Which of the following gives a buffer solution when equal volumes...

Question

Which of the following gives a buffer solution when equal volumes of the two solutions are mixed?(a) 0.10 M NH3 and 0.10 M HCl(b) 0.20 M NH3 and 0.10 M HCl(c) 0.10 M NH4Cl and 0.10 M NH3 (d) 0.20 M NH4Cl and 0.10 M NaOH

Accepted Answer

Step 1: Understand what a buffer solution is. A buffer solution is a solution that can resist changes in pH when small amounts of an acid or a base are added. It is usually made up of a weak acid and its conjugate base, or a weak base and its conjugate acid.. Step 2: Identify the weak base and its conjugate acid in the given options. In this case, NH3 is a weak base and its conjugate acid is NH4+ (which is present in NH4Cl).. Step 3: Look for the option where both the weak base (NH3) and its conjugate acid (NH4+) are present. This is because a buffer solution is formed when a weak base and its conjugate acid (or a weak acid and its conjugate base) are mixed together.. Step 4: From the given options, (c) 0.10 M NH4Cl and 0.10 M NH3 is the pair that forms a buffer solution. This is because NH4Cl is a source of NH4+ (the conjugate acid of NH3) and NH3 is the weak base.. Step 5: Note that the other options do not form a buffer solution because they do not contain both a weak base and its conjugate acid. For example, in option (a), HCl is a strong acid, not a weak one, so it does not form a buffer with NH3. Similarly, in option (d), NaOH is a strong base, not a weak one, so it does not form a buffer with NH4Cl.

Which of the following gives a buffer solution when equal volumes of the two solutions are mixed?(a) 0.10 M NH3 and 0.10 M HCl(b) 0.20 M NH3 and 0.10 M HCl(c) 0.10 M NH4Cl and 0.10 M NH3 (d) 0.20 M NH4Cl and 0.10 M NaOH

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Key Concepts

Buffer Solutions

Weak Acids and Bases

Conjugate Acid-Base Pairs