Thank you for visiting Given a 250 mL buffer with a pH of 4 10 and a pKa of 3 74 containing 35 9 g of NaCOOH how many. This page is designed to guide you through key points and clear explanations related to the topic at hand. We aim to make your learning experience smooth, insightful, and informative. Dive in and discover the answers you're looking for!
Answer :
To solve this problem, we'll use the Henderson-Hasselbalch equation, which relates the pH of a buffer solution to the pKa of the acid and the ratio of the concentrations of the conjugate base to the weak acid.
The Henderson-Hasselbalch equation is:
pH = pKa + log ([base][acid])
Given that the pH of the buffer solution is 4.10 and the pKa of the acid is 3.74, we can rearrange the Henderson-Hasselbalch equation to solve for the ratio of base to acid:
pH = pKa + log ([base][acid])
10pH-pKa = [base][acid]
[base] = [acid] x 10pH-pKa
Since we know the concentration of the base (NaCOOH) and the acid (formic acid) are equal in a buffer solution, we can find the concentration of the acid using the given concentration of the base.
First, let's find the concentration of NaCOOH in the buffer solution:
Molarity of NaCOOH = moles of NaCOOH
Volume of solution (L)
Given that the volume of the buffer solution is 250 mL (0.250 L), and the molar mass of NaCOOH is 68.01 g/mol, we can find the moles of NaCOOH:
moles of NaCOOH = mass \ molar mass
moles of NaCOOH = 35.9g \ 68.01g\mol
moles of NaCOOH = 0.527 mol
Now, using the Henderson-Hasselbalch equation, we can find the concentration of formic acid (HCOOH) in the buffer solution:
[base] = [acid] x 10^pH-pKa
0.527 = [acid] x 10^4.10- 3.74
0.527 = [acid] x 10^0.39
[acid] = 0.527 \ 10^0.36
[acid] = 0.335 mol
Therefore, the moles of formic acid needed are approximately 0.335 mol, which is closest to option:
c) 0.30 mol
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