What ratio of acid to base is needed to prepare a buffer with a pH = 4.0 using the conjugate pair HCOOH/HCOO-1 (Ka = 1.78x10^-4)? A [HCOOH]/[HCOO-] = 1.78 B [HCOOH]/[HCOO-] = 0.250 C [HCOOH]/[HCOO-] = 3.99 D [HCOOH]/[HCOO-] = 0.562
Added by Teresa C.
Close
Step 1
We know that the pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]) Show more…
Show all steps
Your feedback will help us improve your experience
Madhur L and 61 other Chemistry 101 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
You want to prepare a buffer solution with a pH of 4.5. Which acid / conjugate base pair is the best choice? 1) CH3COOH / CH3COO- Ka = 1.8 x 10-5 2) HNO2 / NO2- Ka = 4.5 x 10-4 3) H2PO4- / HPO42- Ka = 7.5 x 10-3 4) HSeO4- / SeO42- Ka = 1.2 x 10-2 5) HIO3 / IO3- Ka = 1.7 x 10-1
David C.
What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 4.5? The pKa value of the acid is 4.05 at 250C.
John I.
What ratio of NaCHO2:HCHO2 would be required to make a buffer with pH 3.73? Formic Acid, HCHO2 pKa = 3.74
Sri K.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD