Question
Calculate the pH of a buffer made by dissolving 1 mol formic acid $(\mathrm{HCOOH})$ and 1 mol sodium formate $(\mathrm{HCOONa}$ ) in 1 L of solution (see Table 9.9).
Step 1
In this case, we have formic acid (HCOOH) as the weak acid and sodium formate (HCOONa) as the conjugate base. Show more…
Show all steps
Your feedback will help us improve your experience
David Collins and 82 other educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
What is the pH of a buffer solution made by dissolving $0.10 \mathrm{mol}$ of formic acid, $\mathrm{HCOOH}$, and $0.10 \mathrm{mol}$ of sodium formate, HCOONa, in 1 L of water?
What is the pH of a buffer solution made by dissolving 0.10 mol of formic acid, HCOOH, and 0.10 mol of sodium formate, HCOONa, in 1 L of water? pKa of formic acid is 3.75.
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD