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, c ac2h 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

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10. Acids and Bases

Buffers

GOB Chemistry

10. Acids and Bases

Buffers

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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

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Verified step by step guidance

Understand that a buffer solution resists changes in pH upon the addition of small amounts of acid or base. It typically consists of a weak acid and its conjugate base.

Identify the components of the buffer: HC2H3O2 (acetic acid) is the weak acid, and NaC2H3O2 (sodium acetate) provides the conjugate base, C2H3O2⁻.

Calculate the initial moles of HC2H3O2 and NaC2H3O2 in the buffer. Use the formula: moles = concentration (M) × volume (L).

Consider the effect of adding strong acids or bases. Adding a strong base like NaOH will react with the weak acid, potentially depleting it and destroying the buffer capacity if added in sufficient quantity.

Evaluate the given options: Determine which addition would neutralize a significant portion of the buffer components, particularly the weak acid, thus destroying the buffer's ability to resist pH changes.