Equilibrium practice · Mixed difficulty

pH of 0.2 M aqueous solution of sodium benzoate will be ($P{K_a}$ of benzoic acid = 4.2)

Assertion : In the titration of ${Na}_2 {CO}_3$ with ${HCl}$ using methyl orange indicator, the volume required at the equivalence point is twice that of the acid required using phenolphthalein indicator.

Reason : Two moles of ${HCl}$ are required for the complete neutralization of one mole of ${Na}_2 {CO}_3$

The concentration of $\mathrm{C}{\mathrm{O}_2}$ be in equilibrium with $2.5 \times {10^{ - 2}}\;\mathrm{mol}\;\mathrm{ litr}{\mathrm{e}^{ - 1}}\;\mathrm{of }\;\mathrm{CO}\;\mathrm{at}\,\,100^\circ C$ for the reaction : $\mathrm{FeO}\left( s \right)\; + \,\,\mathrm{CO}\left( \mathrm{g} \right)\;\,\leftrightharpoons\;\mathrm{Fe}\left( s \right) + \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right);\;{K_c} = 5.0$

STATEMENT I : pH value of acidic buffer solution change, k if bufler solution is diluted upto very larger extent.

STATEMENT II : $\left[H^{+}\right]$ decrease due to change in concentration as well as $\alpha$ and decrease in concentration is more as compare to increase in $\alpha$.

The equilibrium concentrations of the species in the reaction $A+B \rightleftharpoons C+D$ are $2,3,10$ and $6 \mathrm{~mol} \mathrm{~L}^{-1}$, respectively at $300 \mathrm{~K}$. $\Delta \mathrm{G}^{\circ}$ for the reaction is $(R=2 \, \mathrm{cal} / \mathrm{mol} \, \mathrm{K})$

Acidosis is diagnosed when blood $\mathrm{pH}$:

$100\;\mathrm{ }mL\;\mathrm{ }of\;\mathrm{ }0.01\mathrm{ }M$ solution of $\mathrm{NaOH}$ is diluted to $1\;\mathrm{d}{\mathrm{m}^3}$. What is the pH of the diluted solution?

The decreasing order of strength of the bases,

$\mathrm{O}{\mathrm{H}^ - },\mathrm{NH}_2^ - ,\mathrm{H}-\mathrm{C} \equiv {\mathrm{C}^ - }\;and\;\mathrm{C}{\mathrm{H}_3}-\mathrm{CH}_2^ - ,\;is$

(A): In polybasic acids $K_{a_2}$ is always smaller than $K_{a_1}$

(R): Second dissociation takes place to a much smaller extent than the first dissociation.

${\mathrm{H}_2}\mathrm{S}$ is passed into one $\mathrm{d}{\mathrm{m}^3}$ of a solution containing $0.1\;\mathrm{mole}\;\mathrm{ of }\;\mathrm{Z}{\mathrm{n}^3}\mathrm{ \;and}\;0.01\;\mathrm{mole }\;\mathrm{of}\;\mathrm{ C}{\mathrm{u}^2}$  till the sulphide ion concentration reaches $8.1\; \times \;{10^{10}}$ moles. Which one of the following statements is true? [${K_{\mathrm{sp}}}$ of $\mathrm{Zn}$ and $\mathrm{CuS}$ $\mathrm{are}\;3\; \times {10^{22}}\;\mathrm{and}\;8\; \times {10^{36}}$ respectively]

The internal and external indicator among the following respectively are:

Which of the following will supress the ionisation of acetic acid is aqueous solution?

Although $\mathrm{CO}$ is neutral but it shows acidic nature on reaction with high $P$ and $T$:

The Henderson’s equation used to calculate the $\mathrm{pOH}$ of basic buffer is:

Acidity of $B{F_3}$ can be explained on the basis of which of the following concept

Arrange $\mathrm{NH}_4^ + ,{\mathrm{H}_2}\mathrm{O},{\mathrm{H}_3}{\mathrm{O}^ + },\mathrm{HF }\;\mathrm{and}\;\mathrm{ O}{\mathrm{H}^ - }$ in increasing order of acidic nature

4 moles of A is mixed with 4 moles of B, at equilibrium for the reaction $A + BC + D$, 2 moles of C and D is formed. The equilibrium constant for the reaction will be

In a reaction at equilibrium $'X'$ mole of the reactant $A$ decompose to give $1\;mole$ each of $C\;and\;D$ . If the fraction of $A$ decomposed at equilibrium is independent of initial concentration of $A$, then the value of $'X'$ is :

For exothermic reaction, if we change temperature from $70^{\circ} \mathrm{C}$ to $40^{\circ} \mathrm{C}$ then $\mathrm{K}_{\mathrm{C}}$ will:

Which of the following has ${P^H}$ is equal to near about one

What is equilibrium expression for the reaction, ${P_4}(s) + 5{O_2}(g)\leftrightharpoons{P_4}{O_{10}}(s)\,\,?$

Equimolar solutions of the following were prepared in water separately. Which one of the solutions will record the highest $pH$?

For the system; $3A + 2B\leftrightharpoons\;C$,the expression for equilibrium constant is

According to Arrhenius concept, base is a substance that:

A higher value for equilibrium constant, $K$ shows that:

A cylinder fitted with a movable piston contains liquid water in equilibrium with water vapour at 250C. Which operation result in a decrease in the equilibrium vapour pressure?

Assertion : $S O_2(g)+\frac{1}{2} O_2(g) \rightleftharpoons S O_3(g)+$ heat.
Forward reaction is favoured at high temperature and low pressure.

Reason : Reaction is exothermic.

The equilibrium constant for the reaction between $C{H_4}\left( g \right)$ and ${H_2}S\left( g \right)$ to form $C{S_2}\left( g \right)$ and ${H_2}\left( g \right)$ , at 1173 K is 3.6. For the following composition of the reaction mixture, $\left[ {C{H_4}} \right] = 1.0\,M,\,\left[ {{H_2}S} \right] = 1.20M\,\,\,\left[ {C{S_2}} \right] = 2.0M,\,\,\left[ {{H_2}} \right] = 1.8M$ decide which of the following option is correct? $\left[ {C{H_4}\left( g \right) + 2{H_2}S\left( g \right)C{S_2}\left( g \right) + 4{H_2}\left( g \right)} \right]$

The $\mathrm{pH}$ of a $\mathrm{0}\mathrm{.02}\;\mathrm{M}$ solution of hydrochloric acid is:

4.5 moles each of hydrogen and iodine heated in a sealed 10 L vessel. At equilibrium 3 moles of HI were found. The equilibrium constant for ${\mathrm{H}_2}\left( \mathrm{g} \right) + {\mathrm{I}_2}\left( \mathrm{g} \right)\leftrightharpoons2\mathrm{HI}\left( \mathrm{g} \right)$ is