Titration Curves What’s in the beaker. Always ask… What’s in the beaker? When I start the...
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Transcript of Titration Curves What’s in the beaker. Always ask… What’s in the beaker? When I start the...
Always ask…
What’s in the beaker?
When I start the titration, there is only water and whatever it is I’m titrating (and maybe indicator, but we’ll ignore that).
Let’s titrate HCl with NaOH
10.00 mL of 0.100 M HCl diluted with 50.0 mL of water
What’s in the beaker?
Cl-
H2O
Cl-
H2O
Cl-
H2O
H+
H+
H+
I know what’s in the beaker…
Now I ask: what reactions are possible?
Cl-
H2O
Cl-
H2O
Cl-
H2O
H+
H+
H+
“What reactions are possible”?
H+ + H2O H+ + H2O
Cl- + H2O HCl + OH-
H2O + H2O H3O+ + OH-
Which reactions matter?
NONE!
Cl-
H2O
Cl-
H2O
Cl-
H2O
H+
H+
H+
“What reactions are possible”?
H+ + H2O H+ + H2O
Cl- + H2O HCl + OH-
H2O + H2O H3O+ + OH-
10.00 mL of 0.100 M HCl diluted with 50.0 mL of water
What’s the pH?
0.100 M * 10.0 mL = [HCl]* 60.0 mL
[HCl] = 1.667x10-2 M = [H+] = [Cl-] (it’s a strong acid)
pH = - log (1.667x10-2 M) = 1.778
10.00 mL of 0.100 M HCl diluted with 50.0 mL of water. Then add 2.00 mL of 0.100 M
NaOH.What’s in the beaker?
Cl-
H2O
Cl-
H2O
Cl-
H2O
H+
Na+
H+
I know what’s in the beaker…
Now I ask: what reactions are possible?
Cl-
H2O
Cl-
H2O
Cl-
H2O
Na+
H+
H+
“What reactions are possible”?
H+ + H2O H+ + H2O
Cl- + H2O HCl + OH-
Na+ + H2O NaOH + H+
H2O + H2O H3O+ + OH-
Which reactions matter?
NONE!
Cl-
H2O
Cl-
H2O
Cl-
H2O
H+
H+
H+
“What reactions are possible”?
H+ + H2O H+ + H2O
Cl- + H2O HCl + OH-
Na+ + H2O NaOH + H+
H2O + H2O H3O+ + OH-
10.00 mL of 0.100 M HCl diluted with 50.0 mL of water. Then add 2.00 mL of 0.100 M
NaOH.What’s the pH? I like an ICE chart here, just to keep track of
things!
Moles is better for my ICE chart because of dilution issues.
0.100 M * 0.0100 L = 0.00100 moles HCl initial
0.100 M NaOH * 0.00200 L = 0.0002 mol NaOH
Always start with a balanced equation. Which one?
H+ + OH- H2O
I 0.001 mol 0.0002 mol -
C -0.0002 mol -0.0002 mol -
End 0.0008 mol 0 mol
So….
0.0008 mol H+ = 1.29x10-2 M
0.062 L
pH = - log(1.29x10-2 M) = 1.889
Notice, not a lot of change.
10.00 mL of 0.100 M HCl diluted with 50.0 mL of water. Then add 5.00 mL of 0.100 M
NaOH.What’s the pH? I like an ICE chart here, just to keep track of
things!
Moles is better for my ICE chart because of dilution issues.
0.100 M * 0.0100 L = 0.00100 moles HCl initial
0.100 M NaOH * 0.00500 L = 0.0005 mol NaOH
Always start with a balanced equation. Which one?
H+ + OH- H2O
I 0.001 mol 0.0005 mol -
C -0.0005 mol -0.0005 mol -
End 0.0005 mol 0 mol
So….
0.0005 mol H+ = 7.69x10-3 M
0.065 L
pH = - log(7.69x10-3 M) = 2.114
Notice, not a lot of change.
10.00 mL of 0.100 M HCl diluted with 50.0 mL of water. Then add 10.00 mL of 0.100 M
NaOH.What’s the pH? I like an ICE chart here, just to keep track of
things!
Moles is better for my ICE chart because of dilution issues.
0.100 M * 0.0100 L = 0.00100 moles HCl initial
0.100 M NaOH * 0.0100 L = 0.00100 mol NaOH
Always start with a balanced equation. Which one?
H+ + OH- H2O
I 0.001 mol 0.001 mol -
C -0.001 mol -0.001 mol -
End 0.00 mol 0 mol
So….
Nothing left….so is [H+] = 0?
