Download presentation
Presentation is loading. Please wait.
1
Acids and Bases/Equilibrium
(EXTREMELY IMPORTANT) a. Molarity mol/L b. Molality mol/kg c. Parts per million gsolute/gsolvent x d. pH from [H+] -log[H+] e. [H+] from pH 10-pH f. [H+] from [OH-] 1.0 x 10-14/[OH-1]
2
Acids and Bases/Equilibrium
(ALSO EXTREMELY IMPORTANT) 2. What is the pH range of an acid? 0-7 What is the pH range of a base? 7-14 What is neutral? 7 3. The hydrogen ion (hydronium ion) concentration 4. The equivalence point needs to fall within the transition range of the indicator 5. #H+ Macid Vacid = #OH- Mbase Vbase
Similar presentations
![Acids and Bases. Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0 10 -14.](/8/2465222/big_thumb.jpg "Acids and Bases. Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0 10 -14.>")
![Calculating pH and pOH. pH pH = - log [H + ] [H + ] = the hydrogen ion concentration pH: “potential of hydrogen” - A way of expressing the hydrogen ion.](/17/5302527/big_thumb.jpg "Calculating pH and pOH. pH pH = - log [H + ] [H + ] = the hydrogen ion concentration pH: “potential of hydrogen” - A way of expressing the hydrogen ion.>")
![pH scale Logarithmic scale expressing the H + concentration, [H + ]. If the pH changes by a factor of 1, the [H + ] changes by a factor of 10. pH =](/22/6410049/big_thumb.jpg "pH scale Logarithmic scale expressing the H + concentration, [H + ]. If the pH changes by a factor of 1, the [H + ] changes by a factor of 10. pH =>")
