pH and ionisation

At a given temperature, 0.45 g of acetic acid in 50 mL of water is shaken with 1.0 g of charcoal and the pH of the resulting solution is 3.0. Assume the adsorption of acetic acid from the aqueous solution by charcoal follows Freundlich isotherm,
$$\frac xm=kC^{1/n}$$
If the plot of $\log_{10}(x/m)$ against $\log_{10}C$ gives a straight line with slope 1, the value of $k$ in L mol$^{-1}$ is ____.

Given: The molar mass of acetic acid is 60 g mol$^{-1}$.
The acid dissociation constant of acetic acid is $1.0\times10^{-5}$ at the given temperature.
$x$ is the mass (in grams) of acetic acid adsorbed.
$m$ is the mass (in grams) of charcoal.
$C$ is the equilibrium concentration of acetic acid in the solution after the adsorption is complete.
$k$ and $n$ are constants for acetic acid-charcoal system at the given temperature.

19.5 g of fluoro acetic acid (molar mass = 78 g mol$^{-1}$) is dissolved in 500 g of water at 298 K. The depression in the freezing point of water was 1 °C. What is $K_a$ of fluoro acetic acid ? (For water, $K_f=1.86$ K kg mol$^{-1}$). Assume molarity and molality to have same values.

The first and second ionization constants of a weak dibasic acid $\ce{H2A}$ are $8.1\times10^{-8}$ and $1.0\times10^{-13}$ respectively. 0.1 mol of $\ce{H2A}$ was dissolved in 1 L of 0.1 M HCl solution. The concentration of $\ce{HA-}$ in the resultant solution is :

Arrange the following resultant mixtures in increasing order of their pH values

A. 10 mL 0.2 M $\ce{Ca(OH)2}$ + 25 mL 0.1 M HCl

B. 10 mL 0.01 M $\ce{H2SO4}$ + 10 mL 0.01 M $\ce{Ca(OH)2}$

C. 10 mL 0.1 M $\ce{H2SO4}$ + 10 mL 0.1 M KOH

Choose the correct answer from the options given below:

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

At 25 °C, the concentration of $\ce{H+}$ ions in $1.00\times10^{-3}$ M aqueous solution of a weak monobasic acid having acid dissociation constant ($K_a$) of $4.00\times10^{-11}$ is $\boldsymbol{X}\times10^{-7}$ M. The value of $\boldsymbol{X}$ is _____.

Use: Ionic product of water $(K_w) = 1.00\times10^{-14}$ at 25 °C

Plotting $1/\Lambda_\mathrm{m}$ against $c\Lambda_\mathrm{m}$ for aqueous solutions of a monobasic weak acid (HX) resulted in a straight line with y-axis intercept of P and slope of S. The ratio $\mathrm{P}/\mathrm{S}$ is

[$\Lambda_\mathrm{m}$ = molar conductivity; $\Lambda^\circ_\mathrm{m}$ = limiting molar conductivity; c = molar concentration; $K_\mathrm{a}$ = dissociation constant of HX]

Concentration of $\ce{H2SO4}$ and $\ce{Na2SO4}$ in a solution is 1 M and $1.8 \times 10^{-2}$ M, respectively. Molar solubility of $\ce{PbSO4}$ in the same solution is $X \times 10^{-Y}$ M (expressed in scientific notation). The value of $Y$ is ________.

[Given: Solubility product of $\ce{PbSO4}$ $(K_{sp}) = 1.6 \times 10^{-8}$. For $\ce{H2SO4}$, $K_{a1}$ is very large and $K_{a2} = 1.2 \times 10^{-2}$]

The cell potential for the following cell
$$\mathrm{Pt\,|H_2(g)|H^+(aq)\,||\,Cu^{2+}(0.01\ M)|Cu(s)}$$
is 0.576 V at 298 K. The pH of the solution is ______. (Nearest integer)

(Given : $E^\circ_{\mathrm{Cu^{2+}/Cu}}=0.34$ V and $\dfrac{2.303RT}F=0.06$ V)

pH value of 0.001 M NaOH solution is ______.

$K_a$ for butyric acid $(\mathrm{C_3H_7COOH})$ is $2\times10^{-5}$. The pH of 0.2 M solution of butyric acid is ______ $\times10^{-1}$. (Nearest integer)

[Given log 2 = 0.30]

200 mL of 0.01 M HCl is mixed with 400 mL of 0.01 M H$_2$SO$_4$. The pH of the mixture is _______.

Given: log 2 = 0.30, log 3 = 0.48, log 5 = 0.70, log 7 = 0.84, log 11 = 1.04

The value of $\alpha$ is ____.

The value of $\mathbf y$ is ____.

When 9.45 g of ClCH$_2$COOH is added to 500 mL of water, its freezing point drops by 0.5°C. The dissociation constant of ClCH$_2$COOH is $x\times10^{-3}$. The value of $x$ is _______. (Rounded off to the nearest integer)

[$K_{f(\mathrm{H_2O})}$ = 1.86 K kg mol$^{-1}$]

The structure of a peptide is given below.

If the absolute values of the net charge of the peptide at pH = 2, pH = 6, and pH = 11 are $|z_1|$, $|z_2|$, and $|z_3|$, respectively, then what is $|z_1| + |z_2| + |z_3|$?

The conductance of a 0.0015 M aqueous solution of a weak monobasic acid was determined by using a conductivity cell consisting of platinized Pt electrodes. The distance between the electrodes is 120 cm with an area of cross section of $1\ \mathrm{cm^2}$. The conductance of this solution was found to be $5 \times 10^{-7}$ S. The pH of the solution is 4. The value of limiting molar conductivity $(\Lambda_m^o)$ of this weak monobasic acid in aqueous solution is $Z \times 10^2\ \mathrm{S\,cm^{-1}\,mol^{-1}}$. The value of $Z$ is

The molar conductivity of a solution of a weak acid HX (0.01 M) is 10 times smaller than the molar conductivity of a solution of a weak acid HY (0.10 M). If $\lambda^0_{\ce{X-}}\approx\lambda^0_{\ce{Y-}}$, the difference in their $\mathrm pK_a$ values, $\mathrm pK_a(\ce{HX})-\mathrm pK_a(\ce{HY})$, is (consider degree of ionization of both acids to be $\ll1$)

Assuming that the degree of hydrolysis is small, the pH of 0.1 M solution of sodium acetate ($K_a=1.0\times10^{-5}$) will be :

The initial rate of hydrolysis of methyl acetate (1 M) by a weak acid (HA, 1 M) is 1/100$^\text{th}$ of that of a strong acid (HX, 1 M), at 25 °C. The $K_a$ of HA is