Suddenly, one of my reactions is relevant:
H2O + H2O H3O+ + OH-
The pH is 7 at equivalence because of the Kw
reaction.
10.00 mL of 0.100 M HCl diluted with 50.0 mL of water. Then add 12.00 mL of 0.100 M
NaOH.What’s in the beaker?
Cl-
H2O
Cl-
H2O
Cl-
H2O
Na+
Na+
Na+
Na+
OH-
OH-
OH-
Na+
Na+
I know what’s in the beaker…
Now I ask: what reactions are possible?
“What reactions are possible”?
OH- + H2O OH- + H2O
Cl- + H2O HCl + OH-
Na+ + H2O NaOH + H+
H2O + H2O H3O+ + OH-
Cl-
H2O
Cl-
H2O
Cl-
H2O
Na+
Na+
Na+
10.00 mL of 0.100 M HCl diluted with 50.0 mL of water. Then add 12.00 mL of 0.100 M
NaOH.What’s the pH? I like an ICE chart here, just to keep track of
things!
Moles is better for my ICE chart because of dilution issues.
0.100 M * 0.0100 L = 0.00100 moles HCl initial
0.100 M NaOH * 0.01200 L = 0.0012 mol NaOH
Always start with a balanced equation. Which one?
H+ + OH- H2O
I 0.001 mol 0.0012 mol -
C -0.001 mol -0.001 mol -
End 0.00 mol 0.0002 mol
So….
0.0002 mol OH- = 2.778x10-3 M OH-
0.072 L
pOH = - log(2.778x10-3 M) = 2.556
pH = 14 – 2.556 = 11.444
10.00 mL of 0.100 M HCl diluted with 50.0 mL of water. Then add 15.00 mL of 0.100 M
NaOH.What’s the pH? I like an ICE chart here, just to keep track of
things!
Moles is better for my ICE chart because of dilution issues.
0.100 M * 0.0100 L = 0.00100 moles HCl initial
0.100 M NaOH * 0.01500 L = 0.0015 mol NaOH
Always start with a balanced equation. Which one?
H+ + OH- H2O
I 0.001 mol 0.0015 mol -
C -0.001 mol -0.001 mol -
End 0.00 mol 0.0005 mol
So….
0.0005 mol OH- = 6.667x10-3 M OH-
0.075 L
pOH = - log(6.667x10-3 M) = 2.176
pH = 14 – 2.176 = 11.824
10.00 mL of 0.100 M HOAc diluted with 50.0 mL of water
What’s in the beaker?
H2O
HOAc
H2O H2O
HOAc
HOAc
I know what’s in the beaker…
Now I ask: what reactions are possible?
“What reactions are possible”?
HOAc + H2O OAc- + H3O+
H2O + H2O H3O+ + OH-
H2O
HOAc
H2O H2O
HOAc
HOAc
10.00 mL of 0.100 M HOAc diluted with 50.0 mL of water
What’s the pH?
0.100 M * 10.0 mL = [HOAc]* 60.0 mL
[HOAc] = 1.667x10-2 M(initial concentration)
ICE-ICE-BABY-ICE-ICE
Always start with a balanced equation. Which one?
HOAc + H2O OAc- + H3O+
I 1.667x10-2 M - 0 0
C -x - +x +x
E 1.667x10-2 -x - x x
So….
Ka = 1.80x10-5 = (x)(x)
(1.667x10-2 M –X)
Assume x<<1.667x10-2
Ka = 1.80x10-5 = (x)(x)
(1.667x10-2 M)
3.000x10-7 = x2
X= 5.48x10-4 M (works…barely)
pH = - log (5.48x10-4) = 3.26
HOAc + H2O OAc- + H3O+
I 1.667x10-2 M - 0 0
C - 5.48x10-4 M - 5.48x10-4 M 5.48x10-4 M
E 1.612x10-2 -x - 5.48x10-4 M 5.48x10-4 M
10.00 mL of 0.100 M HOAc diluted with 50.0 mL of water. Add 2.00
mL NaOH.What’s in the beaker?
OAc-
H2O
HOAc
H2OOAc-
H2O
Na+
HOAc
Na+HOAc
HOAc
Why?
NaOH + HOAc NaOAc + H2O
I know what’s in the beaker…
Now I ask: what reactions are possible?
“What reactions are possible”?
HOAc + H2O OAc- + H3O+
H2O + H2O H3O+ + OH-
OAc- + H2O HOAc + OH- (but this is the same as the first one)
OAc-
H2O
HOAc
H2OOAc-
H2O
H+
HOAc
H+HOAc
HOAc
10.00 mL of 0.100 M HOAc diluted with 50.0 mL of water. Add 2.00 mL
of NaOH.What’s the pH?
