.1 ? 10^{-9}$).

The $pK_a$ of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which $50\%$ of the acid is ionized is

In a sautrated solution of the sparingly soluble strong electrolyte $AgIO_3$ (Molecular mass $= 283$) the equilibrium which sets in is $ {AgIO_{3(s)}<=>Ag^+_{(aq)} +IO^{-}_{3(aq)}}$ If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1.0 ??10^{-8}$, what is the mass of $AgIO_3$ contained in $100\, ml$ of its saturated solution?

For the reaction $ {2NO2(g) <=> 2\,NO(g) + O2(g)}$ $\left(K_{c} = 1.8\times10^{-6} \,at \,184^{\circ}C\right)$ $\left(R = 0.00831 \,k J/\left(mol. K\right)\right)$ When $K_{p}$ and $K_{c}$ are compared at $184^{\circ}$ C it is found that :

Hydrogen ion concentration in mol/L in a solution of pH = 5.4 will be :

What is the conjugate base of $OH^-$ ?

For the reaction, $ {CO(g) + Cl2(g) <=> COCl2(g)}$ the $\frac{K_{p}}{K_{c}}$ is equal to

What is the equilibrium expression for the reaction $ {P_{4(s)} +5O_{2(g)} <=> P4O_{10(s)}}$ ?

A solution of an acid has pH = 4.70. Find out the number of $OH^-$ ions $(pK_w = 14)$

How do we differentiate between $Fe^{3+}$ and $Cr^{3+}$ in group III ?