The solubility product of a sparing soluble salt AX₂ is $3.2\times {10}^{-11}$. Its solubility (in mol L^-1) is

An acid solution of 0.005 M has a pH of 5. The degree of ionization of acid is

pKa value of four acids are given below. The strongest acid is

(I) 4.0

(II) 3.5

(III) 2.5

(IV) 2

A solution has hydrogen ion concentration 0.0005 M, its pOH is

At 25°C, the pH of a solution containing 0.10 M sodium acetate and 0.03 M acetic acid will be:

[pK_a value of ${\mathrm{CH}}_3\mathrm{COOH}=4.57$]-

Ionization constant of acetic acid is $1.8\times {10}^{-5}$. The concentration of H⁺ ions in 0.1 M solution is

The dissociation constant of a weak acid is $4.9\times {10}^{-8},$ its percentage ionization at 0.1 M is

The pH of a 0.1 M aqueous solution of a weak acid (HA) is 3. What is its degree of dissociation?

75 ml of 0.2 M HCl is mixed with 25 ml of 1M HCl. To this solution, 300 ml of distilled water is added. What is the pH of the resultant solution?

The dissociation constant of two acids HA₁ and HA₂ are $3.0\times {10}^{-4}$ and $1.8\times {10}^{-5}$ respectively. The relative strengths of the acids is

0.005 M acid solution has 5 pH. The percentage ionization of acid is

100 ml of 0.015 M HCl solution is mixed with 100 ml of 0.005 M HCl. What is the pH of the resultant solution?

The solubility product of A₂X₃ is $1.08\times {10}^{-23}$. Its solubility will be

M(OH) x has ${\mathrm{K}}_{\mathrm{sp}}=4\times {10}^{-12}$ and solubility 10^-4 M, x is

The pH values of 1 M solutions of CH₃COOH (I), CH₃COONa (II), CH₃COONH₄ (III), and KOH (IV) will be in the order

What should be the ratio of the concentration of salt and acid for preparing a buffer solution of pH 6 by mixing sodium acetate and acetic acid?(Ka=10^-5)

The strongest Bronsted base among the following ions is

The degree of ionization of water was found to be $1.8\times {10}^{-9}$. The ${\mathrm{K}}_{\mathrm{a}}$ (ionization constant) of water is

The decreasing order of acidic nature of ${\mathrm{H}}_2{\mathrm{SO}}_4 \left(\mathrm{I}\right), {\mathrm{H}}_3{\mathrm{PO}}_4 \left(\mathrm{II}\right), \mathrm{and} {\mathrm{HClO}}_4 \left(\mathrm{III}\right)$ is

The number of H⁺ ions present in 1cm³ of a solution whose pH is 10 is

The Ka value of formic acid and acetic acid are respectively $1.77\times {10}^{-4}$ and $1.75\times {10}^{-5}$. The ratio of the acid strength of 0.1 N acids is

ZnS is not precipitated by passing H₂S in an acidic medium but CuS is precipitated. The reason for it is

Consider the following acids:

I. HCN

II. CH₃COOH

III. HCOOH

IV. Cl-CH₂COOH

The correct order of strength is

The hydrogen ion concentration is 0.2 M ethanoic acid $({\mathrm{K}}_{\mathrm{C}}=2\times {10}^{-5} \mathrm{mol} {\mathrm{dm}}^{-3})$ is approximately

The pH of a solution made by mixing 50 mL of 0.01 M barium hydroxide solution with 50 mL of H₂O is

Find the molar solubility of Fe(OH)₃ in a buffer solution that 0.10 M in NH₄Cl and 0.10 M in NH₃. If ${\mathrm{K}}_{\mathrm{b}} \left({\mathrm{NH}}_3\right)=1.8\times {10}^{-5}$ and ${\mathrm{K}}_{\mathrm{sp}} \left[\mathrm{Fe}{\left(\mathrm{OH}\right)}_3\right]=2.6\times {10}^{-39}.$

A base dissolved in water yields a solution with a hydroxyl ion concentration of 0.05 mol litre^-1. The solution is

Ionization constant of CH₃COOH is $1.7\times {10}^{-5}$ and concentration of H⁺ ion is $3.4\times {10}^{-4}$. Then initial concentration of CH₃COOH is

At $25°\mathrm{C}$ the dissociation constant of a base, BOH is $1.0\times {10}^{-12}$, the concentration of hydroxyl ions 0.01 M aqueous solution of the base would become

The solubility product of AgI at $25°\mathrm{C}$ is $1.0\times {10}^{-16} {\mathrm{mol}}^2 {\mathrm{L}}^{-2}$. The solubility of AgI in 10^-4 N solution of KI at $25°\mathrm{C}$ is :  (in mol L^-1)

When 0.1 mole of CH₃NH₂ (ionization constant ${\mathrm{K}}_{\mathrm{b}}=5\times {10}^{-4}$) is mixed with 0.08 mol HCl and the volume is made up of 1 litre. The [H⁺] of resulting solution is -

(log 4 =  0.60)

Which of the following solutions will have a pH value that is close to 1.0?

