Equilibrium practice · Medium

The $\mathrm{pH}$ of $0.005 \mathrm{~M}-\mathrm{NaOH}$ solution is $(\log 2=0.3)$

In a reversible reaction $A+B \rightleftharpoons 2 C$, the equilibrium concentrations of (A), (B) and (C) are $2 \mathrm{M}, 2 \mathrm{M}$ and $4 \mathrm{M}$ respectively then $\mathrm{K}_{\mathrm{C}}$ for the reaction is

Statement (S): HCl acts as weak base in liquid HF but weak acid in acetic acid
Explanation (E): The tendency to act as acid or base also depends upon the nature of other substance to accept or donate a proton.

STATEMENT I : $p H$ of $10 \mathrm{M}$ $HCl$ aqucous solution is less than 1.

STATEMENT II : $p H$ is equal to logarithm of $\mathrm{H}^{+}$concentration.

The exothermic formation of $\mathrm{Cl}{\mathrm{F}_3}$ is represented by the equation
$\mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right) + 3{\mathrm{F}_2}\left( \mathrm{g} \right)\leftrightharpoons2\mathrm{Cl}{\mathrm{F}_3}\left( \mathrm{g} \right);$
$\Delta H = - 329\,\mathrm{kJ}$
Which of the following will increase the quantity of $\mathrm{Cl}{\mathrm{F}_3}$ in an equilibrium mixture of $\mathrm{C}{\mathrm{l}_2},{\mathrm{F}_2}\mathrm{and Cl}{\mathrm{F}_3}$?

Hydrogen ion concentration in mol/L in a solution of $\mathrm{pH} = 5.4$ will be

For the following Assertion and Reason the correct option is
Assertion: The pH of water increases with increase in temperature.
Reason: The dissociation of water into ${H^ + }$ and $O{H^ - }$ is an exothermic reaction.

Statement-I: pH of a buffer solution does not change on dilution.

Statement-II:On dilution the ratio of concentration of salt and acid (or base) remains unchanged.

${K}_{{P}}$ and ${K}_{{C}}$ ratio for the following reaction

${SO}_2({~g})+\frac{1}{2} {O}_2({~g}) \rightleftharpoons {SO}_3({~g})$ will be

Statement I In the titration of weak acid with strong base,
neutral point can't be attained
Statement II Salt formed is hydrolysed to form alkaline
solution

$20 \mathrm{~mL}$ of $0.1 \mathrm\,\,{M} \mathrm\,\,\,{NH}_4 \mathrm{OH}$ is mixed with $40 \mathrm{~mL}$ of $0.05 \mathrm\,\,{M} \mathrm\,\,\,{HCl}$. The $\mathrm{pH}$ of the mixture is nearest to
(Given : $\mathrm{K}_{\mathrm{b}}\left(\mathrm{NH}_4 \mathrm{OH}\right)=1 \times 10^{-5}, \log 2=0.30, \log 3=$ $0.48, \log 5=0.69, \log 7=0.84, \log 11=1.04$ )

In ${A}+{B} \rightleftharpoons {C}$. The unit of equilibrium constant is :

STATEMENT I : Addition of $\mathrm{HCl}(a q)$ to $\mathrm{HCOOH}(a q)$ decreases the ionization of $\mathrm{HCOOH}$

STATEMENT II : Common ion effect of $\mathrm{H}^{+}$ion, reduces the ionization of $\mathrm{HCOOH}$

Which of the following combinations of $\mathrm{CH}_3 \mathrm{COOH}+\mathrm{NaOH}$ would result in the formation of acidic buffer?

Assertion (A): On increasing temperature pH of $\mathrm{H}_2 \mathrm{O}$ decreases.

Reason (R): At high temperature water become acidic.

Calculate the $\mathrm{pH}$ of solution made by two solution having $\mathrm{pH}=1.5$ and 2.5

$\mathrm{C}(\mathrm{s})+\mathrm{H}_2 \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{H}_2(\mathrm{g}) ; \Delta \mathrm{H} < 0$. The above equilibrium will proceed in forward direction when

A solution that has reserve acidity (or) alkalinity is called

At $90^{\circ} \mathrm{C}$ pure water has $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=10^{-6} \mathrm{M}$. What is the value of $\mathrm{K}_{\mathrm{w}}$ at this temperature?

The melting points of most of the solid substances increase with an increase of pressure. However, ice melts at a temperature lower than its usual melting point when the pressure is increased. This is because:

$pH$ for the solution of salt undergoing anionic hydrolysis (say $\mathrm{C}{\mathrm{H}_3}\mathrm{COONa}$ ) is given by:

The solubility of $\mathrm{AgCl}$ in $0.2 \mathrm{~M} \mathrm{~NaCl}$ is

$\left[\mathrm{K}_{\mathrm{sp}} \mathrm{AgCl}=1.8 \times 10^{-10}\right]$

An aqueous solution of aniline of concentration $0.24 \mathrm{~M}$ is prepared. What is concentration of sodium hydroxide is needed in this solution so that anilinium ion concentration remains at $1 \times 10^{-8} \mathrm{M}$ ? ( $K_b$ for $\left.\mathrm{C}_6 \mathrm{H}_5 \mathrm{NH}_3{ }^{+}=2.4 \times 10^{-5} \mathrm{M}\right)$

Solubility product principle can be applied when

Assertion :-For a reaction $A\left( g \right) + B\left( g \right) \rightleftarrows AB_{\left( g \right)}$ if inert gas is added in a container at
constant volume. The equilibrium shifts to left side.
Reason :- Because partial pressure of $A, B$ and $AB$ decreases.

The $K_{s p}$ of $\mathrm{PbCrO}_4$ is $1.0 \times 10^{-16}$. Then the molar solubility of $\mathrm{PbCrO}_4$ is:

The value of $K_{\mathrm{P}}$ for the process: $\mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O}(\mathrm{s})\rightleftharpoons \mathrm{CuSO}_4 \cdot 3 \mathrm{H}_2 \mathrm{O}(\mathrm{s})+2 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$ is $1.21 \times 10^{-4} \mathrm{~atm}^2$ at certain temperature. If aqueous tension at that temperature is 40 torr, then at what relative humidity of air will $\mathrm{CuSO}_4 \cdot 5 \mathrm{H}_2 \mathrm{O}$ effloresces?

The strength of an acid depends on its tendency to

A saturated solution of $\mathrm{Mg}{\left( {\mathrm{OH}} \right)_2}$ in water at $25^\circ C$ contains $0.11\;\mathrm{g}\;\mathrm{Mg}{\left( {\mathrm{OH}} \right)_2}$ per litre of solution. The solubility product of $\mathrm{Mg}{\left( {\mathrm{OH}} \right)_2}$ is:

The concentration of $\mathrm{KI }\;\mathrm{and}\;\mathrm{ KCl}$ in a certain solution containing both is 0.001 M each. If 20 mL of this solution is added to 20 mL of a saturated solution of AgI in water. What will happen?

$({K_{\mathrm{sp}}}\;\mathrm{AgCl} = {10^{ - 10}},\;{K_{\mathrm{sp}}}\;\mathrm{AgI} = {10^{ - 16}})$