Download presentation
Presentation is loading. Please wait.
1
pH and pOH By: Sam F., Sam D., Rochani, Evan, Will, Sherry, Mariana
2
pH ● Measure of the acidity or basicity of an aqueous solution ● Acid: 0 - 7 ● Base: 7 - 14 ● 7 is neutral
3
pH Calculation ● pH=-log [H+] ● Molarity of acid = [H+] ● Ex: o.1 M HCl what is the pH? o.001 M HBr what is the pH?
![pH Calculation ● pH=-log [H+] ● Molarity of acid = [H+] ● Ex: o.1 M HCl what is the pH.](http://images.slideplayer.com./9/2504102/slides/slide_3.jpg "o.001 M HBr what is the pH .")
4
pOH ● measures the concentration of the hydroxide ion ● Acid: 7-14 ● Base: 0-7 ● 7 is neutral
5
pOH Calculation ● pOH= -log [OH-] ● Molarity of base= [OH-] ● Ex: o.0001 M Ca(OH)2 what is pOH? o.01 M Ba(OH)2 what is pOH?
![pOH Calculation ● pOH= -log [OH-] ● Molarity of base= [OH-] ● Ex: o.0001 M Ca(OH)2 what is pOH.](http://images.slideplayer.com./9/2504102/slides/slide_5.jpg "o.01 M Ba(OH)2 what is pOH .")
6
pH and pOH scale
7
Relationship ● Use this to find the pH or pOH: o pH+pOH=14 ● Ex: o.001 M NaOH what’s the pH? o.000001 M HCl, what’s the pOH?
8
Relationship ● To find [H+] and [OH-] use: o [OH-]=10^-pOH o [H+]=10^-pH ● Ex: o pH is 7.4 what is the [H+]? o pOH is 6.3 what is [OH-]?
![Relationship ● To find [H+] and [OH-] use: o [OH-]=10^-pOH o [H+]=10^-pH ● Ex: o pH is 7.4 what is the [H+].](http://images.slideplayer.com./9/2504102/slides/slide_8.jpg "o pOH is 6.3 what is [OH-] .")
Similar presentations
![PH. There is a formula to find pH pH = -log [H + ] or pH = -log [H 3 O + ] – (brackets around a substance means that substances concentration in molarity)](/8/2422811/big_thumb.jpg "PH. There is a formula to find pH pH = -log [H + ] or pH = -log [H 3 O + ] – (brackets around a substance means that substances concentration in molarity)>")
![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.>")
![PH Scale. Ion product constant for water K w H 2 O H + + OH - K w = [H + ] [OH - ] = 1.0 X 10 -14 mol/L Since [H + ] = [OH - ] for water Then each equals.](/9/2504100/big_thumb.jpg "PH Scale. Ion product constant for water K w H 2 O H + + OH - K w = [H + ] [OH - ] = 1.0 X 10 -14 mol/L Since [H + ] = [OH - ] for water Then each equals.>")
![Continuing into the world of acids and bases…. pH of a solution is the negative logarithm of the hydrogen ion concentration pH = -log [H + ] This.](/9/2504106/big_thumb.jpg "Continuing into the world of acids and bases…. pH of a solution is the negative logarithm of the hydrogen ion concentration pH = -log [H + ] This.>")
![pH Water Water is in equilibrium with its ions H 2 O(l) H + (aq) + OH - (aq) K w = [H + ][OH - ] K w = 1.0 x 10 -14 at 25°C In neutral solutions [H.](/9/2516310/big_thumb.jpg "pH Water Water is in equilibrium with its ions H 2 O(l) H + (aq) + OH - (aq) K w = [H + ][OH - ] K w = 1.0 x 10 -14 at 25°C In neutral solutions [H.>")
