1 / 17

The Chemistry of Acids & Bases

The Chemistry of Acids & Bases. Properties of Acids. Lemons have citric acid!. Vinegar has acetic acid!. Dilute solution have a _____taste Aqueous solutions conduct an electric current  What do we call substances that can conduct electric currents?

kendall-tran
Download Presentation

The Chemistry of 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. The Chemistry of Acids & Bases

  2. Properties of Acids Lemons have citric acid! Vinegar has acetic acid! • Dilute solution have a _____taste • Aqueous solutions conduct an electric current  What do we call substances that can conduct electric currents? **The greater the # of ions in solution, the greater the electrical conductivity. • Acids react with bases to form a water & salt  _____________________ • Acids react with certain metals to produce H2 gas  Table J: _____________________________ • Acids cause acid-base indicators to change color _________________ Strong acid = Weak acid =

  3. Properties of Bases • Bases have a bitter taste. • Bases have a slippery or soapy feeling. • Bases conduct an electric current. • Bases react with acids to form water & salt. • Bases cause acid-based indicators to change color. Strong base= Weak base =

  4. Arrhenius Theory • Arrhenius Acid = ______________________________________ ______________________________________ - Ex: **Some notes on the hydrogen ion!:  H+ is really just a _________!  In a water solution, the positively charged proton is attracted to an unshared pair of electrons in the water molecules. Proton ends up covalently bonding with water to form _______________________ http://hogan.chem.lsu.edu/matter/chap26/animate3/an26_037.mov

  5. So, acids dissolve in water & react to produce ______________ & ________________. H2SO4  2H3O+ (aq) + SO42- (aq) H3SO4  3H3O+ (aq) + SO42- (aq)

  6. Arrhenius Theory • Arrhenius Base: = _____________________________________________ _____________________________________________ - Remember: hydroxide ion = OH- NaOH  Na+(aq) + OH- (aq) KOH  K+(aq) + OH- (aq) http://hogan.chem.lsu.edu/matter/chap26/animate3/an26_038.mov

  7. Other Acid/Base Definitions Brønsted – Lowry Acids = _____________ Brønsted – Lowry Bases = _____________ Note: A “proton” is really just a hydrogen atom that has lost it’s electron! Lewis acid = _____________________________ Lewis base = _____________________________

  8. Neutralization Reactions = an Arrhenius acid reacts with an Arrhenius base to produce water & a salt • General reaction: **All neutralization reactions have the same net equation: = http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/animations/HClandNaOHtgV8.html

  9. Acid-Base Titration = the process of adding measured volumes of an acid or base of known concentration to an acid or base of unknown concentration until neutralization takes place • Through a titration, it is possible to calculate the concentration of the unknown solution: MAVA = MBVB http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/flashfiles/stoichiometry/acid_base.html

  10. Monoprotic Acid: H+ molarity = molarity of acid solution - Ex: 2.5M HCl = 2.5M H+ Diprotic Acid: H+ molarity = 2 x molarity of acid solution - Ex: 2.5M H2SO4 = ___ H+ Triprotic Acid: H+ molarity = 3 x molarity of acid solution - Ex: 2.5M H3SO4 = ___ H+ Monohydroxy Bases: OH- molarity = molarity of base solution - Ex: 3.0M NaOH = ___ OH- Dihydroxy Bases: OH- molarity = 2 x molarity of base solution - Ex: 3.0M Ba(OH)2 = ___ OH-

  11. Acidity vs. Alkalinity ** These terms refer to the relative strength of the acid or base in terms of H+ and OH- concentrations.** • Acidity ___________________________ • Alkalinity _________________________ [H+] > [OH-] :_________ [H+] < [OH-] :_________

  12. pH Scale • The pH scale expresses [H+] as a number from 0 to 14 • Each pH unit represents a tenfold increase or decrease in [H+] and [OH-]. • As [H+] increases, [OH-] decreases (and vice-versa).

  13. Acid-Base Indicators Indicator = ____________________________________ ____________________________________ **REMEMBER: Everything you need to know about acid-base indicators is on Table M in the reference tables!!** http://hogan.chem.lsu.edu/matter/chap27/demos/dm27_010.mov

More Related