If ${\mathrm{Ag}}^{+}+2{\mathrm{NH}}_3\rightleftharpoons \mathrm{Ag}{{\left({\mathrm{NH}}_3\right)}_2}^{+}; {\mathrm{K}}_1=1.8\times {10}^7$

${\mathrm{Ag}}^{+}+{\mathrm{Cl}}^{-}\rightleftharpoons \mathrm{AgCl}; {\mathrm{K}}_2=5.6\times {10}^9$

Then for

$\mathrm{AgCl}+2{\mathrm{NH}}_3\rightleftharpoons {\left[\mathrm{Ag}{\left({\mathrm{NH}}_3\right)}_2\right]}^{+}+{\mathrm{Cl}}^{-},$

Equilibrium constant will be

2. $3.11\times {10}^2$

There sparingly soluble saltrs A₂X, AX and AX₃ have the same solubility product.Their solubilities will be in the order

Which of the following solution(s) have pH between 6 and 7?

I. $2\times {10}^{-6} \mathrm{M}\hspace{0.17em}\mathrm{NaOH}$

II. $2\times {10}^{-6} \mathrm{M}\hspace{0.17em}\mathrm{HCL}$

III. ${10}^{-8} \mathrm{M}\hspace{0.17em}\mathrm{HCl}$

IV. ${10}^{-13} \mathrm{M}\hspace{0.17em}\mathrm{NaOH}$

What is the pH value at which Mg(OH)₂ begins to precipitate from a solution containing 0.10 M Mg⁺² ion? Ksp of Mg(OH)₂ is $1\times {10}^{-11}.$

50 litres of 0.1 M HCl are mixed with 50 litres of 0.2 M NaOH. The pH of the resulting solution is

The pH of a 0.05 M aqueous solution of diethylamine is 12. Its K_b value will be:

K_a for HCN is $5\times {10}^{-10}$ at $25°\mathrm{C}$. For maintaining a constant pH of 9, the volume of 5 M KCN solution required to be added to 10 mL of 2 M HCN solution is-

The approximate pH of a solution formed by mixing equal volumes of solutions of 0.1 M sodium propionate and 0.1 M propanoic acid (the dissociation constant of propanoic acid is $1.3\times {10}^{-5} \mathrm{mol} {\mathrm{dm}}^{-3}$) will be

The dissociation constant of acetic acid is $1.6\times {10}^{-5}$. The degree of dissociation $\left(\mathrm{\alpha }\right)$ of 0.01 M acetic acid in the presence of 0.1 M HCl is equal to

If the equilibrium constant of the reaction of weak acid HA with strong base is 10⁹, then pH of 0.1 M NaA is

If Ksp of Al(OH)₃ is $1.0\times {10}^{-15} \mathrm{M}.$ Find at what pH does $1.0\times {10}^{-3} \mathrm{M}$ Al³⁺ precipitate on the addition of buffer of NH₄Cl and NH₄OH solution.

The solubility of CaF₂ in water at 298 K is $1.7\times {10}^{-3}$ gm per 100 cm³. The solubility product of CaF₂ at 298 K is

A solution of monoprotic weak acid has acidity constant K_a the minimum intial concentration 'c' in terms of K_a, such that the concentration of the undissociated acid can be equated to 'c' within a 10% limit of error, would be

The solubility product of PbI₂ is $7.47\times {10}^{-9}$ at $15°\mathrm{C}$ and $1.39\times {10}^8$ at $25°\mathrm{C}$. The molar heat of solution of PbI₂ is (use log 1.86=0.2695)

Which of the following compounds is in the correct sequence in terms of relative basic strength?

The concentration of CH₃COOH that will have the same [H⁺] as obtained from 10^-2 M HCOOH, is-

$\left(\mathrm{Ka}\right({\mathrm{CH}}_3\mathrm{COOH})={10}^{-5}, \mathrm{Ka}(\mathrm{HCOOH})={10}^{-4})$

When NH₄Cl is added to an aqueous solution of NH₄OH, then

500 ml of 0.2 M HCl is mixed with 500 ml of 0.2 M CH₃COOH. 25 ml of the mixture is titrated with 0.1 M NaOH solution. By how many units does the pH change from the start to the stage when HCl is just completely neutralized. K_a for acetic acid$=2.0\times {10}^{-5}$.