Ionic Equilibrium

The pH of rain water, is approximately :

In an acid-base titration, 0.1 M HCl solution
was added to the NaOH solution of unknown
strength. Which of the following correctly
shows the change of pH of the titraction
mixture in this experiment?

If solublity product of Zr3(PO4)4 is denoted by Ksp and its molar solubility is denoted by S, then
which of the following relation between S and Ksp is correct ?

If Ksp of Ag2CO3 is 8 \(\times\) 10–12, the molar solubility of Ag2CO3 in 0.1 M AgNO3 is -

What is the molar solubility of Al(OH)3 in 0.2 M NaOH solution ? Given that, solubility product of Al(OH)3 = 2.4 × 10–24
:

The molar solubility of Cd(OH)2 is 1.84 × 10–5
M in water. The expected solubility of Cd(OH)2 in a buffer
solution of pH = 12 is :

The decreasing order of electrical conductivity of the following aqueous solutions is :
0.1 M Formic acid (A),
0.1 M Acetic acid (B),
0.1 M Benzoic acid (C)

A mixture of 100 m mol of Ca(OH)2 and 2 g of sodium sulphate was dissolved in water and the volume was made up to 100 mL. The mass of calcium sulphate formed and the concentration of OH– in resulting solution, respectively, are : (Molar mas...

Consider the following statements
(a) The pH of a mixture containing 400 mL of 0.1 M H2SO4 and 400 mL of 0.1 M NaOH will be approximately 1.3
(b) Ionic product of water is temperature dependent.
(c) A monobasic acid with Ka = 10–5
has pH =...

The pH of a 0.02 M NH4Cl solution will be :
[given Kb (NH4OH) = 10–5
and log 2 = 0.301]

Which of the following is a Lewis acid?

The minimum volume of water required to dissolve 0.1 g lead (II) chloride to get a saturated solution (Ksp of PbCl2 = 3.2 \(\times\) 10-8 atomic mass of Pb = 207 u ) is :

Following four solutions are prepared by mixing different volumes of NaOH and HCl of different concentrations, pH of which one of them will be equal to 1 ?

Which of the following are Lewis acids?

Which of the following salts is the most basic in aqueous solution?

An aqueous solution contains 0.10 M H2S and 0.20 M HCl. If the equilibrium constants for the formation of HS– from H2S is 1.0 \(\times\) 10–7 and that of S2- from HS– ions is 1.2 \(\times\) 10–13 then the concentration of S2- ions in aqueou...

An alkali is titrated against an acid with methyl orange as indicator, which of the following is a correct combination?

An aqueous solution contains an unknown concentration of Ba2+. When 50 mL of a 1 M solution of Na2SO4 is added, BaSO4 just begins to precipitate. The final volume is 500 mL. The solubility product of BaSO4 is 1 \(\times\) 10–10. What is the...

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

Additin of sodium hydroxide solution to a weak acid (HA)results in a buffer of pH 6. If ionition constant of HA is 10\(-\)5, the ratio of salt to acid concentration in the buffer solution will be :

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

How many litres of water must be added to 1 litre of an aqueous solution of HCl with a pH of 1 to create an
aqueous solution with pH of 2?

The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, Ka of this acid is :

At 25°C, the solubility product of Mg(OH)2 is 1.0 \(\times\) 10–11. At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001 M Mg2+ ions?

Solubility product of silver bromide is 5.0 \(\times\) 10–13. The quantity of potassium bromide (molar mass taken as 120g of mol–1) to be added to 1 litre of 0.05 M solution of silver nitrate to start the
precipitation of AgBr is :

Three reactions involving \(H_2PO_4^−\) are given below :
(i) H3PO4 + H2O \(\to\) H3O+ + \(H_2PO_4^−\)
(ii) \(H_2PO_4^−\) + H2O \(\to\) \(HPO_4^{2−}\) + H3O+
(iii) \(H_2PO_4^−\) + OH- \(\to\)H3PO4 + O2-
In which of the above does $$H_2PO_4^...

Solid Ba(NO3)2 is gradually dissolved in a 1.0 \(\times\) 10-4 M Na2CO3 solution. At what concentration of Ba2+ will a precipitate begin to form ?
(Ksp for BaCO3 = 5.1 \(\times\) 10−9 )

The pKa of a weak acid, HA, is 4.80. The pKb of a weak base, BOH, is 4.78. The pH of an aqueous
solution of the corresponding salt, BA, will be

Four species are listed below
i. \(HCO_3^−\)
ii. \(H_3O^+\)
iii. \(HSO_4^−\)
iv. \(HSO_3F\)
Which one of the following is the correct sequence of their acid strength?

The pKa of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of
the acid is ionized is :

The first and second dissociation constants of an acid H2A are 1.0 \(\times\) 10−5
and 5.0 \(\times\) 10−10 respectively. The overall dissociation constant of the acid will be :

In a sautrated solution of the sparingly soluble strong electrolyte AgIO3 (Molecular mass = 283) the
equilibrium which sets in is
AgIO3(s) \(\leftrightharpoons\) Ag+(aq) + \(IO_3^-\)
If the solubility product constant Ksp of AgIO3 at a giv...

What is the conjugate base of OH-?

The solubility product of a salt having general formula MX2, in water is: 4 \(\times\) 10-12 . The
concentration of M2+ ions in the aqueous solution of the salt is :

Hydrogen ion concentration in mol / L in a solution of pH = 5.4 will be :

The molar solubility (in ol L-1) of a sparingly soluble salt MX4 is "s". The corresponding solubility product is Ksp. 's' is given in term of Ksp by the relation :

The conjugate base of H2PO4- is :

The solubility in water of a sparingly soluble salt AB2 is 1.0 \(\times\) 10-5 mol L-1. Its solubility product number will be :

Which one of the following statements is not true?

When rain is accompanied by a thunderstorm, the collected rain water will have a pH value :

1 M NaCL and 1 M HCL are present in an aqueous solution. The solution is

Let the solubility of an aqueous solution of Mg(OH)2 be x then its Ksp is :

Species acting as both Bronsted acid and base is :