1 / 30

ACIDS & BASES

ACIDS & BASES. Acid Nomenclature Flowchart. Oxyacids or Ternary. Binary. NAMES AND FORMULAS A Review. HX means Acid If anion ends in “–ide” Acid name begins with “hydro-” Ends with “–ic ” , followed by “ Acid” HCl – Hydro chlor ic Acid HBr – Hydro brom ic Acid

kasimir-key
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

  2. Acid Nomenclature Flowchart Oxyacids or Ternary Binary

  3. NAMES AND FORMULASA Review HX means Acid If anion ends in “–ide” Acid name begins with“hydro-” Ends with “–ic” , followed by “Acid” HCl – HydrochloricAcid HBr – HydrobromicAcid HCN – Hydrocyanic Acid Binary

  4. NAMES AND FORMULAS If anion ends in “–ite” Acid ends with “–ous”, followed by “Acid” H2SO3 – SulfurousAcid HNO2 – NitrousAcid H3PO3 – PhosphorousAcid Oxyacids or Ternary

  5. NAMES AND FORMULAS If anion ends in “–ate” Acid ends with “–ic” ,followed by “Acid” H2SO4 – SulfuricAcid HNO3 – NitricAcid H3PO4 – PhosphoricAcid

  6. NAMES AND FORMULAS Bases named same as ionic compound NaOH –Sodium Hydroxide (Lye) Ca(OH)2 – Calcium Hydroxide (Lime) Pb(OH)2 –Lead Hydroxide KOH – Potassium Hydroxide

  7. WATER IONIZATION Water molecules in continuous random motion Collisions between two molecules Result in transfer of hydrogen ion H2O + H2O H3O+ + OH- H3O+ = hydronium ion OH- = hydroxide ion

  8. 3 Theories Acid/Base • Theory #1: Arrhenius (traditional) a) Acids – produce H+ ions (or hydronium ions H3O+) in aqueous solution i: Monoprotic Acid gives up 1 H+ (HCL) ii: Diprotic Acid  gives up 2 H+ (H2SO4) iii: Triprotic Acid  gives up 3 H+ (H3PO4) b) Bases – produces OH- ions in aqueous solutions

  9. Arrhenius acid is a substance that producesH+ (H3O+)in water Arrhenius base is a substance that produces OH-in water

  10. Brønsted – Lowry • Theory #2: Brønsted – Lowry a) Acids – proton (H+) donor (H+ is given away) b) Bases – proton (H+) acceptor (H+ gained) A “proton” is really just a hydrogen atom that has lost it’s electron!

  11. A Brønsted-Lowryacidis a proton donor A Brønsted-Lowrybaseis a proton acceptor conjugateacid conjugatebase base acid

  12. Lewis Theory #3 – Lewis a)Lewis acid – electron pair acceptor b) Lewis base – electron pair donor

  13. WATER DISSOCIATION,SIMPLIFIED Dissociation of water: H2O  H+ + OH- One H+ and one OH- produced, so [H+] = [OH-] [ X ] = concentration (Molarity)

  14. PROPERTIES OF ACIDS • Sour or tart taste in foods • Strong Acid = Strong Electrolyte • Release H+ ions in water • Turn blue litmus paper Red

  15. Hydrogen Ion in Water Water + a proton  Hydronium Ion H2O + H+  H3O +1 The H+ ion has no electrons so it attached itself to a water molecule to share its electrons

  16. ARRHENEIUS ACIDS Theory developed by Arrhenius (1859-1927) Defined acids and bases as compounds that ionize to produce H+ and OH-

  17. ARRHENIUS ACIDS Theory: substance that contains hydrogen, and releases the H+ in water HCl + H2O (1) H3O+ (aq) + Cl - (aq)monoprotic H2SO4 + H2O (2) H3O+ (aq) + SO4-2 (aq) diprotic H3PO4 + H2O -(3) H3O+ (aq) + PO4-3 (aq) triprotic

  18. Types of Arrhenius Acids Monoprotic acids contain 1 ionizable proton HCl, HBr, HF, HI Diprotic acids contain 2 ionizable protons H2SO4 Triprotic acids contain 3 ionizable protons H3PO4

  19. PROPERTIES OF BASES • Feels slippery • Bitter taste • Strong Base = Strong Electrolyte • Produce hydroxide ions in water LYE USED IN SOAPMAKING AMMONIA USED IN CLEANING

  20. ARRHENIUS BASES Substance that contains OH and releases the OH- in water. NaOH + H2O  Na+1 (aq) + OH- (aq) Mg(OH)2 + H2O  Mg +2 (aq) + 2OH-(aq)

  21. Complete book practice problems • Pg 609 • #34,43,44,45,46 • Or check your Power packet ( Acids + Bases) pg 9

  22. ALTERNATE THEORIES Not all materials w/ acidic/basic properties in aqueous solution contain H or OH. Do not fit Arrhenius definition of acids and base Johannes Brønsted (1879-1947) and Thomas Lowry (1874-1936) independently proposed a new definition.

  23. Brønsted – Lowry Acids and Bases B/L Acid is a hydrogen ion donor B/L base is a hydrogen ion acceptor Arrhenius acids and bases fit into the Brønsted – Lowry Theory

  24. Brønsted – Lowry Acids and Bases NH3 + H2O g NH4+ + OH- Ammonia is a base accepts hydrogen ion Water is an acid donates hydrogen ion

  25. Brønsted – Lowry Acids and Bases Conjugate Acid Formed when a base gains a hydrogen ion. NH4+ is the Conjugate Acid Conjugate Base What remains when an acid has donated the hydrogen ion. OH- is the Conjugate Base

  26. Brønsted – Lowry Acids and Bases Conjugate Acid Conjugate Base Base Acid

  27. Brønsted – Lowry Acids and Bases Conjugate acid / base pair Two substances that are related by the loss or gain of a hydrogen ion. HCl + H2O g H3O+ + Cl- Water is Amphoteric - Acts as both Acid and Base

  28. Brønsted – Lowry Acids and Bases In General: Conjugate Base of a Strong Acid is weak HCl (acid) has a weak conjugate base in Cl- Conjugate Acid of a Strong Base is weak NaOH (base) has a weak conjugate acid in Na+

  29. ALTERNATE THEORIES Gilbert Lewis (1875-1946) focused on the donation or acceptance of electrons. Lewis acid accepts electrons to form a covalent bond Lewis base donates electrons to form a covalent bond Remember the Lewis Dot Structure? This is the same guy…

More Related