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Assertion : Buffer solutions are those w...

Assertion : Buffer solutions are those which resist change in pH value on the addition of a small amount of acid or a base to it.
Reason: Mixture of `NH_4OH` and `NH_4 Cl` acts as basic buffer.

A

Assertion and reason both are correct statements and Reason is correct explanation for assertion.

B

Assertion and reason both are correct statement but reason is not correct explanation for assertion

C

Assertion is correct statement but reason is wrong statement.

D

Assertion is wrong statement but reason is correct statement

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding the assertion and reason provided, we will analyze both statements step by step. ### Step-by-Step Solution: 1. **Understanding the Assertion**: - The assertion states that buffer solutions resist changes in pH when small amounts of acid or base are added. - A buffer solution is typically composed of a weak acid and its conjugate base or a weak base and its conjugate acid. This combination allows the solution to neutralize added acids or bases, thus maintaining a relatively stable pH. 2. **Understanding the Reason**: - The reason given is that a mixture of ammonium hydroxide (NH₄OH) and ammonium chloride (NH₄Cl) acts as a basic buffer. - Ammonium hydroxide is a weak base, and ammonium chloride is the salt of its conjugate acid (NH₄⁺). This combination indeed forms a basic buffer solution. 3. **Conclusion**: - Since both the assertion and the reason are true, and the reason correctly explains the assertion, we can conclude that the assertion is correct, and the reason is also correct and provides a valid explanation for the assertion. ### Final Answer: - Both the assertion and reason are true, and the reason explains the assertion.
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Assertion (A ) : A buffer solution has a capacity to resist the change in pH value on addition is small amount of acid or base to it. Reason (R ) : An aqueous solution of ammonium acetate can act as a buffer.

The dissociation of weak electrolyte (a weak base or weak acid) id expressed in terms of Ostwald dilution law. An acid is a substance which furnishes a proton or accepts an electron pair whereas a base is proton acceptor or electron pair donor. Storonger is the acid weaker is its conjugate base. The dissociation constants of an acid (K_(a)) and its conjugate base are related by (K_(w)=K_(a)xxK_(b) , where K_(w) is ionic prodcut of water equal to 10-14 at 25^(@) C. The numerical value of K_(w) however increases with temperature. In a solution of an acid or base [H^(+)][OH^(-)]=10^(14) .Thus, the [H^(+)] in a solution is expressed as : [H^(+)]=10^(-pH) and pH+pOH=14 . Buffer solutions are the solutions which do not show appreciable change in the pH on addition of small amount of acid or base. The pK_(a) value of NH_(4)^(+) is 9. The pK_(b) value of NH_(4) OH would be :

The dissociation of weak electrolyte (a weak base or weak acid) is expressed in terms of Ostwald's dilution law. An acid is substance which furnishes a proton or accepts an electron pair, where a base is proton acceptor or electron pair donor. Stronger is acid, weaker is its conjugate base. The dissociation constants of an acid (K_(a)) and its conjugate base (K_(b)) are related by K_(w)=K_(a)xxK_(b) , where K_(w) is ionic product of water equal to 10^(-14) at 25^(@)C . The numerical value of K_(w) however increase with temperature. In a solution of an acid or base [H^(+)][OH^(-)]=10^(-14) . Thus the [H^(+)] in a solution is expressed as: [H^(+)]=10^(-pH) and pH+pOH=14 . Buffer solution are the solutions which do not show appreciable change in the pH on addition of small amount of acid or base. The pK_(a) value of NH_(4)^(+) is 9. The pK_(b) value of NH_(4)OH would be:

Asseration : A solution containing a mixture of acetic acid and sodium acetate maintains a constant value of ph on addition of small amounts of acid or alkali. Reason : A solution containing a mixture of acetic acid and sodium acetate acts as a buffer solution around ph 4.75.

Choose the correct set of True/Fasle for following statements: (i) Silver chloride is more soluble in very concentrated sodium chloride solution than in pure water. (ii) The pH of a buffer solution does not change on addition of small amount of an acid or a base. (iii) Addition of NH_(4)Cl does not affect the pH of a solution of NH_(4)OH (iv) Degree of hydrolysis of ammonium acetate does not depend upon the concentration of ammonium acetate solution. (v) A mixture of acetic acid and sodium acetate can act as buffer solution.

The pH of buffer of NH_4OH + NH_4Cl - type is given by -