Ionic Equilibrium

If the solubility product of PbS is $8\times10^{-28}$, then the solubility of PbS in pure water at 298 K is $x\times10^{-16}$ mol L$^{-1}$. The value of $x$ is _______. (Nearest Integer)

[Given : $\sqrt2$ = 1.41]

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

A compound 'X' is a weak acid and it exhibits colour change at pH close to the equivalence point during neutralization of NaOH with CH$_3$COOH. Compound 'X' exists in ionized form in basic medium. The compound 'X' is

50 mL of 0.1 M CH$_3$COOH is titrated against 0.1 M NaOH solution. When 10 mL of NaOH is added, the pH of the solution becomes _______ $\times10^{-1}$. (nearest integer)

Given: pKa (CH$_3$COOH) = 4.8, log 2 = 0.3

The value of $|\mathbf y|$ is ____.

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$^{-1}$]

5.00 mL of 0.10 M oxalic acid solution taken in a conical flask is titrated against NaOH from a burette using phenolphthalein indicator. The volume of NaOH required for the appearance of permanent faint pink color is tabulated below for five experiments. What is the concentration, in molarity, of the NaOH solution?

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 $|z_1| + |z_2| + |z_3|$?

A solution of 0.1 M weak base (B) is titrated with 0.1 M of a strong acid (HA). The variation of pH of the solution with the volume of HA added is shown in the figure below. What is the p$K_b$ of the base? The neutralization reaction is given by $\ce{B + HA -> BH+ + A-}$.

An acidified solution of 0.05 M $\ce{Zn^{2+}}$ is saturated with 0.1 M $\ce{H2S}$. What is the minimum molar concentration (M) of $\ce{H+}$ required to prevent the precipitation of ZnS?

Use $K_{sp}(\ce{ZnS}) = 1.25\times10^{-22}$ and overall dissociation constant of $\ce{H2S}$, $K_{\text{NET}} = K_1K_2 = 1\times10^{-21}$.

For the following reaction, the equilibrium constant $K_c$ at 298 K is $1.6\times10^{17}$.

$$\ce{Fe^{2+}(aq) + S^{2-}(aq) <=> FeS(s)}$$

When equal volumes of 0.06 M $\ce{Fe^{2+}}(aq)$ and 0.2 M $\ce{S^{2-}}(aq)$ solutions are mixed, the equilibrium concentration of $\ce{Fe^{2+}}(aq)$ is found to be $Y\times10^{-17}$ M. The value of $Y$ is ______

The solubility of a salt of weak acid (AB) at pH 3 is $\mathbf Y\times10^{-3}$ mol L⁻¹. The value of Y is ______.

(Given that the value of solubility product of AB ($K_{sp}$) = $2\times10^{-10}$ and the value of ionization constant of HB ($K_a$) = $1\times10^{-8}$)

Dilution processes of different aqueous solutions, with water, are given in LIST-I. The effects of dilution of the solutions on $[\mathrm{H^+}]$ are given in LIST-II.

(Note: Degree of dissociation ($\alpha$) of weak acid and weak base is $\ll 1$; degree of hydrolysis of salt $\ll 1$; $[\mathrm{H^+}]$ represents the concentration of $\mathrm{H^+}$ ions)

Match each process given in LIST-I with one or more effect(s) in LIST-II. The correct option is

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

p$K_a$ of a weak acid (HA) and p$K_b$ of a weak base (BOH) are 3.2 and 3.4, respectively. The pH of their salt (AB) solution is :

In the following reactions, ZnO is respectively acting as a/an :

(a) $\ce{ZnO + Na2O -> Na2ZnO2}$

(b) $\ce{ZnO + CO2 -> ZnCO3}$

Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of pH 6. If ionisation constant of HA is $10^{-5}$, the ratio of salt to acid concentration in the buffer solution will be :

50 mL of 0.2 M ammonia solution is treated with 25 mL of 0.2 M HCl. If $pK_b$ of ammonia solution is 4.75, the pH of the mixture will be :