8
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 :
9
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.
10
Conjugate base for Bronsted acids H2O and HF are :
11
pH of a saturated solution of Ca(OH)2 is 9. The solubility product (Ksp) of Ca(OH)2 is :
12
Which will make basic buffer?
13
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)
14
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. 75 mL $${M \over {5}}$$ HCl + 25 mL $${M \over {5}}$$ NaOH
D. 100 mL $${M \over {10}}$$ HCl + 100 mL $${M \over {10}}$$ NaOH
pH of which one of them will be equal to 1?
15
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
16
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
17
The solubility of AgCl(s) with solubility product 1.6 $$ \times $$ 10$$-$$10 in 0.1 M NaCl solution would be
18
Which of the following fluro-compounds is most likely to behave as a Lewis base ?
19
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?
20
Which one of the following pairs of solution is not an acidic buffer ?
21
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
22
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 AgNO3 solution is added to the solution containing equal moles of NaCl, NaBr, Nal and Na2CrO4?
AIPMT 2015 Cancelled Paper
23
Which of the following salts will give highest pH in water?
24
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
25
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 ?
26
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)
27
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
28
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
29
Which of these is least likely to act as a lewis base ?
30
Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value ?
31
Buffer solutions have constant acidity and alkalinity because
32
pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product (Ksp) of Ba(OH)2 is
33
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 the Cl$$-$$ concentration is 0.10 M. What will the concentrations of Ag+ and Pb2+ be at equilibrium ?
(Ksp for AgCl = 1.8 $$ \times $$ 10$$-$$10, Ksp for PbCl2 = 1.7 $$ \times $$ 10$$-$$5)
34
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)
35
Which of the following is least likely to behave as Lewis base?
36
If pH of a saturated solution of Ba(OH)2 is 12, the value of its Ksp is
37
In a buffer solution containing equal concentration of B$$-$$ and HB, the Kb for B$$-$$ is 10$$-$$10. The pH of buffer solution is
38
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
39
The ionization constant of ammonium hydroxide is 1.77 $$ \times $$ 10$$-$$5 at 298 K. Hydrolysis constant of ammonium chloride is
40
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?
41
Which of the following molecules acts as a Lewis acid?
42
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?
43
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
44
Calculate the pOH of a solution at 25oC that contains 1 $$ \times $$ 10$$-$$10 M of hydronium ions, i.e. H3O+.
45
Which of the following pairs constitutes a buffer?
46
The hydrogen ion concentration of a 10$$-$$8 M, HCl aqueous solution at 298 K (Kw = 10$$-$$14) is
47
At 25oC, the dissociation constant of a base, BOH, is 1.0 $$ \times $$ 10$$-$$12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be
48
H2S gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because
49
The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base (In$$-$$) forms of the indicator by the expression
50
The solubility product of a sparingly soluble salt AX2 is 3.2 $$ \times $$ 10$$-$$11. Its solubility (in moles/L) is
51
The solubility product of AgI at 25oC is 1.0 $$ \times $$ 10$$-$$16 mol2 L$$-$$2. The solubility of AgI in 10$$-$$4 N solution of KI at 25oC is approximately (in mol L$$-$$1
53
Solubility of MX2 type electrolytes is 0.5 $$ \times $$ 10$$-$$4 mole/lit., then find out Ksp of electrolytes.
54
Solution of 0.1 N NH4OH and 0.1 N NH4Cl has pH 9.25. Then find out pKb of NH4OH
55
Ionisation constant of CH3COOH is 1.7 $$ \times $$ 10$$-$$5 and concentration of H+ ions is 3.4 $$ \times $$ 10$$-$$4. Then find out initial concentration of CH3COOH molecules.
56
In HS$$-$$, I$$-$$, R $$-$$ NH2, NH3 order of proton accepting tendency will be
57
Solubility of M2S salt is 3.5 $$ \times $$ 10$$-$$6 then find out solubility product.
58
Correct relation between dissociation constants of a dibasic acid is
59
Which statement is wrong about pH and H+?
60
Conjugate acid of NH2$$-$$ is