1 / 14

Acids & Bases

Acids & Bases. SC7. Students will characterize the properties that describe solutions and the nature of acids and bases. b. Compare, contrast, and evaluate the nature of acids and bases: • Arrhenius, Bronsted-Lowry Acid/Bases • Strong vs. weak acids/bases in terms of percent dissociation

Download Presentation

Acids & 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. Acids & Bases SC7. Students will characterize the properties that describe solutions and the nature of acids and bases. b. Compare, contrast, and evaluate the nature of acids and bases: • Arrhenius, Bronsted-Lowry Acid/Bases • Strong vs. weak acids/bases in terms of percent dissociation • Hydronium ion concentration • pH • Acid-Base neutralization

  2. Properties of Acids: Sour Taste Electrolytes Change indicator colors React with metals to form hydrogen React with carbonates to form carbon dioxide React with bases to form salt & water Properties of bases: Bitter Feel Slippery Electrolytes Change indicator colors React with acids to produce salt & water Properties

  3. What Are Acids? • Definitions • Arrhenius acid: Produce H+ ion • Arrhenius base: Produce OH- ion • Bronsted-Lowery Acid: H+ donor • Bronsted Lowery Base: H+ acceptor • **More Broad definition than Arrhenius** • Lewis acid- can accept pr of e- to form a covalent bond (H+) • Lewis base- can donate pr of e- to form a covalent bond (OH-) • Look for lone pr • ** is more broad than other two def Amphoteric- can be acid or base

  4. Arrhenius acid • Acids Form H+ Ions when Dissolved in Water Ex HCl + H20 dH+ + Cl- + H20 Actually it forms H3O+ & Cl-

  5. HCl +H2O  H3O+ + Cl- Monoprotic Acid- Produces 1 Hydrogen Ion Hydrogen Ion concentration can be measured in molarity H2SO4+2H2O  2H3O++ SO4-2 Di-protic acids- Produces 2 Hydrogen Ions

  6. Hydronium IonConcentration • H+ or H3O ion concentration can be measured in molarity • Depends on # of Hydrogen Ions per Mole of Acid. • Monoprotic 1x HCl • Diprotic 2x H2SO4 • Triprotic 3x H3PO4 More on That Later?

  7. Arrhenius Base • Form a Hydroxide Ion (OH-) During Solvation • NaOH + H2O d Na+ + OH- + H2O • Name Bases according to Ionic Rules • Most are hydroxides • NaOH – sodium hydroxide • OH- Ion Concentration can also be measured in Molarity

  8. Neutralization • - Double displacement Reaction • Acid + Base  salt + water • Nitric acid & calcium hydroxide • Sulfuric acid & aluminum hydroxide • Can find acid & base that form salt • NaCl • NaHCO3

  9. Self Ionization Of Water • H2O (HOH) can self Ionize into a H+ & an OH- • H2O + H2O  H3O+ + OH- • Hydronium ion H3O+ • Hydroxide ion OH- • Only 1X 10 –14 M of water molecules do this so [H3O+][OH-] = 1X 10 –14 M • If [H3O+]=[OH-] neutral solution • If [H3O+]>[OH-] acidic solution • If [H3O+]<[OH-] basic or alkaline solution

  10. Ionization Constants • A constant (k), is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation • HA  H+ + A-

  11. Strengths of Acids and Bases • The strength of an acid or a base, is a measure of how many ions are formed when dissolved in water • Strong Acids Disassociate completely • Weak Acids do not completely Disassociate • Weak acids have Ka

  12. Acids HCl HBr HI HNO3 H2SO4 HClO3 HClO4 Bases LiOH NaOH KOH RbOH CsOH Ca(OH)2 Sr(OH)2 Mg(OH)2 Strong Acids & Bases

  13. pH Scale • pH=-Log[H3O] • pOH=-log[OH-] • pH+pOH=14 • pH 1-6 7 8-14 • Acid neutral base • pOH 14-8 7 6-1 • pH +pOH=14 • Use to find one given the other. • Find the pOH if the pH is 8.2.

  14. Calculate the pH of a solution of HCl if the [H3O+] is 0.234 M 1) A 0.001 M solution of HCl 2) A 0.09 M solution of HBr 3) A 1.34 x 10-4 M solution of HCl 4) A 2.234 x 10-6 M solution of HI 5) A 7.98 x 10-2 M solution of HNO3

More Related