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)

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

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 these is not likely to act as Lewis base?

(a)

BF₃

(b)

PF₃

(c)

CO

(d)

F^–

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

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

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

H₂PO₄^- the conjugate base of _______.

(a)

PO₄³⁻

(b)

P₂O₅

(c)

H₃PO₄

(d)

HPO₄^2-

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)

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

Which of the following is not a Lewis acid?

(a)

SiCl₄

(b)

AICl₃

(c)

SO₃

(d)

CO

Pick the strongest conjugate base among the following

(a)

Cl^-

(b)

\({ NO }_{ 2 }^{ - }\)

(c)

\({ SO }_{ 4 }^{ 2- }\)

(d)

CH₃COO^-

Pick the odd one out

(a)

Cl^-

(b)

CaO

(c)

SO₂

(d)

CH^-₃

The conjugate base of NH^-₂ is _______.

(a)

NH^-

(b)

NH₃

(c)

NH⁺₃

(d)

NH^2-

The relationship between degree of dissociation of a weak acid and its dissociation constant in a very dilute solution is _______.

(a)

K_a = α²C

(b)

K_a = \(\frac{α^2C}{(1+α)}\)

(c)

K_a = \(\frac{α^2}{(1+α)C}\)

(d)

K_a = \(\frac{α}{C(1+α)}\)

An example of basic buffer is _______.

(a)

NH₄OH and NH₄CI

(b)

NH₄OH and NaOH

(c)

NaOH and NH₄Cl

(d)

NaOH and KOH

Buffer index is _______.

(a)

\(\beta =\frac { dB }{ p{ K }_{ a } } \)

(b)

\(\beta =\frac { dB }{ d(pH) } \)

(c)

\(\beta =\frac { dB }{ pH } \)

(d)

\(\beta =\frac { dB }{ pOH } \)

The condition for a compound to be precipitated is _______.

(a)

Ionic product = solubility product

(b)

Ionic product < solubility product

(c)

Ionic product > solubility product

(d)

Ionic product ≤ solubility product

Degree if dissociation is nearly equal to for _______.

(a)

Strong acids and strong bases

(b)

Strong acids and weak bases

(c)

Weak acids and strong bases

(d)

Weak acids and weak bases

NH₄OH is a weak base because _______.

(a)

it has low vapour pressure

(b)

it is only partially ionised

(c)

it is completely ionised

(d)

it has low densit

When 10^-6 mole of a monobasic strong acid is dissolved in one litre of solvent, the pH of the solution is _______.

(a)

6

(b)

7

(c)

less than 6

(d)

more than 7