Equilibrium

The numerical value of the equilibrium constant $K$ depends on:

For the reaction $PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$, what are the units of $K_c$?

The reaction quotient $Q_c$ is used to:

If the reaction $2A + B \rightleftharpoons C$ has an equilibrium constant $K$, then the reaction $C \rightleftharpoons 2A + B$ has a constant:

For the reaction $A(g) \rightleftharpoons 2B(g)$, $K_p$ is $4\,atm$ at a certain temperature. If the equilibrium partial pressure of $B$ is $2\,atm$, what is the equilibrium partial pressure of $A$?

If $\Delta n = 0$ for a gaseous reaction, which of the following is always true regarding the units of $K_p$ and $K_c$?

What is the unit of $K_c$ for the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$?

For the decomposition of $Ag_2O(s) \rightleftharpoons 2Ag(s) + 0.5O_2(g)$, the value of $K_p$ is equal to:

If the degree of dissociation of $PCl_5$ is $0.5$ at $1$ atm, find the pressure at which it will be $0.7$ dissociated at the same temperature.

The $K_c$ for $A + B \rightleftharpoons C + D$ is $49$. If $1$ mole of each $A$ and $B$ are taken in a $1$ L vessel, what is the equilibrium concentration of $D$?

In the reaction $H_2(g) + Cl_2(g) \rightleftharpoons 2HCl(g)$, the effect of increasing the concentration of $Cl_2$ is to:

What is the result of adding more $CaO(s)$ to the equilibrium $CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)$?

For the equilibrium $2H_2(g) + CO(g) \rightleftharpoons CH_3OH(g)$, what happens to the equilibrium if the volume is halved?

Le Chatelier's Principle can be applied to which of the following?

In the equilibrium $2A(g) \rightleftharpoons B(g) + C(g)$, how will the concentration of $B$ change if the pressure is increased by reducing the volume?

For the equilibrium $CH_4(g) + 2S_2(g) \rightleftharpoons CS_2(g) + 2H_2S(g)$, if the concentration of $S_2$ is increased, the concentration of $H_2S$ will:

The formation of $NO_2$ from $NO$ and $O_2$ is exothermic: $2NO(g) + O_2(g) \rightleftharpoons 2NO_2(g)$. If the reaction mixture is cooled, the color of the gas (assuming $NO_2$ is brown and $NO$ is colorless):

In the auto-ionization of water $2H_2O(l) \rightleftharpoons H_3O^+(aq) + OH^-(aq)$, the process is endothermic. If the temperature is increased from $25^{\circ}C$ to $60^{\circ}C$, the water will:

For the reaction $XeF_6(g) + H_2O(g) \rightleftharpoons XeOF_4(g) + 2HF(g)$, the equilibrium is established. If the volume of the reaction vessel is doubled, the equilibrium will shift:

When a catalyst is added to a system at equilibrium, the equilibrium constant:

Which of the following is a Lewis acid?

What happens to the $pH$ of water if we increase the temperature?

Which of the following is a property of a buffer solution?

The concentration of $OH^-$ ions in a solution with $pOH = 4$ is:

If the $K_a$ of a weak acid is $1.0 \times 10^{-5}$, what is the $pOH$ of its $0.1 M$ solution?

Which of the following acts as a buffer in the presence of $NaOH$?

The $pH$ of a solution is 3.0. How many times is the $H^+$ ion concentration higher than that of a solution with $pH$ 6.0?

The ionic product of water at $60^{\circ} C$ is $9.6 \times 10^{-14}$. A solution with $pH = 7$ at this temperature is:

Calculate the concentration of $OH^-$ in a $0.1\text{ M}$ solution of $NaOC_6H_5$ (Sodium Phenoxide). (Given $K_a$ for Phenol = $1.0 \times 10^{-10}$)

What happens to the $pH$ of a buffer solution of $NH_4OH$ and $NH_4Cl$ when a small amount of $HCl$ is added?

If the $pH$ of a solution increases from 3 to 4, the $[H^+]$ concentration:

Solubility product $K_{sp}$ of a salt depends on:

The numerical value of $pH$ for a $0.1\ M$ strong monobasic acid is:

What is the $pOH$ of a solution whose $pH$ is 4.5 at $298\ K$?

If the $pH$ of a saturated solution of $M(OH)_2$ is $12$, then its $K_{sp}$ is:

What is the $pH$ of $0.1\ M$ acetic acid ($K_a = 1.8 \times 10^{-5}$)?

The solubility of $AgCl$ in $0.1\ M\ NaCl$ is much lower than in pure water. This is because:

Calculate the $pH$ of a $0.01\ M\ NH_4OH$ solution which is $5\%$ ionized.

A buffer solution is prepared by mixing $10\ mL$ of $1.0\ M\ CH_3COOH$ and $20\ mL$ of $0.5\ M\ CH_3COONa$. If the solution is diluted to $100\ mL$, the $pH$ will:

If the $pH$ of a saturated solution of $M(OH)_3$ is $9.0$, what is the $K_{sp}$ of $M(OH)_3$?