Determine whether or not the mixing of each pair of solutions results in a buffer. a. 75.0 mL of 0.10 M HF; 55.0 mL of 0.15 M NaF b. 150.0 mL of 0.10 M HF; 135.0 mL of 0.175 M HCl d. 125.0 mL of 0.15 M CH₃NH₂; 120.0 mL of 0.25 M CH₃NH₃Cl

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Hello. Everyone in this video. We're trying to see if this combination right here is able to make a buffer. So let's take a look here. Let's recall that a buffer solution can be made of the following. So first combination it could be a weak base plus its conjugate acid. 2nd mixture. It can be a weak acid with its conjugate base. 3rd option is if we have a weak acid plus a strong base for this third combination because we have a strong base, we want to make sure that the concentration of our acid. So the weak acid here is actually going to be stronger than the concentration of our base. So the strong base. Alright, last option is going to be where we have a weak base plus a strong acid. Similar to the third option here. We want to make sure that we have a strong asset that the base or the concentration of our base is actually going to be greater than the concentration of the acid. All right. So recognizing the regions that we have, we have our C H C O H. And then we have our H. C. L. Well, the first one here that's going to be actually a weak acid. And if you didn't know our hcl was a known strong acid. So we have our weak acid and our strong acid. That's none of these combinations here. And therefore you can answer the question saying no that this combination is not a buffer solution. All right. And this is going to be my final answer. First question. Thank you all so much for watching.

Determine whether or not the mixing of each pair of solutions results in a buffer. a. 75.0 mL of 0.10 M HF; 55.0 mL of 0.15 M NaF b. 150.0 mL of 0.10 M HF; 135.0 mL of 0.175 M HCl d. 125.0 mL of 0.15 M CH₃NH₂; 120.0 mL of 0.25 M CH₃NH₃Cl

Verified Solution

Key Concepts

Buffer Solutions

Weak Acids and Strong Acids

pH and Acid-Base Reactions

Determine whether or not the mixing of each pair of solutions results in a buffer. a. 75.0 mL of 0.10 M HF; 55.0 mL of 0.15 M NaF b. 150.0 mL of 0.10 M HF; 135.0 mL of 0.175 M HCl d. 125.0 mL of 0.15 M CH3NH2; 120.0 mL of 0.25 M CH3NH3Cl

Verified Solution

Key Concepts

Buffer Solutions

Weak Acids and Strong Acids

pH and Acid-Base Reactions

Determine whether or not the mixing of each pair of solutions results in a buffer. a. 75.0 mL of 0.10 M HF; 55.0 mL of 0.15 M NaF b. 150.0 mL of 0.10 M HF; 135.0 mL of 0.175 M HCl d. 125.0 mL of 0.15 M CH₃NH₂; 120.0 mL of 0.25 M CH₃NH₃Cl