Concentration of the Ag⁺ ions in a saturated solution of Ag₂C₂O₄ is 2.24 ×10^-4mol L^-1 solubility product of Ag₂C₂O₄ is_______.

(a)

2.42 × 10^-8mol³L^-3

(b)

2.66 × 10^-12mol³L^-3

(c)

4.5 × 10^-11mol³L^-3

(d)

5.619 × 10^-12mol³L^-3

Following solutions were prepared by mixing different volumes of NAOH of HCL different concentrations
1) 60 mL\(\frac{M}{10}\)HCl + 40mL\(\frac{M}{10}\)NaOH
2) 55 mL\(\frac{M}{10}\)HCl + 45mL\(\frac{M}{10}\)NaOH
3) 75 mL\(\frac{M}{5}\)HCl + 25mL\(\frac{M}{5}\)NaOH
4) 100 mL\(\frac{M}{10}\)HCl + 100mL\(\frac{M}{10}\)NaOH
pH of which one of them will be equal to 1?

(a)

(iv)

(b)

(i)

(c)

(ii)

(d)

(iii)

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

(a)

1.08 × 10^-14mol²L^-2

(b)

1.08 × 10^-12mol²L^-2

(c)

1.08 × 10^-10mol²L^-2

(d)

1.08 × 10^-8mol²L^-2

pH of a saturated solution of Ca(OH)₂ is 9. The Solubility product (K_sp) of Ca(OH)₂ _______.

(a)

0.5 × 10^-15

(b)

0.25 × 10^-10

(c)

0.125 × 10^-15

(d)

0.5 × 10^-10

Conjugate base for Bronsted acids H₂O and HF are _______.

(a)

OH^- and H₂FH⁺, respectively

(b)

H₃O⁺ and F^-, respectively

(c)

OH^- and F^-, respectively

(d)

H₃O⁺ and H₂F⁺, respectively

Which will make basic buffer?

(a)

50 mL of 0.1M NaOH+25mL of 0.1M CH₃COOH

(b)

100 mL of 0.1M CH₃COOH+100 mL of 0.1M NH₄OH

(c)

100 mL of 0.1M HCl+200 mL of 0.1M NH₄OH

(d)

100 mL of 0.1M HCl+100 mL of 0.1M NaOH

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

(a)

BF₃

(b)

PF₃

(c)

CF₄

(d)

SiF₄

Which of these is not likely to act as Lewis base?

(a)

BF₃

(b)

PF₃

(c)

CO

(d)

F^–

What is the decreasing order of strength of bases
OH, NH₂^- H - C ≡ C and CH₃ - CH₂^-

(a)

OH^->NH₂^- >H-C≡C >CH₃^-CH₂^-

(b)

NH₂^->OH^->CH₃^-CH₂^- >H-C≡C

(c)

CH₃^-CH₂^->NH₂^->H-C≡C^->OH^-

(d)

OH^->H-C ≡ C^->CH₃^-CH₂^- >NH₂^-

The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively _______.

(a)

acidic, acidic, basic

(b)

basic, acidic, basic

(c)

basic, neutral, basic

(d)

none of these

The percentage of pyridine (C₅H₅N) that forms pyridinium ion (C₅H₅NH) in a 0.10M aqueous pyridine solution _______.(K_b for C₅H₅N = 1.7×10^-9) is 

(a)

0.006%

(b)

0.013%

(c)

0.77%

(d)

1.6%

Equal volumes of three acid solutions of pH 1,2 and 3 are mixed in a vessel. What will be the H⁺ ion concentration in the mixture?

(a)

3.7 × 10^-2

(b)

10^-6

(c)

0.111

(d)

none of these

The solubility of AgCl (s) with solubility product 1.6 × 10^-10 in 0.1M NaCl solution would be _______.

(a)

1.26 × 10^-5M

(b)

1.6 × 10^-9M

(c)

1.6 × 10^-11M

(d)

Zero

If the solubility product of lead iodide is 3.2 × 10^-8, its solubility will be _______.

(a)

2 × 10^-3M

(b)

4 × 10^-4M

(c)

1.6 × 10^-5M

(d)

1.8 × 10^-5M

Using Gibb’s free energy change, ∆G^o=57.34 kJ mol^-1, for the reaction, X₂Y_(s)⇌2X⁺+Y^2- (aq), calculate the solubility product of X₂Y in water at 300 K_______. (R = 8.3 J K^-1Mol^-1)

(a)

10^-10

(b)

10^-12

(c)

10^-14

(d)

can not be calculated from the given dat

MY and NY₃, are insoluble salts and have the same K_sp values of 6.2 × 10^-13 at room temperature. Which statement would be true with regard to MY and NY₃?

(a)

The salts MY and NY₃ are more soluble in 0.5M KY than in pure water

(b)

The addition of the salt of KY to the suspension of MY and NY₃ will have no effect on their solubility’s

(c)

The molar solubility of MY and NY₃ in water are identical

(d)

The molar solubility of MY in water is less than that of NY₃

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

(a)

2.0

(b)

3

(c)

7.0

(d)

12.65

The dissociation constant of a weak acid is 1 × 10^-3. In order to prepare a buffer solution with a pH = 4, the [Acid]/[Salt] ratio should be _______.

(a)

4:3

(b)

3:4

(c)

10:1

(d)

1:10

The pH of 10^-5M KOH solution will be _______.

(a)

9

(b)

5

(c)

19

(d)

none of these

H₂PO₄^- the conjugate base of _______.

(a)

PO₄³⁻

(b)

P₂O₅

(c)

H₃PO₄

(d)

HPO₄^2-

Which of the following can act as Lowery – Bronsted acid well as base?

(a)

HCl

(b)

SO₄²⁻

(c)

HPO₄²⁻

(d)

Br^-

The pH of an aqueous solution is Zero. The solution is _______.

(a)

slightly acidic

(b)

strongly acidic

(c)

neutral

(d)

basic

The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salts is given by _______.

(a)

\([{ H }^{ + }]=\frac { { K }_{ a }[acid] }{ [salt] } \)

(b)

\([{ H }^{ + }]={ K }_{ a }[salt]\)

(c)

\([{ H }^{ + }]={ K }_{ a }[acid]\)

(d)

\([{ H }^{ + }]=\frac { { K }_{ a }[salt] }{ [acid] } \)

Which of the following relation is correct for degree of hydrolysis of ammonium acetate?

(a)

\(h=\sqrt { \frac { { K }_{ h } }{ C } } \)

(b)

\(h=\sqrt { \frac { { K }_{ a } }{ K_b } } \)

(c)

\(h=\sqrt { \frac { { K }_{ w } }{ { K }_{ a }.{ K }_{ b } } } \)

(d)

\(h=\sqrt { \frac { { { K }_{ a }.{ K }_{ b } } }{ { K }_{ w } } } \)

Dissociation constant of NH₄OH is 1.8 x 10^-5  the hydrolysis constant of NH₄Cl would be _______.

(a)

1.8 × 10^-19

(b)

5.55 × 10^-10

(c)

5.55 × 10^-5

(d)

1.80 × 10^-5