A buffer solution is comprised of 50.0 mL of a 0.100 M HC 2 H 3 O 2 and 60.0 mL of a 0.100 M NaC 2 H 3 O 2 . Which of the following actions would completely destroy the buffer?

So above our solutions comprised of 50 ml of 0.100 molar acetic acid and 60 ml of a 0.100 molar sodium acetate. Which of the following actions would completely destroy the buffer? Alright. The first thing we're gonna say is, in order to destroy a buffer you do that by adding either strong acid or strong base. If you add too much strong acid or too much strong base, it'll destroy the buffer. Here for a, a can't be an answer because in a, all we're doing is adding more weak acid. This will help to make the buffer more concentrated by increasing the weak acid component. This will only help the buffer. Same thing can be said for B. For B, CAC2H 3 022 is just a conjugate base of the weak acid. It's not the same conjugate base here but it's still a conjugate base of the weak acid. So it's gonna help to strengthen the buffer. So this is out. Now our answer has to be one of the last three choices because in those three choices we have a strong base and then we have strong acids. Remember, adding too much strong acid or too much strong base can destroy a buffer. To get the right answer here, we just have to remember, what are the conditions that help to make a buffer? Well, if we have a weak acid, the weak acid has to be in greater amount than the strong base. Remember, the weak species has to be higher than the strong species. Or the conjugate base, which is also a weak base, needs to be greater than the strong acid. Again, whatever is weak has to be higher than what is strong in order to make a buffer. So as long as these requirements are met, we'll have a buffer. If these requirements are broken, then we will not have a buffer because it's been destroyed. Remember the word of means multiply. If we divide the ml's by a 1,000, we'll get their liters. And if you multiply them by their molarities you'll have your moles. Okay so the amount of weak acid we have is 0.005 moles of my weak acid. And then we'll have 0.006 moles of my conjugate base. Remember, in order to have a buffer, the weak species need to be higher than the strong species. If we don't have them being higher, then the buffer has been destroyed. So if we look at our choices, remember our conjugate base here is 0.006 moles and this is 0.005 moles. Here if I add strong base, adding strong base will attack the weak acid. So my strong base is 0.005 moles. As we can see, the weak acid is 0.005 moles. The strong base is 0.005 moles. In this situation, the buffer has been destroyed because again the weak species needs to be higher than the strong species. It's not, so this has successfully destroyed our buffer. In the last two options we have 0.004 moles and 0.001 moles of strong acid. In both situations, the conjugate base, which is the weak base, is still greater than those amounts. So in both of these situations we'll still have a buffer. Only in situation C is the weak acid not greater than the strong base. So then therefore a buffer has been destroyed.

A buffer solution is comprised of 50.0 mL of a 0.100 M HC 2 H 3 O 2 and 60.0 mL of a 0.100 M NaC 2 H 3 O 2 . Which of the following actions would completely destroy the buffer?

Adding 0.007 mol Ca(C 2 H 3 O 2 ) 2

Table of contents

Skip topic navigation

1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

14. Acids and Bases

Buffers

Introduction to Chemistry

14. Acids and Bases

Buffers

Previous problemNext problem

Struggling with Introduction to Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

A buffer solution is comprised of 50.0 mL of a 0.100 M HC₂H₃O₂ and 60.0 mL of a 0.100 M NaC₂H₃O₂. Which of the following actions would completely destroy the buffer?

Adding 0.003 mol HC₂H₃O₂

Adding 0.007 mol Ca(C₂H₃O₂)₂

Adding 0.005 mol NaOH

Adding 0.004 mol HCl

Adding 0.001 mol HCl

Previous problemNext problem

Verified step by step guidance

Understand the concept of a buffer solution: A buffer solution resists changes in pH when small amounts of acid or base are added. It typically consists of a weak acid and its conjugate base.

Identify the components of the buffer: In this problem, the buffer is made of acetic acid (HC2H3O2) and its conjugate base, sodium acetate (NaC2H3O2).

Calculate the initial moles of each component: Use the formula \( \text{moles} = \text{concentration} \times \text{volume} \). For HC2H3O2, calculate \( 0.100 \text{ M} \times 0.050 \text{ L} \). For NaC2H3O2, calculate \( 0.100 \text{ M} \times 0.060 \text{ L} \).

Analyze the effect of adding each substance: Adding a strong base like NaOH will react with the weak acid, potentially depleting it and destroying the buffer. Calculate the moles of NaOH added and compare it to the moles of HC2H3O2 to see if it exceeds the buffer capacity.

Consider the effect of adding HCl: Adding a strong acid like HCl will react with the conjugate base, potentially depleting it. Calculate the moles of HCl added and compare it to the moles of NaC2H3O2 to determine if it exceeds the buffer capacity.