Equilibrium

The pH of a $0.01\ \mathrm{M}$ aqueous solution of $\mathrm{HCl}$ at $25^\circ\mathrm{C}$ is

Given is a concentrated solution of a weak electrolyte $\mathrm{A_xB_y}$ of concentration 'c' and dissociation constant 'K'. The degree of dissociation is given by :

In a closed flask at 600 K, one mole of $\mathrm{X_2Y_4(g)}$ attains equilibrium as given below : $\mathrm{X_2Y_4(g)}\rightleftharpoons2\mathrm{XY_2(g)}$. At equilibrium, 75% $\mathrm{X_2Y_4(g)}$ was dissociated and the total pressure is 1 atm. The magnitude of $\Delta_rG^\ominus$ (in kJ mol$^{-1}$) at this temperature is ______. (Nearest Integer) (Given : $R=8.3$ J mol$^{-1}$ K$^{-1}$; $\ln10=2.3$, $\log2=0.3$, $\log3=0.48$, $\log5=0.69$, $\log7=0.84$)

The first and second ionization constants of a weak dibasic acid $\mathrm{H_2A}$ are $8.1\times10^{-8}$ and $1.0\times10^{-13}$ respectively. 0.1 mol of $\mathrm{H_2A}$ was dissolved in 1L of 0.1 M HCl solution. The concentration of $\mathrm{HA^-}$ in the resultant solution is :

At 25$^\circ$C, 20.0 mL of 0.2 M weak monoprotic acid HX is titrated against 0.2 M NaOH. The pH of the solution (a) at the start of the titration (when NaOH has not been added) and (b) when 10 mL of NaOH is added respectively, are : Given : $K_a=5\times10^{-4}$, $pK_a=3.3$, $\alpha\ll1$

At T(K), the equilibrium constant of $\mathrm{A_2(g)+B_2(g)\rightleftharpoons C(g)}$ is $2.7\times10^{-5}$. What is the equilibrium constant for $\frac13\mathrm{A_2(g)}+\frac13\mathrm{B_2(g)}\rightleftharpoons\frac13\mathrm{C(g)}$ at the same temperature?

The pH of a solution obtained by mixing 5 mL of 0.1 M $\mathrm{NH_4OH}$ solution with 250 mL of 0.1 M $\mathrm{NH_4Cl}$ solution is ______ $\times10^{-2}$. (Nearest integer) Given: $\mathrm{p}K_b(\mathrm{NH_4OH})=4.74$, $\log2=0.30$, $\log3=0.48$, $\log5=0.70$

20 mL of a solution of acetic acid required 28.4 mL of 0.1 M NaOH for its neutralization. A solution (X) was prepared by mixing 20 mL of the above acetic acid and 14.2 mL of 0.1 M NaOH solution. What is the pH of the solution (X)? ($\mathrm{p}K_a$ value of acetic acid is 4.75).

For the following reaction at 50 °C and at 2 atm pressure, $\mathrm{2N_2O_5(g)\rightleftharpoons2N_2O_4(g)+O_2(g)}$, $\mathrm{N_2O_5}$ is 50% dissociated. The magnitude of standard free energy change at this temperature is $x$. $x=$ ______ J mol$^{-1}$ [Nearest integer]. Given: $R=8.314$ J mol$^{-1}$ K$^{-1}$, log 2 = 0.30, log 3 = 0.48, ln10 = 2.303, °C + 273 = K

$\mathrm{M_3A_2}$ is a sparingly soluble salt of molar mass $y$ g $\mathrm{mol^{-1}}$ and solubility $x$ g $\mathrm{L^{-1}}$. The ratio of the molar concentration of the anion ($\mathrm{A^{3-}}$) to the solubility product of the salt is