Question
A citric acid-citrate buffer has a pH of 3.20 . You want to increase the pH to a value of 3.35 . Would you add citric acid or sodium citrate to the solution? Explain.
Step 1
A citric acid-citrate buffer consists of citric acid (the weak acid) and sodium citrate (the conjugate base). The pH of the buffer is determined by the ratio of these two components according to the Henderson-Hasselbalch equation. Show more…
Show all steps
Your feedback will help us improve your experience
David Collins and 52 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
Citric acid is an organic acid naturally present in citrus fruits. In a chemistry lab, a citric acid/sodium citrate buffer has a pH of 3.20. You are asked to raise the pH of the buffer to a value of 4.20. What do you add? [Select all that apply] Group of answer choices sodium citrate citric acid citronella hydrochloric acid sodium hydroxide
Citric acid (C6H8O7) is a triprotic acid with pKa values of 3.1, 4.8 and 6.4. You are provided with solid sodium citrate (Na3C6H5O7, 258.05 g/mol) and 6.00 M HCl. Calculate and explain how you would prepare 550.0 mL of a 0.30 M citrate buffer with a pH of 4.6. You don't need to show your work but should include answers to steps you used to get the final answer (this will help with part marks if your final answer is incorrect).
Suppose you have a phosphate buffer $\left(\mathrm{H}_{2} \mathrm{PO}_{4}^{-} / \mathrm{HPO}_{4}^{2-}\right)$ of pH 7.21 . If you add more solid $\mathrm{NaH}_{2} \mathrm{PO}_{4}$ to this buffer, would you expect the pH of the buffer to increase, decrease, or remain unchanged? Explain.
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD