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Assertion. The pH at the end point of an...

Assertion. The pH at the end point of any acid-base titration is always 7.
Reason. The aqueous solution of a salt is always neutral.

A

If both assertion and reason are true, and reason is the true explanation of the assertion.

B

If both assertion and reason are true, but reason is not the true explanation of the assertion.

C

If aasertion is true, but reason is false.

D

If both assertion and reason are false.

Text Solution

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The correct Answer is:
To solve the question, we need to analyze both the assertion and the reason provided: **Assertion:** The pH at the end point of any acid-base titration is always 7. **Reason:** The aqueous solution of a salt is always neutral. ### Step-by-Step Solution: 1. **Understanding the Assertion:** - The assertion states that the pH at the end point of any acid-base titration is always 7. - This is only true for the titration of a strong acid with a strong base. For example, titrating hydrochloric acid (HCl) with sodium hydroxide (NaOH) will yield a neutral solution at the equivalence point, resulting in a pH of 7. - However, if a weak acid (like acetic acid) is titrated with a strong base (like NaOH), the pH at the end point will be greater than 7. Conversely, if a strong acid is titrated with a weak base, the pH at the end point will be less than 7. - Therefore, the assertion is **false** as it does not hold true for all acid-base titrations. 2. **Understanding the Reason:** - The reason states that the aqueous solution of a salt is always neutral. - This statement is incorrect. The pH of a salt solution depends on the nature of the acid and base from which it is derived. - For example, a salt formed from a strong acid and a weak base (like ammonium chloride from hydrochloric acid and ammonia) will result in an acidic solution (pH < 7). Conversely, a salt from a weak acid and a strong base (like sodium acetate from acetic acid and sodium hydroxide) will yield a basic solution (pH > 7). - Therefore, the reason is also **false**. 3. **Conclusion:** - Since both the assertion and the reason are false, the correct answer is that both statements are incorrect. ### Final Answer: Both the assertion and the reason are false. ---
To solve the question, we need to analyze both the assertion and the reason provided: **Assertion:** The pH at the end point of any acid-base titration is always 7. **Reason:** The aqueous solution of a salt is always neutral. ### Step-by-Step Solution: 1. **Understanding the Assertion:** ...
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Knowledge Check

  • Assertion. An aqueous solution of ammonium acetate can act as buffer. Reason. An aqueous solution of any pure salt acts as a buffer.

    A
    If both assertion and reason are true, and reason is the true explanation of the assertion.
    B
    If both assertion and reason are true, but reason is not the true explanation of the assertion.
    C
    If aasertion is true, but reason is false.
    D
    If both assertion and reason are false.

  • Aqueous solution of salt of strong base and weak acid

    A
    Undergoes anionic hydrolysis
    B
    Is basic in nature
    C
    Has `P^(H)` greater than `7`
    D
    All the above

  • The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. The pH of the solution is related to ratio of the concentration of the conjugate acid (Hin) and base (In^(-)) forms of the indicator by the expression

    A
    `"log"([In^(-)])/([HIn])=pK_(In)-pH`
    B
    `"log"([HIn])/([In])=pK_(In)-pH`
    C
    `"log"([HIn])/([In^(-)])=pH-pK_(In)`
    D
    `"log"([In^(-)])/([HIn])=pH-pK_(In)`

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