The pH of a 0.01 M NaOH (aq) solution will be:

Which of the following cannot act both as Bronsted acid and as Bronsted base?

The molar solubility of ${\mathrm{CaF}}_2 ({\mathrm{K}}_{\mathrm{sp}}=5.3 \mathrm{x} {10}^{-11})$ in 0.1 M solution of NaF will be

When 10 ml of 0.1 M acetic acid (pK_a=5.0) is titrated against 10 ml of 0.1 M ammonia solution (pK_b=5.0),the pH at equivalence point will be:

For reaction 2NOCl_(g)⇔2NO_(g)+Cl_2(g),

K_C at 427$°$C is $3\times {10}^{-6}\mathrm{L} {\mathrm{mol}}^{-1}$. The value of K_p is nearly-

Which of the oxoacids listed has the highest K_a value?

For the equilibrium, $\underset{\left(g\right)}{PQ} \rightleftharpoons \underset{\left(g\right)}{P}+\underset{\left(g\right)}{Q}$ at 300 K. The pressure at which 50% of PQ is dissociated is numerically equal to 

The number of ${\mathrm{H}}^{\oplus }$ ions present in 1 ml of a solution whose pH= 4 , is given as:

($N_A= Avogadro\text{'}s number$)

$K_c for PC{I}_5\left(g\right)\rightleftharpoons PC{I}_3\left(g\right)+C{I}_2\left(g\right) is 0.04 at 25°.$ The number of moles of $PC{I}_5$ required to a 3.0 liter flask to obtain $C{I}_2$ of concentration 0.15 M is

1. 1.5 mole

For the following reaction,

 $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right) at 250°C,$

The effect on the state of equilibrium on doubling the volume of the system will be:

Which of the following can not act as a buffer?

If solubility product of Ca${\left(\mathrm{OH}\right)}_2 \mathrm{is} {10}^{-11}$, the pH at which $\mathrm{Ca}{\left(\mathrm{OH}\right)}_2$ precipitate from a solution containing decimolar concentration of ${\mathrm{Ca}}^{2+}$ is

For the reaction,

${\mathrm{CuSO}}_4.5{\mathrm{H}}_2\mathrm{O}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{CuSO}}_4.3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{s}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

Which one is the correct representation?

The solubility of ${\mathrm{PbCI}}_{2 }\mathrm{in} \mathrm{water} \mathrm{is} 0.01 \mathrm{M} \mathrm{at} 25°\mathrm{C}.$ Maximum concentration of $\left[{\mathrm{Pb}}^{2+}\right]$ in 0.1 M NaCI will be

If the pH of 0.1 M NaCN solution is 11, then the percentage hydrolysis will be:

How much water should be added to 400 mL of HCI solution in order to raise the pH by one unit?

Vapour density of ${\mathrm{N}}_2{\mathrm{O}}_4$ when heated to $100°\mathrm{C}$ becomes 24.5. its degree of dissociation at this temperature is

For the equilibrium ${\mathrm{SO}}_2{\mathrm{CI}}_2\left(\mathrm{g}\right)\underset{}{\overset{}{\rightleftharpoons }}{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{CI}}_2\left(\mathrm{g}\right)$ volume is increased. When the equilibrium is reestablished

In the reaction A(g) + 2B(g) ⇌ 2C(g) + D(g), the initial concentration of B is twice that of A and, at equilibrium, the concentrations of A and D are equal. Then the value of the equilibrium constant will be:

$2\mathrm{HI}\stackrel{}{\rightleftharpoons }{\mathrm{H}}_2+{\mathrm{I}}_2$ for 22% dissociation what would be the value of equilibrium constant?

The degree of hydrolysis of which of the following salts is independent of the concentration of a solution?

The dissociation of solid ${\mathrm{NH}}_4\mathrm{SH}$ in a closed container produces a pressure of 4 atm at $95°\mathrm{C}$, then ${\mathrm{K}}_{\mathrm{p}}$ for the reaction will be:

${\mathrm{NH}}_4\mathrm{SH}\left(\mathrm{s}\right)\stackrel{}{\rightleftharpoons }{\mathrm{NH}}_3\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$

Which of the following favours the backward reaction in a chemical equilibrium?

If the pH of an acidic buffer is 5.7 and ${\mathrm{pK}}_{\mathrm{a}}$ is 5 then the ratio of $\frac{\left[\mathrm{Salt}\right]}{\left[\mathrm{Acid}\right]}$ will be:

On adding NH₄CI to an NH₄OH solution, the pH of the solution will 

Consider the following two reactions : 

$\mathrm{NO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\stackrel{}{\rightleftharpoons }{\mathrm{NO}}_2\left(\mathrm{g}\right); {\mathrm{K}}_1= 4\times {10}^{-3}$

$2{\mathrm{NO}}_2\left(\mathrm{g}\right)\stackrel{}{\rightleftharpoons }2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right); {\mathrm{K}}_2=?$

If ${\mathrm{K}}_1 \mathrm{and} {\mathrm{K}}_2$ are equilibrium constants, the value of ${\mathrm{K}}_2$ will be:

The concentration of $\left[{\mathrm{H}}^{+}\right]$ ion in a solution containing 0.1 M HCN and 0.2 M NaCN will be:

(${\mathrm{K}}_{\mathrm{a}}$ for HCN = $6.2\times {10}^{-10}$)

If the molar concentration of ${\mathrm{SnCl}}_4$ is $1.5 \times {10}^{-3}$ mol L^–1,the concentration of chloride ions will be:

Find out the solubility of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ in 0.1 M NaOH. Given that the ionic product of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ is 2x ${10}^{-15}$

Which of the following change will shift the reaction in forward direction?

${\mathrm{I}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{l}\left(\mathrm{g}\right)\hspace{0.17em}\mathrm{Take} ∆\mathrm{H}°=+150 \mathrm{kJ}$

A reversible reaction is said to have attained equilibrium, when

In what manner will increase of pressure affect the following equation?

$\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$

The equilibrium between water and its vapour, in an open vessel

Which of the following equilibrium, in gaseous phase, would be unaffected by an increase in pressure?

A saturated solution of non-radioactive sugar was taken and a little radioactive sugar was added to it. A small amount of it gets dissolved in solution and an equal amount of sugar was precipitated. This proves

When two reactants A and B are mixed to give products C and D, the reaction quotient Q, at the initial stages of the reaction

A vessel at equilibrium, contains SO₃, SO₂ and O₂. Now some helium gas is added, so that total pressure increasese while temperature and volume remain constant. According to Le Chatelier's Principle, the dissociation of SO₃ 

A chemical reaction is catalysed by a catalyst X. Hence, X

If for the reaction given below

$$\begin{gathered} \underset{\mathrm{g}}{2\mathrm{PQ} }\rightleftharpoons \underset{\mathrm{g}}{ {\mathrm{P}}_2 }+\underset{\mathrm{g}}{ {\mathrm{Q}}_2 ; }{\mathrm{K}}_1=2.5\times {10}^5 \\ \underset{\mathrm{g}}{\mathrm{PQ} }+ \frac{1}{2}\underset{\mathrm{g}}{{\mathrm{R}}_2 }\rightleftharpoons \underset{\mathrm{g}}{\mathrm{PQR}; }{\mathrm{K}}_2=5\times {10}^{-3} \end{gathered}$$

find K₃ for the reaction $\frac{1}{2}{\mathrm{P}}_2 + \frac{1}{2}{\mathrm{Q}}_2 +\frac{1}{2}{\mathrm{R}}_{2 }\rightleftharpoons \mathrm{PQR}$

For equilibrium reaction

$2{\mathrm{NO}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)+14.6 \mathrm{J},$ increase in temperature would

In the reaction ${\mathrm{H}}_2+{\mathrm{I}}_2\rightleftharpoons 2\mathrm{HI}$ at equilibrium, some I₂ is added. What happens to the equilibrium?

Which of the following reaction will be favoured at low pressure?

For the reaction

${\mathrm{PCl}}_5\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

the forward reaction at constant temperature is favoured by

A. introducing an inert gas at constant volume

B. introducing chlorine gas at constant volume

C. introducing an inert gas at constant pressure

D. increasing the volume of the container

E. introducing PCl₅ at constant volume

For the reaction

$\mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$

at a given temperature, the equilibrium amount of ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ can be increased by

In which of the following cases does the reaction remain fastest to completion?

Consider the following reactions:

A. ${\mathrm{AB}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{B}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{AB}}_3\left(\mathrm{g}\right)$

B. $2{\mathrm{AB}}_3\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{AB}}_2+{\mathrm{B}}_2\left(\mathrm{g}\right)$

If K₁ and K₂ are the equilibrium constants at $27°\mathrm{C}$ in reactions A and B respectively, then K₁, and K₂ are related as

For the reaction, ${\mathrm{H}}_2+{\mathrm{I}}_2\rightleftharpoons 2\mathrm{HI}$, the equilibrium concentrations of H₂, I₂ and HI are 8, 3 and 28 mol L^-1 respectively. Equilibrium constant of the reaction is

In which of the following case, the value of K_p is less than K_c?

Equilibrium constants K₁, and K₂ for the following equilibria

$$\begin{gathered} \mathrm{NO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\stackrel{{\mathrm{K}}_1}{\rightleftharpoons }{\mathrm{NO}}_2\left(\mathrm{g}\right) \mathrm{and} \\ 2{\mathrm{NO}}_2\left(\mathrm{g}\right)\stackrel{{\mathrm{K}}_2}{\rightleftharpoons }2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2 \end{gathered}$$

are related as

In a chemical equilibrium rate constant of forward reaction is $7.5\times {10}^{-4}$ and the equilibrium constant is 1.5. The rate constant of a backward reaction is