Ionic Equilibrium

\(\text { The correct order of solubility of the given salts in water at } 298 \mathrm{~K} \text { is }\)
$$ \begin{array}{|l|l|} \hline \text { Salt } & \mathbf{K}_{\text {sp }} \text { at } \mathbf{2 9 8} \text { K } \\ \hline \mathrm{A...

Phenolphthalein is used as an indicator for the titration of sodium hydroxide solution against a standard solution of oxalic acid. The colour change that is observed at an alkaline pH close to the equivalence point during this titration is:...

At 298 K , a certain buffer solution contains equal concentrations of $\mathrm{X}^{-}$and $\mathrm{HX}, \mathrm{K}_{\mathrm{b}}$ for $\mathrm{X}^{-}$is $10^{-10}$. What is the pH of this buffer solution?

In a qualitative analysis, $\mathrm{Bi}^{3+}$ is detected by appearance of precipitate of $\mathrm{BiO}(\mathrm{OH})(\mathrm{s})$. Calculate pH when the following equilibrium exists at 298 K .
$$ \mathrm{BiO}(\mathrm{OH})(\mathrm{s}) \right...

Phosphoric acid ionizes in three steps with their ionization constant values $K_{a_1}, K_{a_2}$ and $K_{a_3}$, respectively, while $K$ is the overall ionization constant. Which of the following statements are true?
A. $\quad \log \mathrm{K}...

If the molar conductivity $\left(\Lambda_{\mathrm{m}}\right)$ of a $0.050 \mathrm{~mol} \mathrm{~L}^{-1}$ solution of a monobasic weak acid is $90 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$, its extent (degree) of dissociation will be
[...

The ratio of solubility of AgCl in 0.1 M KCl solution to the solubility of AgCl in water is:
(Given : Solubility product of AgCl = 10\(^{–10}\))

Which indicator is used in the titration of sodium hydroxide against oxalic acid and what is the colour change at the end point?

An acidic buffer is prepared by mixing :

0.01 M acetic acid solution is 1% ionised, then pH of this acetic acid solution is :

The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is [Given pKa of CH3COOH = 4.57]

The pKb of dimethyl amine and pKa of acetic acid are 3.27 and 4.77 respectively at T (K). The correct option for the pH of dimethyl ammonium acetate solution is :

Find out the solubility of Ni(OH)2 in 0.1M NaOH. Given that the ionic product of Ni(OH)2 is 2 \(\times\) 10-15.

pH of a saturated solution of Ca(OH)2 is 9. The solubility product (Ksp) of Ca(OH)2 is :

Which will make basic buffer?

Conjugate base for Bronsted acids H2O and HF are :

Following solutions were prepared by mixing
different volumes of NaOH and HCl of different
concentrations :
A. 60 mL \({M \over {10}}\) HCl + 40 mL \({M \over {10}}\) NaOH
B. 55 mL \({M \over {10}}\) HCl + 45 mL \({M \over {10}}\) NaOH
C. 7...

The solubility of BaSO4
in water is
2.42 × 10–3 g L–1 at 298 K. The value of its
solubility product (Ksp) will be (Given molar
mass of BaSO4
= 233 g mol–1)

Concentration of the Ag+ ions in a saturated solution of Ag2C2O4 is 2.2 \(\times\) 10\(-\)4 mol L\(-\)1. Solubility product of Ag2C2O4 is

The solubility of AgCl(s) with solubility product 1.6 \(\times\) 10\(-\)10 in 0.1 M NaCl solution would be

Which of the following fluro-compounds is most likely to behave as a Lewis base ?

The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5N+H) ina 0.10 M aqueous pyridine solution (Kb for C5H5N = 1.7 \(\times\) 10\(-\)9) is

MY and NY3, two nearly insoluble salts, have the same Ksp values of 6.2 \(\times\) 10\(-\)13 at room temperature. Which statement would be true in regard to MY and NY3?

The Ksp of Ag2CrO4,  AgCl,  AgBr  and Agl  are respectively, 1.1 \(\times\) 10\(-\)12, 1.8 \(\times\) 10\(-\)10, 5.0 \(\times\) 10\(-\)13, 8.3 \(\times\) 10\(-\)17. Which one of the following salts will precipitate last if AgN...

What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?

Which one of the following pairs of solution is not an acidic buffer ?

Which of the following salts will give highest pH in water?

The values of Ksp of CaCO3 and CaC2O4 are 4.7 \(\times\) 10\(-\)9 and 1.3 \(\times\) \(-\)9 respectively at 25oC. If the mixture of these two is washed with water, what is the concentration of Ca2+ ions in water ?

The dissociation constant of weak acid is 1 \(\times\) 10\(-\)4. In order to prepare a buffer solution with a pH = 5, the [Salt]/[Acid] ratio should be

At 100oC the Kw of water is 55 times its value at 25oC. What will be the pH of neutral solution? (log 55 = 1.74)

Accumulation of lactic acid (HC3H5O3), a monobasic acid in tissues leads to pain and a feeling of fatigue. In a 0.10 M aqueous solution, lactic acid is 3.7% dissociates. The value of dissociation constant, Ka, for this acid will be

KMnO4 can be prepared from K2MnO4 as per the reaction,
3MnO42\(-\) + 2H2O \(\rightleftharpoons\) 2MnO4\(-\) + MnO2 + 4OH\(-\)
The reaction can go to completion by removing OH\(-\) ions by adding

Which of these is least likely to act as a lewis base ?

Buffer solutions have constant acidity and alkalinity because

Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value ?

pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product (Ksp) of Ba(OH)2 is

A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of NH+4 is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 \(\times\) 10\(-\)5, what is the pH of this solution? (log 2.7 = 0.43)

Which of the following is least likely to behave as Lewis base?

In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+ and pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until t...

What is [H+] in mol/L of a solution that is 0.20 M in CH3COONa and 0.10 M in CH3COOH? Ka for CH3COOH = 1.8 \(\times\) 10\(-\)5

In a buffer solution containing equal concentration of B\(-\) and HB, the Kb for B\(-\) is 10\(-\)10. The pH of buffer solution is

If pH of a saturated solution of Ba(OH)2 is 12, the value of its Ksp is

The ionization constant of ammonium hydroxide is 1.77 \(\times\) 10\(-\)5 at 298 K. Hydrolysis constant of ammonium chloride is

What is the [OH\(-\)] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba(OH)2?

Which of the following molecules acts as a Lewis acid?

Equal volumes of three acid solutions of pH 3, 4 and 5 are mixed in a vessel. What will be the H+ ion concentration in the mixture?

Calculate the pOH of a solution at 25oC that contains 1 \(\times\) 10\(-\)10 M of hydronium ions, i.e. H3O+.

A weak acid, HA, has a Ka of 1.00 \(\times\) 10\(-\)5. If 0.100 mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closest to

Which of the following pairs constitutes a buffer?

The hydrogen ion concentration of a 10\(-\)8 M, HCl aqueous solution at 298 K (Kw = 10\(-\)14) is