Solution

The value of K_c for the reaction
2NO(g)⟶ N₂(g) + O₂ (g) is 1.8 × 10_-2.
Calculate the value of C_K for the reaction
¹/₂N₂(g) + ¹/₂O₂(g) ⟶ NO(g)

Solution

A litre of solution is saturated with AgCl. To this solution if 1.0 × 10^-4 mole of solid NaCl is added, what will be the[Ag⁺], assuming no volume change?

More
Less
Equal
Zero

Solution

The dissociation of a weak electrolyte (AgCl) is suppressed on adding the strong electrolyte having a common ion (Cl^-), hence concentration of Ag⁺ ion will be less.

Solution

100 ml solution of an acid of pH= 1, is mixed with 100 ml solution of the same acid of pH = 2. The hydrogen ion concentration of the mixture will be:

5.5 × 10^–2
10^–2
10^–3
10^–4

Solution

Solubility product of BaCl₂ is 4 × 10^-9 moles/litre. Its solubility would be :

1× 10^-27
1 × 10^-3
1 × 10^-7
1 × 10^-2

Solution

The solubility of AgCl in 0.2 M NaCl solution is : (K_sp of AgCl = 1.20 ×10^–10)

6.0 × 10^–10 M
0.2 M
1.2 × 10^–10 M
0.2 × 10^–10 M

Solution

A buffer solution is prepared by mixing 10 ml of 1.0 M CH₃COOH and 20 ml of 0.5 M CH₃COONa and then diluted to 100 ml with distilled water. If pK_a of CH₃COOH is 4.76,what is the pH of the buffer solution ?

5.8
4.34
5.21
4.76

Solution

If sand S are respectively solubility and solubility product of a sparingly soluble binary electrolyte then :

s = S
s = S²
s = S^1/2
s = ¹/₂S

Solution

Which one has maximum solubility in liquid CCl₄?

NaCl
Cl₂
I₂
Br₂

Solution

(i)NaCl is ionic compound and therefore it is least soluble in liquid CCl₄.
(ii)Covalent compounds are soluble in liquid CCl₄. Solubility of covalent compounds \(\propto \frac{1}{Molecularmass}\)

∴ Cl₂ has highest solubility in liquid CCl₄

Which of the following solution can not act as a buffer?

NaH₂PO₄ + H₃PO₄
CH₃COOH + CH₃COONa
HCl + NH₄Cl
H₃PO₄ + NaH₂PO₄

Solution

HCl + NH₄Cl. HCl is strong acid hence not used in buffer.

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