Chapter Fifteen 1 Hall © 2005 Prentice Hall © 2005 General Chemistry 4 th edition, Hill, Petrucci, McCreary, Perry Acids, Bases, and Acid–Base Equilibria.
Mullis Acids, Bases and Salts Acids give up hydrogen ions (H + ) in a water solution. Bases give up hydroxide ions (OH - ) in a water solution.
Init: 5/25/2011 by Daniel R. Barnes. 1.H 2 O 2. H 2 SO 4 3.NaCl 4.NaOH 5.HCl 6.NaHCO 3 Our Samples: 7.NaClO 8.NH 3 9.CH 3 COOH 10. CH 3 CHOHCH 3 11. C.
PH = - log [H 3 O + ] [H 3 O + ] = 10 - pH mol/L For pure water at 25 o C pH = - log (1.0 x 10 -7 ) = 7.00 For a change in pH by 1, H 3 O + concentration.
Strong Acid-Weak Base and Weak Acid - Strong Base.
19-1 CHEM 1B: GENERAL CHEMISTRY Chapter 19: Ionic Equilibria in Aqueous Systems Instructor: Dr. Orlando E. Raola Santa Rosa Junior College.
Acid/Base Chemical Equilibria. The Brønsted Definitions Brønsted Acid proton donor Brønsted Base proton acceptor Conjugate acid - base pair.
Chapter 8 Acids and Bases and Oxidation- Reduction Denniston Topping Caret 6 th Edition Copyright The McGraw-Hill Companies, Inc. Permission required.
Chapter 16 Acid–Base Equilibria Lecture Presentation James F. Kirby Quinnipiac University Hamden, CT © 2015 Pearson Education, Inc.
Chapter 8 Acids and Bases and Oxidation-Reduction Denniston Topping Caret 5 th Edition Copyright The McGraw-Hill Companies, Inc. Permission required.
Chapter 15. Bronsted Lowry Acids and Bases An acid is a proton donor and a base is a proton acceptor. The loss of a proton is called as deprotonation:
![PH = - log [H 3 O + ] [H 3 O + ] = 10 - pH mol/L For pure water at 25 o C pH = - log (1.0 x 10 -7 ) = 7.00 For a change in pH by 1, H 3 O + concentration.](https://static.fdocuments.in/doc/330x215/56649d4c5503460f94a29c0c/ph-log-h-3-o-h-3-o-10-ph-moll-for-pure-water-at-25-o-c-ph.jpg)
