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Solution

Solution

Reaction (c) can be obtained by adding reactions (a)and (b) therefore K₃= K₁. K₂
Hence (c) is the correct answer.

A weak acid, HA, has a K_a of 1.0 × 10^–5. If 0.1 mole of this acid dissolved in one litre of water, the percentage of acid dissociated at equilbrium is closest to

1.0%
99.9%
0.1%
99.0%

Solution

Which of the following is conjugate base of [C₂H₅NH₃]⁺

C₂H₅NH₂
C₂N⁺H₄(OH)^-
[C₂H₂NH]^-
None of these

Solution

A buffer solution is prepared by mixing 0.1 M ammonia and 1.0 M ammonium chloride. At 298 K, the pK_b of NH₄OH is 5.0. The pH of the buffer is

10.0
9.0
6.0
8.0

Solution

Solubility of BaF₂ in a solution of Ba(NO₃)₂ will be represented by

[Ba²⁺]
[NO₃]^-
\(\frac{1}{2}\)[F^-]
[Ba]²

Solution

Ba⁺⁺ is common ion in the both solution. The solubility will depend on more reactive element.Option (c) is correct

When equal volumes of the following solutions are mixed,precipitation of AgCl (K_sp= 3 × 10^-10) will occur with –

10^-4 M AgNO₃ and 10^-5 M KCl
10^-5 M AgNO₃ and 10^-5 M KCl
10^-4 M AgNO₃ and 10^-4 M KCl
Both (a)and (c)

Solution

If the equilibrium constant of the reaction of weak acid HA with strong base is 10⁷, then pOH of the aqueous solution of 0.1M NaA is –

Solution

The buffering action of an acidic buffer is maximum when its pH is equal

5
7
1
pK_a

Solution

Buffering action is maximum when[Salt] = [Acid]i.e., pH = pK_a

In qualitative analysis, in III group NH₄Cl is added before NH₄OH because

to increase the concentration of NH₄⁺ ions
to increase concentration of Cl^- ions
to reduce the concentration of OH^- ions
to increase concentration of OH^- ions

Solution

Due to common ion effect addition of NH₄Cl in group(III) suppresses the ionisation of NH₄OH with the result concentration of OH^- decreases.

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