Assertion : $H_{2} S$ is more acidic than $H_{2} O$ . Reason: $H - S$ bond is more polar than $H - O$ bond.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Both Assertion and Reason are incorrect

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Solution

The correct option is A Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
The S-H bond is weaker than the O-H bond, meaning that $H_{2} S$ more easily donates a proton and is, therefore, more acidic.
Water is amphoteric; it can act both as a proton donor (acid property) and as a proton acceptor (base property).
Because of this, oxygen holds onto the hydrogen better than sulfur. So $H_{2} S$ is a stronger acid because sulfur can't hang onto that hydrogen as well as oxygen can. Remember, to be a good acid, you need to be able to lose your hydrogen atoms.
Thus, option $A$ is correct.

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(1 + \frac{P b}{R T})

Reason: The compressibility factor for

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Assertion (A) p-nitrophenol is more acidic than phenol.
Reason (R) Nitro group helps in the stabilisation of the phenoxide ion by dispersal of negative charge due to resonance.
(a) Assertion and reason both are correct and reason is correct explanation of assertion.
(b) Assertion and reason both are wrong statements.
(c) Assertion is correct statement but reason is wrong statement.
(d) Assertion is wrong statement but reason is correct statement.
(e) Both assertion and reason are correct statements but reason is not correct explanation of assertion.

Q. Read the assertion and reason carefully to mark the correct option out of the options given below: