Your SlideShare is downloading. ×
  • Like
Acid & base
Upcoming SlideShare
Loading in...5

Thanks for flagging this SlideShare!

Oops! An error has occurred.


Now you can save presentations on your phone or tablet

Available for both IPhone and Android

Text the download link to your phone

Standard text messaging rates apply


Published in Education , Business , Technology
  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
    Be the first to comment
    Be the first to like this
No Downloads


Total Views
On SlideShare
From Embeds
Number of Embeds



Embeds 0

No embeds

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

    No notes for slide


  • 1. By : Siti Auliaddina
  • 2. Do you know the definition of acids and bases in general ?
  • 3. Produce H+ (as H3O+) ions in waterProduce a negative ion (-) tooTaste sourCorrode metalsReact with bases to form salts and water
  • 4.  Produce OH- ions in water Are electrolytes Feel soapy, slippery React with acids to form salts and water LecturePLUS Timberlake 4
  • 5. • Used for acid and bases in solution (neutralization)• Cations (positive ions) derived from the bases and anions (negative ions) derived from acid• Salt: compounds which can remove ion of• H + positive and negative ion of non OH-
  • 6.  Acids produce H+ in aqueous solutions water HCl H+(aq) + Cl- (aq) Bases produce OH- in aqueous solutions water NaOH Na+(aq) + OH- (aq)
  • 7. • In this idea, the ionization of an acid by water is just one example of an acid-base reaction. H H + Cl H + O HO + Cl H H acid base conjugate acid conjugate base conjugate acid-base pairs• Acids and bases are identified based on whether they donate or accept H+.• “Conjugate” acids and bases are found on the products side of the equation. A conjugate base is the same as the starting acid minus H+.
  • 8. Arrehenius  Acids – produce H+ only in water  Bases - produce OH-  Acids – donate H+ Bronsted-Lowry  Bases – accept H+ any solvent Lewis  Acids – accept e- pairused in organic chemistry,  Bases – donate e- pairwider range of substances
  • 9. Acid, Base Name or SaltCaCl2 ______ _________________KOH ______ _________________Ba(OH)2 ______ _________________HBr ______ _________________H2SO4 ______ __________________
  • 10.  The pH scale measures how acidic or basic a solution is.
  • 11.  The pH scale is the concentration of hydrogen ions in a given substance. pH log H
  • 12.  Acids have a ph from 0-7 Lower pH value indicates a stronger acid. Bases have a pH from 7-14 Higher pH value indicates a stronger base.
  • 13. Strong acids/bases – 100% dissociation into ions HCl NaOH HNO3 KOH H2SO4Weak acids/bases – partial dissociation, both ions and molecules CH3COOH NH3 Weak Acid Weak Base
  • 14. pH of Rainwater across United States in 2001 You are here!Why is the eastern US more acidic?
  • 15. Dissolved carbon dioxide lowers the pHCO2 (g) + H2O  H2CO3  H+ + HCO3-Atmospheric pollutants from combustionNO, NO2 + H2O …  HNO3 both strong acidsSO2, SO3 + H2O …  H2SO4 pH < 5.3