Equilibrium practice · Mixed difficulty

On mixing equal volumes of two buffer solutions of pH value 3 and 5, the pH of the resultant solution will be

The phenomenon of interaction of anions and cations furnished by a electrolyte with the ${\mathrm{H}^ + }$ and $\mathrm{O}{\mathrm{H}^ - }$ ions of water to produce acidic nature or alkalinity is known as hydrolysis. In hydrolysis:

Assertion :- If $\mathrm{K}_{\mathrm{sp}} <$ ionic produce, precipitate is formed.

Reason :- Solubility product $\left(\text{K}_{\mathrm{sp}}\right)$ is the highest limit of ionic product of the electrolyte in saturated solutions.

The equilibrium constant for the reaction, $\mathrm{HONO} + \mathrm{C}{\mathrm{N}^ - } \to \mathrm{HCN} + \mathrm{ON}{\mathrm{O}^ - }$ is $1 \times {10^{ - 14}}.$ The magnitude of the equilibrium constant suggests that:

When hydrogen molecules decomposed into it’s atoms which conditions gives maximum yield of H atom?

Buffer capacity of a buffer solution is x, the volume of 1M added to 100 ml of this solution if the change of ${P^H}$ by 1 is

The principal buffer present in human blood

In a 500 mL flask, the degree of dissociation of $\mathrm{PC}{\mathrm{l}_5}$ at equilibrium is $40\%$ and the initial amount is 5 moles. The value of equilibrium constant in $\mathrm{mol}\;{\mathrm{L}^{ - 1}}$ for the decomposition of $\mathrm{PC}{\mathrm{l}_5}$ is

The following equilibrium constants were determined at $1120 {~K}$ :
$\begin{aligned} & 2 {CO}(g) \rightleftharpoons {C}({s})+{CO}_2({~g}) ; K_{p_1} =10^{-14} {~atm}^{-1} \\ & {CO}(g)+{Cl}_2(g) \rightleftharpoons {COCl}_2({~g}) ; K_{p_2} =6 \times 10^{-3} {~atm}^{-1} \end{aligned}$
What is the equilibrium constant $K_c$ for the following reaction at $1120 {~K}$ :
${C}({s})+{CO}_2({~g})+2 {Cl}_2({~g}) \rightleftharpoons 2 {COCl}_2({~g})$

The equilibrium constant for the reaction ${\mathrm{N}_2} + 3{\mathrm{H}_2}\;\leftrightharpoons2\mathrm{N}{\mathrm{H}_3}$ is $K$ then the equilibrium constant for the equilibrium,

$\mathrm{N}{\mathrm{H}_3}\;\leftrightharpoons\frac{1}{2}{\mathrm{N}_2} + \frac{3}{2}{\mathrm{H}_2}\;is$

Degree of dissociation of $\mathrm{N}{\mathrm{H}_4}\mathrm{OH}$ in water is $1.8 \times {10^{ - 5}}$, then hydrolysis constant of $\mathrm{N}{\mathrm{H}_4}\mathrm{Cl}$ is

Phosphorus pentachloride dissociates as follows, in a closed reaction vessel,,br>
$\mathrm{PC}{\mathrm{l}_5}\left( \mathrm{g} \right)\leftrightharpoons\mathrm{PC}{\mathrm{l}_3}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right)$

If total pressure at equilibrium of the reaction mixture is $p$ and degree of dissociation of $\mathrm{PC}{\mathrm{l}_5}\;\mathrm{is}\;x$, the partial pressure of $\mathrm{PC}{\mathrm{l}_3}$ will be

The $\mathrm{pH}$ of blood is:

The $\left[ {{\mathrm{H}^ + }} \right]$ ion concentration in $0.001\;M$ acetic acid is $1.34 \times {10^{ - 4}}\;\mathrm{g}\;\mathrm{ ion}\;/\mathrm{litre}\mathrm{.}$ The $\left[ {{\mathrm{H}^ + }} \right]$ ion concentration of $0.164\;\mathrm{g}\;\mathrm{ of}\;\mathrm{ C}{\mathrm{H}_3}\mathrm{COONa}$ is added to a litre of $0.001\;M$ $\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}$ will be:

Strongest acid is

Assertion (A): Increasing order of acidity of hydrogen halides is $\mathrm{HF} < \mathrm{HCl} < \mathrm{HBr} < \mathrm{HI}$.