0.100 M * 0.010 L = 0.001 mol HOAc
0.100 M * 0.002 L = 0.0002 mol NaOH
DOUBLE ICE- DOUBLE ICE-BABY-DOUBLE ICE- DOUBLE ICE
Always start with a balanced equation. Which one?
HOAc + NaOH NaOAc + H2O
I 0.0010 mol
0.0002 mol 0 -
C -0.0002 mol
-0.0002 mol
+0.0002 -
E 0.0008 mol
0 mol 0.0002
So….H-H equation
Ka = 1.80x10-5 =
pKa = - log (1.80x10-5) = 4.74
pH = 4.74 + log [OAc-] [HOAc]
pH = 4.74 + log (0.0002) = 4.14 (0.0008)
10.00 mL of 0.100 M HOAc diluted with 50.0 mL of water. Add 5.00
mL NaOH.What’s in the beaker?
OAc-
H2O
HOAc
H2OOAc-
H2O
Na+
HOAc
Na+HOAc
HOAc
Why?
NaOH + HOAc NaOAc + H2O
I know what’s in the beaker…
Now I ask: what reactions are possible?
“What reactions are possible”?
HOAc + H2O OAc- + H3O+
H2O + H2O H3O+ + OH-
OAc- + H2O HOAc + OH- (but this is the same as the first one)
OAc-
H2O
HOAc
H2OOAc-
H2O
Na+
HOAc
Na+HOAc
HOAc
10.00 mL of 0.100 M HOAc diluted with 50.0 mL of water. Add 5.00 mL
of NaOH.What’s the pH?
0.100 M * 0.010 L = 0.001 mol HOAc
0.100 M * 0.005 L = 0.0005 mol NaOH
DOUBLE ICE- DOUBLE ICE-BABY-DOUBLE ICE- DOUBLE ICE
Always start with a balanced equation. Which one?
HOAc + NaOH NaOAc + H2O
I 0.0010 mol
0.0005 mol 0 -
C -0.0005 mol
-0.0005 mol
+0.0005 -
E 0.0005 mol
0 mol 0.0005
So….H-H equation
Ka = 1.80x10-5 =
pKa = - log (1.80x10-5) = 4.74
pH = 4.74 + log [OAc-] [HOAc]
pH = 4.74 + log (0.0005) = 4.74 (0.0005)
10.00 mL of 0.100 M HOAc diluted with 50.0 mL of water. Add 10.00
mL NaOH.What’s in the beaker?
OAc-
H2O
OAc-
H2OOAc-
H2O
Na+
OAc-
Na+OAc-
Na+
Why?
NaOH + HOAc NaOAc + H2O
I know what’s in the beaker…
Now I ask: what reactions are possible?
“What reactions are possible”?
H2O + H2O H3O+ + OH-
OAc- + H2O HOAc + OH-
No more HOAc, no more Ka
OAc-
H2O
Na+
H2OOAc-
H2O
Na+
OAc-
Na+OAc
Na+
10.00 mL of 0.100 M HOAc diluted with 50.0 mL of water. Add 10.00
mL of NaOH.What’s the pH?
0.100 M * 0.010 L = 0.001 mol HOAc
0.100 M * 0.010 L = 0.001 mol NaOH
DOUBLE ICE- DOUBLE ICE-BABY-DOUBLE ICE- DOUBLE ICE
Always start with a balanced equation. Which one?
HOAc + NaOH NaOAc + H2O
I 0.0010 mol
0.0005 mol 0 -
C -0.0010 mol
-0.0010 mol
+0.001 -
E 0 0 mol 0.001
On to the 2nd ICE chart
OAc + H2O HOAc + OH-
I 0.001 mol
0.070 L
- 0. 0
C -x - +x +x
E 6.9x10-2 -x - x x
So….
Kb = Kw = 1.0x10-14 = 5.56x10-10 Ka 1.80x10-5
5.56x10-10 = (x)(x) 0.069-XAssume x<<0.069x10-2
5.56x10-10 = (x)(x) 0.069
3.836x10-11 = x2
X= 6.19x10-6 M
pOH = - log 6.19x10-6 = 5.2pH = 14 – 5.2 = 8.8
OAc + H2O HOAc + OH-
I 0.001 mol
0.070 L
- 0. 0
C -6.19x10-6 M - +6.19x10-6 M +6.19x10-6 M
E 6.9x10-2 - 6.19x10-6 M 6.19x10-6 M