Ionic Equilibrium

A weak monobasic acid is $4\%$ dissociated in $0.05$ M solution. What is percent dissociation in $0.1$ M solution ?

Calculate the pOH of $0.01$ M monobasic acid that is completely dissociated, at $298$ K.

What is the normal pH range of human blood?

What is the pH of 1 molar HCl solution? (assume complete dissociation)

Calculate the pH of buffer solution containing 0.1M $\text{CH}_3\text{COOH}$ and 0.1 M $\text{CH}_3\text{COONa}$ $[K_a = 1.8 \times 10^{-5}]$

There are two different solutions, A and B. The pH of solution A is 4. Find the pH of solution B having $[\text{H}^+]$ three times that of solution A.

What is the pH of solution containing $5 \times 10^{-4}\ \text{M}\ \text{H}^+$ ion?

A weak base is $1.3\%$ dissociated in its aqueous solution. If $K_b$ for weak base is $1.69 \times 10^{-5}$ at $298$ K. Find the concentration of aqueous solution of weak base.

Calculate the molar concentration of weak monobasic acid if $K_a = 1.8 \times 10^{-5}$ and degree of dissociation is $0.01$ ?

If $[\text{H}_3\text{O}^+]$ of a solution is $1 \times 10^{-4}$. What is the value of pOH at $298\,\text{K}$ ?

Calculate the $[\text{H}_3\text{O}^+]$ if pH of the solution is $4.25$

Identify the conjugate bases of $\text{H}_3\text{PO}_3$ and $\text{H}_2\text{SO}_4$ respectively from following.

What is the molarity of $\text{H}_2\text{SO}_4$ solution having $\text{pH} = 4$ ?

The solubility of a sparingly soluble a salt $\text{AB}_2$ is $1 \times 10^{-6}\ \text{mol/dm}^3$. Calculate its solubility product?

Which of the following is Lewis acid?

Which of the following aqueous salt solutions has the least pH value ?

An organic monobasic acid has dissociation constant $1.96 \times 10^{-8}$. What is its percentage dissociation in $0.01$ M solution ?

The solubility of salt $\text{AX}_2$ is $6 \times 10^{-12}\ \text{mol dm}^{-3}$. What is solubility product of the salt ?

Which from following salts does not undergo hydrolysis ?

Calculate the solubility in mol $\text{dm}^{-3}$ of sparingly soluble salt BA at 293 K if its solubility product is $8.56 \times 10^{-5}$ at same temperature.

Which of the following is correct relationship between solubility and solubility product for silver oxalate ?

What is the pH of resulting solution when $20 \text{ mL } \dfrac{M}{10} \text{ NaOH}$ and $10 \text{ mL } \dfrac{M}{10} \text{ H}_2\text{SO}_4$ are mixed together ?

The solubility of sapringly soluble salt $\text{AB}_2$ is $18 \cdot 78 \times 10^{-4} \text{ g/dm}^3$ What is its solubility product ? (Molar mass of $\text{AB}_2 = 187 \cdot 8 \text{ g mol}^{-1}$)

Identify from following a weak electrolyte based on their dissociation nature in aqueous medium.

The solubility of AgCl in 0.1 M NaCl is S mol/L. If the solubility product of AgCl is $1.8 \times 10^{-10}$, then S is approximately:

The solubility product of a sparingly soluble salt BA is $6.4 \times 10^{-13}$. Calculate it's solubility in $\text{g dm}^{-3}$ .Molar mass of salt is $190\ \text{g mol}^{-1}$ .

Identify from the following salts an example of a salt of strong acid and weak base.

Which of the following salt undergoes anionic hydrolysis ?

The solubility product of sparingly soluble salt BA is $4 \times 10^{-13}$. Calculate the $[\text{A}^-]$ if $[\text{B}^+]$ is $1 \times 10^{-6}\ \text{M}$.

Identify the strongest base according to Bronsted-Lowry theory from following.

The solubility of sparingly soluble salts $\text{MX}_1$, $\text{MX}_2$ and $\text{MX}_3$ is $1 \times 10^{-3}$ mol/L. Hence, their respective solubility products are

The dissociation constant of weak acid HA is $1.5 \times 10^{-5}$. Find the percent dissociation, containing $0.2$ moles per $2$ liters of solution.

Identify from following the conjugate base of $[\text{Zn}(\text{H}_2\text{O})_4]^{2+}$

Calculate pOH of 0.001M HCl solution.

What is the solubility product of binary sparingly soluble salt BA if 100 mL saturated solution of salt consist $10^{-4}$ moles at room temperature?

Which of the following sentences is true for a basic solution?

What is the relationship between the degree of dissociation of a weak base and its concentration?

A weak monobasic acid is 0.04 % dissociated in 0.25 M solution. What is pH of the solution?

What is the concentration of hydrogen ion in the solution when the concentration of hydroxyl ion is $0.08$ mol / dm$^3$ at $298$ K ?

Find the pH of a solution formed by mixing equal volume of solution of $0.1$ M sodium propionate and $0.1$ molar propionic acid.(Given The dissociation constant of propionic acid is $1.3 \times 10^{-5}$)

Match List I with List IIList I(Buffers)List II(Applications)(A) $\text{HCO}_3^{-1} + \text{H}_2\text{CO}_3$(I) Maintain the pH of blood forms $7.36$ to $7.42$(B) Phosphates(II) In Medicine(C) Sodium Citrate(III) In Qualitative analysis of ...

What happens when $\text{CuSO}_4$ is dissolved in water?Identify correct statements from the following

What happens when solid $\text{Na}_2\text{CO}_3$ dissolved in water?

Which of the following aqueous solution of salt have $pH < 7$ at $298$ K?

What is the normal pH of human blood?

What is the solubility of $\text{BaSO}_4$ in g /$\text{dm}^3$ if its solubility product is $1.0 \times 10^{-10}$ at $25^\circ$C. [Molar mass of $\text{BaSO}_4 = 233$ g/mol]

$2.8$ g of KOH is dissolved in a $500$ mL solution at $298$ K. What is the $p^H$ of solution ? (molar mass of KOH = $56$ g/mol)

Calculate the ionisation constant of $0.08 \mathrm{~mol} \mathrm{dm}{ }^{-3}$ of a monobasic acid having $\mathrm{pH}=2$.

Identify conjugate acid and conjugate base for $\mathrm{HCO}_3^{-}$ion respectively

Find the concentration of sodium acetate when added to 0.1 M solution of acetic acid to form a buffer solution of $\mathrm{pH}=5.5$ ?
( $\mathrm{pK}_{\mathrm{a}}$ of $\mathrm{CH}_3 \mathrm{COOH}=4.5$ )