List of top Chemistry Questions on Ionic Equilibrium In Solution

Identify the correct statements from the following I) \[ \text{Conjugate base of nitrous acid is } NO_2^{-} \] II) \[ \text{The concentration of } OH^{-} \text{ ions in } 0.1\,M \text{ aqueous pyridine solution is } \sqrt{2}\times10^{-5}\,M \] \[ (K_b \text{ of pyridine }=2\times10^{-9}) \] III) The acid strength of aqueous hydrogen halides follows \[ HF \gt HCl \gt HBr \gt HI \]

Which of the following is a conjugate acid-base pair?

The pH of a $0.01\text{ M NaOH}$ solution is}

The pH of \(0.01\) M aqueous aniline solution at \(298\) K is \(8.3\). Its degree of dissociation \((\alpha)\) is \[ (K_b\text{ of aniline}=4\times10^{-10}; \ \text{antilog}(0.7)=5.0; \ \text{antilog}(0.3)=2.0; \ \text{antilog}(0.4)=2.5) \]

The solubility of \(BaCO_3\) (molar mass \(197\,g\,mol^{-1}\)) is \(1.4\times10^{-3}\) g per 100 mL. The solubility product constant of \(BaCO_3\) is \(x\times10^{-9}\,mol^2L^{-2}\). The value of \(x\) (nearest integer) is:

Buffer contains $[X^-]:[HX]=1:10$, and $K_b = 10^{-10}$. Find pH.}

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

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.

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.

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

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

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.

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

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

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

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 from following salts does not undergo hydrolysis ?

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

Calculate pOH of 0.001M HCl solution.

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.

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 ?

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?