Equilibrium practice · Mixed difficulty

A volume of $1.0 \mathrm{~L}$ of solution which was in equilibrium with solid mixture of ${AgCl}$ and ${Ag}_2 {CrO}_4$ was found to contain $1 \times 10^{-4}$ moles of ${Ag}^{+}$ ions, $1.0 \times 10^{-6}$ moles of ${Cl}^{-}$ ions and $8.0 \times 10^{-4}$ moles of ${CrO}_4{ }^{2-}$ ions. The ${Ag}^{+}$ ions are added slowly to the above mixture (keeping the volume constant) till $8.0 \times 10^{-7}$ moles of ${AgCl}$ got precipitated. How many moles of ${Ag}_2 {CrO}_4$ were precipitated simultaneously?

The number of ${H^ + }$ ions present in 1 ml of a solution having ${P^H} = 13$ is

At $30^{\circ} \mathrm{C}$, the solubility of ${Ag}_2{CO}_3\left({~K}_{\mathrm{sp}}=8 \times 10^{-2}\right)$ will be maximum in -

Assertion (A): The degree of dissociation of $\mathrm{CH}_3 \mathrm{COOH}$ is more in a solution which is basic than in water.

Reason (R): $\mathrm{K}_{\mathrm{a}}$ of $\mathrm{CH}_3 \mathrm{COOH}$ increases in basic solution.

When 0.5 mole of $\mathrm{N}_2 \mathrm{O}_4$ is placed in a $4.00 \mathrm{~L}$ reaction vessel and heated at $405 \mathrm{~K}, 79.3 \%$ of the $\mathrm{N}_2 \mathrm{O}_4$ decomposes to $\mathrm{NO}_2$. Calculate value of $\mathrm{K}_{\mathrm{P}}$ at $405 \mathrm{~K}$, for the reaction : $\mathrm{N}_2 \mathrm{O}_4(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_2(\mathrm{~g})$.

Given below are two statements: One is labelled as Assertion A and the other labelled as Reason R.
Assertion A: During the boiling of water having temporary hardness, $Mg{(HC{O_3})_2}$ is converted to $MgC{O_3}$.
Reason R The solubility product of $Mg{(OH)_2}$ is greater than that of $MgC{O_3}$.
In the light of the above statements, choose the most appropriate answer from the options given below

What are the product formed when Deuterium is added equilibrium reaction of ${H}_2$ and ${I}_2$ ?

(i) ${HD}$

(ii) ${DI}$

(iii) ${D}_2$

(iv) ${HI}$

Which of the following statements are correct ?

(i) The extent of dissociation of an acid depends on the strength and polarity of the ${H}-{A}$ bond (where ${A}$ is an electronegative element.)

(ii) As the strength of ${H}-{A}$ bond increases, the energy required to break the bond decreases.

(iii) As the electronegativity difference between the atoms ${H}$ and ${A}$ increases, acidity increases

The hydrolysis constant of a salt of weak acid and weak base is inversely proportional to

At a certain temperature, $K_{\mathrm{P}}$ for the dissociation of solid $\mathrm{CaCO}_3$ is $4.5 \times 10^{-2}$ atm and for the reaction $\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g}),$ the $K_{\mathrm{P}}$ value is $2.0 \mathrm{~atm}.$ The pressure of carbon monoxide at this temperature, when solid carbon $\mathrm{CaO}$ and $\mathrm{CaCO}_3$ are mixed together and allowed to attain equilibrium is

At $30^\circ C\;\mathrm{the}\;\mathrm{ solubility}\;\mathrm{ of}\,\mathrm{ A}{\mathrm{g}_2}\mathrm{C}{\mathrm{O}_3}\;\left( {{K_{\mathrm{sp}}} = 8 \times {{10}^{ - 12}}} \right)$ would be greatest in $1\;L$ of

For the equilibrium:

(I) $\mathrm{C}_6 \mathrm{H}_5 \mathrm{COOH}+\mathrm{H}_2 \mathrm{O} \rightleftharpoons \mathrm{C}_6 \mathrm{H}_5 \mathrm{COO}^{-}+\mathrm{H}_3 \mathrm{O}^{+} ; K_1=6.30 \times 10^{-5}$

(II) $\mathrm{C}_6 \mathrm{H}_5 \mathrm{COOH}+\mathrm{OH}^{-} \rightleftharpoons \mathrm{C}_6 \mathrm{H}_5 \mathrm{COO}^{-}+\mathrm{H}_2 \mathrm{O} ; K_2=6.30 \times 10^9$

(III) $\mathrm{H}_2 \mathrm{O}+\mathrm{H}_2 \mathrm{O} \rightleftharpoons \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{OH}^{-} ; K_3-?$

$K_3$ using above equilibria is

$\mathrm{SO}_3(g)$ is partially dissociated into $\mathrm{SO}_2(g)$ and $\mathrm{O}_2(g)$ at $900 \mathrm{~K}$ and $1 \mathrm{~atm}$ as:
$\mathrm{SO}_3(g) \rightleftharpoons \mathrm{SO}_2(g)+\frac{1}{2} \mathrm{O}_2(g)$

The density of the equilibrium mixture was found to be $0.866 \mathrm{~g} \mathrm{~dm}^{-3}$. Thus, degree dissociation of $\mathrm{SO}_3(\mathrm{~g})$. is

Equilibrium constants ${K_1}$ and ${K_2}$  for the following equilibria are related as :
$\mathrm{NO}\left( \mathrm{g} \right) + \frac{1}{2}{\mathrm{O}_2}\left( \mathrm{g} \right)\leftrightharpoons\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right);{K_1}$
$2\mathrm{N}{\mathrm{O}_2}\left( \mathrm{g} \right)\leftrightharpoons2\mathrm{NO}\left( \mathrm{g} \right) + {\mathrm{O}_2}\left( \mathrm{g} \right);{K_2}$

Solid ${Ca}\left({HCO}_3\right)_2$ decomposes as
${Ca}\left({HCO}_3\right)_2({~s}) \rightleftharpoons {CaCO}_3({~s})+{CO}_2({~g})+{H}_2 {O}({g})$

If the total pressure is 0.2 bar at $420 {~K}$, what is the standard free energy change for the given reaction $\left(\Delta_r G^{\circ}\right)$ ?

