$\mathrm{K}_{\mathrm{a}}$ for $\mathrm{CH}_3 \mathrm{COOH}$ is $1.8 \times 10^{-5}$ and $\mathrm{K}_{\mathrm{b}}$ for $\mathrm{NH}_4 \mathrm{OH}$ is $1.8 \times 10^{-5}$. The pH of ammonium acetate will be

Which of the following options will be correct for the stage of half completion of the reaction $\mathrm{A} \rightleftharpoons \mathrm{B}$ ?

On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le-Chatelier's principle. Consider the reaction,

$$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})$$

Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?

What will be the correct order of vapour pressure of water, acetone and ether at $30^{\circ} \mathrm{C}$ ? Given that among these compounds, water has maximum boiling point and ether has minimum boiling point?

At 500 K , equilibrium constant, $\mathrm{K}_{\mathrm{c}}$, for the following reaction is 5.

$$\frac{1}{2} \mathrm{H}_2(\mathrm{~g})+\frac{1}{2} \mathrm{I}_2(\mathrm{~g}) \rightleftharpoons \mathrm{HI}(\mathrm{g})$$

What would be the equilibrium constant $\mathrm{K}_{\mathrm{c}}$ for the reaction?

$$2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_2(\mathrm{~g})+\mathrm{I}_2(\mathrm{~g})$$