1 / 7

Salts as Acids and Bases

Salts as Acids and Bases. Assuming that only one ion affects the pH. Salt Ionic Compound Dissolves Ions Slosh Ions as Acids Ions as Bases. Cations Sloshing Anions Sloshing. Salts that produce Neutral Solutions. Salts that consist of: Cations of strong bases (K + , Na + , etc.)

teo
Download Presentation

Salts as Acids and Bases

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Salts as Acids and Bases Assuming that only one ion affects the pH. Salt Ionic Compound Dissolves Ions Slosh Ions as Acids Ions as Bases CationsSloshing Anions Sloshing

  2. Salts that produce Neutral Solutions • Salts that consist of: • Cations of strong bases (K+, Na+, etc.) • Anions of strong bases (Cl-, NO3-, etc.) EX. KCl, NaCl, NaNO3, KNO3 Turn to p. 657 LOOK AT TABLE!

  3. Salts that produce Basic Solutions • For any salt whose: • cation has neutral properties (Na+ , K+ , etc) • anion is conjugate base of a weak acid … and Kb can be calculated • Salts as Weak Bases Example: Calculate the pH of a .3 M NaF solution. The Ka for HF is 7.2 x 10-4.

  4. Salts that produce Acidic Solutions • For salts in which/that contain: • The anion is not a base • The cation is the conjugate acid of a weak base • Highly charged metal ion (polarizes the O-H bonds causing H to be more acidic) • The higher the charge of the metal ion, the stronger the acidity of the hydrated ion

  5. Salts as Weak Acids Examples • Calculate the pH of 0.10 M NH4Cl solution. The Kb value for ammonia = 1.8 x 10 -5. • Calculate the pH of 0.10 M AlCl3solution. The Kavalue for Al(H2O)6+3= 1.4 x 10 -5.

  6. What if both ions affect pH?Qualitative Comparisons • Compare Ka of acidic ion to Kb value of basic ion Ka>Kb ACIDIC Ka<Kb BASIC Ka=Kb NEUTRAL

  7. CREATE SUMMARY CHART • Go here http://www.sciencegeek.net/APchemistry/Presentations/14_Salts/index.html • Work through examples!

More Related