Reason (R): While comparing acids formed by the elements belonging to the same group of the periodic table, $\mathrm{H}-\mathrm{A}$ bond strength is a more important factor in determining acidity of an acid than the polar nature of the bond.

Conjugate acid-base pair differs by a/an:

${K_c}$ for the reaction : ${\left[ {\mathrm{Ag}{{\left( {\mathrm{CN}} \right)}_2}} \right]^ - }\leftrightharpoons\mathrm{A}{\mathrm{g}^ + } + 2\mathrm{C}{\mathrm{N}^ - },$ the equilibrium constant at $25^\circ C\mathrm{ }\;is\mathrm{ }\;4.0\mathrm{ } \times \mathrm{ }{10^{ - 19}},$ then the silver ion concentration in a solution which was originally $\mathrm{0}\mathrm{.1}\;\mathrm{molar}\;\mathrm{in}\;\mathrm{KCN}$ and $\mathrm{0}\mathrm{.03}\;\mathrm{molar}\;\mathrm{in}\;\mathrm{AgN}{\mathrm{O}_3}$ is :

The reactions, $\mathrm{PCl}_5(\mathrm{~g}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})$ and $\mathrm{COCl}_2(\mathrm{~g})=\mathrm{CO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g})$ are simultaneously in equilibrium in an equilibrium box at constant volume. A few moles of $\mathrm{CO}(\mathrm{g})$ are later introduced into the vessel. After some time, the new equilibrium concentration of

The $\mathrm{pH}$ value of $0.1 \mathrm{~M}$ solutions of $\mathrm{CH}_3 \mathrm{COONa} \text{(I)}, \mathrm{CH}_3 \mathrm{COOH} \text{(II)}, \mathrm{CH}_3 \mathrm{COONH}_4 \text{(III)}, \mathrm{NaOH} \text{(IV)}$ and ${HCl}(\mathrm{V})$ is in the order

For the following reactions, equilibrium constants are given: $S(s) + {O_2}(g)\underset{{}}{\overset{{}}{\leftrightharpoons}}S{O_2}(g);{K_1} = {10^{52}}$
$2S(s) + 3{O_2}(g)\leftrightharpoons2S{O_3}(g);{K_2} = {10^{129}}$
The equilibrium constant for the reaction, $2SO(g) + {O_2}(g)\leftrightharpoons2S{O_3}(g)$ is

The reaction that proceeds in the forward direction is :

From separate solutions of four sodium salts $\mathrm{Na}W,\mathrm{Na}X,\mathrm{Na}Y\;and\;\mathrm{Na}Z$ had $\mathrm{pH}\;\;7.0,9.0,10.0\;and\;11.0$ respectively. When each solution was $0.1\;M$, the strongest acid is:

The $pH$ of a ${10^{ - 9}}$ M solution of $\mathrm{HCl}$ in water is

For reaction in equilibrium, $\mathrm{H}_2(g)+\mathrm{I}_2(g) \rightleftharpoons 2 \mathrm{HI}(g)$

Choose the correct option.

In the following reversible reaction,

$2\mathrm{S}{\mathrm{O}_2} + {\mathrm{O}_2}\leftrightharpoons2\mathrm{S}{\mathrm{O}_3} + Q{\kern 1pt} {\kern 1pt} \mathrm{cal}$

Most suitable condition for the higher production of $\mathrm{S}{\mathrm{O}_3}$ is

In an equilibrium reaction ${H_2}(g) + {I_2}(g)2HI(g);\Delta H = - 3000$ cal. Which factor favours dissociation of HI

$2 A=B, K_{\text {eq }}=X$
$2 B \rightleftharpoons C ; K_{\text {eq }}=Y$
$D\rightleftharpoons C, {K}_{\text {eq }}=Z$
Equilibrium constant for the reaction $D \rightleftharpoons 4 A$ is

For the chemical reaction, $X\,\,\underset{{}}{\overset{{}}{\leftrightharpoons}}\,Y$ , the standard reaction Gibbs energy depends on temperature T (in K) as ${\Delta _r}G^\circ \left( {\mathrm{in}\,\,\mathrm{ kJ}\,\,\mathrm{ mo}{\mathrm{l}^{ - 1}}} \right)\, = 120 - \frac{3}{8}T$
The major component of the reaction mixture at T is

Which one of the following has greater active mass?