CHEM123L Lecture Notes - Lecture 4: Buffer Solution, Ph Meter, Conjugate Acid

455 views1 pages

Document Summary

With acid strengths referring to the ability of the acid to relinquish protons, the stronger the acid, the more easily it gives up on its protons. The relationship if inversely related to the strength of its conjugate base. As such, the stronger the acid, the weaker the conjugate base, and the stronger the base, the weaker the conjugate acid. The equilibrium constant will (cid:271)e used su(cid:272)h a weak a(cid:272)id"s (cid:272)onstant is also known as an a(cid:272)id ionization constant, ka. The equilibrium equation c6h5oh(aq) h+ + c6h5o- will be used to determining. Ka as 1. 28 x 10-10 for a weak acid. This is further used to identify the concentration of an unknown hcl. Buffers solutions are solutions that resist change in ph. , or henderson-hasselbalch equation calculated using the ka expression k=[+][ ] (cid:1868)= pk+(cid:1867)[ ] When increasing the concentration of the conjugate acid and base, the stronger the resisting ability of change in ph.

Get access

Grade+20% off
$8 USD/m$10 USD/m
Billed $96 USD annually
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
40 Verified Answers
Class+
$8 USD/m
Billed $96 USD annually
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
30 Verified Answers

Related textbook solutions

Related Documents

Related Questions