An aqueous solution of $0.1\;M\;\mathrm{N}{\mathrm{H}_4}\mathrm{Cl}$ will have a $pH$ closer to:

${K}_{{c}}$ for the reaction ${N}_2({~g})+{O}_2({~g}) \rightleftharpoons 2 {NO}({g})$ at $300 {~K}$ is $4.0 \times 10^{-6} \cdot {K}_{{p}}$ for the abovereaction will be $\left({R}=2 {calmol}^{-1} {~K}^{-1}\right)$

The solubility product of $Cr{\left( {OH} \right)_3}$ at 298 K is $6.0 \times {10^{ - 31}}$. The concentration of hydroxide ions in a saturated solution of $Cr{\left( {OH} \right)_3}$ will be

$20 \mathrm{~ml}, 0.1 \mathrm{M}$ HA $\left[\left(\mathrm{K}_{\mathrm{b}}\right)_{\mathrm{A}^{-}}=10^{-10}\right]$ is titrated against $0.2 \mathrm{M}, \mathrm{NaOH}$. Select the correct statement :[Given : $\log 2=0.3, \log 3=0.48$ ]

A dilute solution of $\mathrm{HCl}$ contains $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]=5.4 \times 10^{-7} \mathrm{~mol} \mathrm{~L}^{-1}$ at $298 \mathrm{~K}$. What is the concentration of hydroxyl ions in this solution?

For the Haber’s process for the formation of $\mathrm{N}{\mathrm{H}_3}$ at $\mathrm{298}\;\mathrm{K}$ is :
${\mathrm{N}_2} + 3{\mathrm{H}_2}\;\leftrightharpoons2\mathrm{N}{\mathrm{H}_3};\;\;\Delta H = - 460\;\;\mathrm{kJ}$
Which of the following is correct?

$pH$ of $0.1\;M\;\mathrm{N}{\mathrm{a}_2}\mathrm{HP}{\mathrm{O}_4}$ and $0.2\;M\;\mathrm{Na}{\mathrm{H}_2}\mathrm{P}{\mathrm{O}_4}$ solutions are respectively. $\mathrm{p}{K_a}$ for ${\mathrm{H}_3}\mathrm{P}{\mathrm{O}_4}$ are $2.12,7.21$ and $12.0$ for respective dissociation to ${\mathrm{H}_2}\mathrm{PO}_4^ - ,\mathrm{HPO}_4^{2 - }$ and $\mathrm{PO}_4^{3 - }.$

Morphine $\left(\mathrm{C}_{17} \mathrm{H}_{19} \mathrm{NO}_3\right)$ is administered medically to relieve pain. It is a naturally occurring base or alkaloid. What is the $\mathrm{pH}$ of a $0.0025 \mathrm{~M}$ solution of morphine at $25^{\circ} \mathrm{C}?$ The base-ionization constant $K_{{b}}$ is $1.6 \times 10^{-6}$ at $25^{\circ} \mathrm{C}.$ $(\log 2=0.3)$

$\mathrm{pH}$ of a saturated solution of silver salt of monobasic acid $\mathrm{HA}$ is found to be 9. Select the option(s) which is / are correct. Given : $\mathrm{K}_{\mathrm{a}}(\mathrm{HA})=10^{-10}$
I) Solubility of the silver salt is $1.1 \times 10^{-5} \mathrm{~mol} /$ lit
II) Solubility product of the silver salt is $1.1 \times 10^{-11} \mathrm{~M}^2$
III) Concentration of $\mathrm{Ag}^{+}$ in the solution will be greater than that of $\mathrm{A}^{-}$

The pH of a 0.1 M solution of $\mathrm{N}{\mathrm{H}_4}\mathrm{OH}$ (having ${K_b} = 1.0 \times {10^{ - 5}})$ is equal to

What would be the effect on addition of $\mathrm{CaC}{\mathrm{O}_3}$ on the equilibrium of $\mathrm{CaC}{\mathrm{O}_3}\left( s \right)\;\leftrightharpoons\;\mathrm{CaO}\left( s \right) + \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right)$ in a closed container:

Assertion :- Solubility of ${AgBr}$ decreases in the presence of sodium bromide.

Reason :- Sodium bromide undergoes hydrolysis in water.

The best explanation for the solubility of $\mathrm{MnS}$ in dil.$\mathrm{HCl}$ is that:

For the reaction, $\mathrm{CO}\left( \mathrm{g} \right) + \mathrm{C}{\mathrm{l}_2}\left( \mathrm{g} \right)\;\leftrightharpoons\;\mathrm{COC}{\mathrm{l}_2}\left( \mathrm{g} \right)$ the value of ${K_p}/{K_c}$ is equal to :

The acid ionization constant of ${Zn}^{2+}$ is $2.0 \times 10^{-10}.$ What is the $\mathrm{pH}$ of $0.001 \mathrm{~M}$ solution of ${ZnCl}_2?$ $(\log 2=0.3)$