1. 1. Neutralization
2. NaOH + HCl  H2O + NaCl
2NaOH + H2SO4  2H2O + Na2SO4
3. Twice as much HCl was required. Because it takes twice as much HCl (one H) as H2SO4 (two Hs) to neutralize the same amount of NaOH

2. 4. H2SO4(aq) + 2NaOH(aq)  2H2O + Na2SO4(aq)
# L H2SO4=
L NaOH
0.60 mol NaOH
L NaOH x
1 mol H2SO4
2 mol NaOH x
L H2SO4
0.175 mol H2SO4 x
= L = 17.1 mL
5. #H x MA x VA = #OH x MB x VB

3. Titration problems
What volume of 0.10 mol/L NaOH is needed to neutralize 25.0 mL of 0.15 mol/L H3PO4?
25.0 mL of HCl(aq) was neutralized by 40.0 mL of 0.10 mol/L Ca(OH)2 solution. What was the concentration of HCl?
A truck carrying sulfuric acid is in an accident. A laboratory analyzes a sample of the spilled acid and finds that 20 mL of acid is neutral-ized by 60 mL of 4.0 mol/L NaOH solution. What is the concentration of the acid?
What volume of 1.50 mol/L H2S will neutral-ize a solution containing 32.0 g NaOH?

4. Titration problems 1. (3)(0.15 M)(0.0250 L) = (1)(0.10 M)(VB)
VB= (3)(0.15 M)( L) / (1)(0.10 M) = 0.11 L
2. (1)(MA)( L) = (2)(0.10 M)(0.040 L)
MA= (2)(0.10 M)(0.040 L) / (1)( L) = 0.32 M
3. Sulfuric acid = H2SO4
(2)(MA)(0.020 L) = (1)(4.0 mol/L)(0.060 L)
MA = (1)(4.0 M)(0.060 L) / (2)(0.020 L) = 6.0 M
4. mol NaOH = 32.0 g x 1 mol/40.00 g = (2)(1.50 mol/L)(VA) = (1)(0.800 mol)
VA= (1)(0.800 mol) / (2)(1.50 mol/L) = L

5. Titration summary For titrations we use the formula:
#H x MA x VA = #OH x MB x VB
Or NA x VA = NB x VB
NA is the combination of MA and #H
N is also known as normality
You can think of it a neutralizing power
We will stick with the first equation, you do not have to know N or what it stands for
This is a simplification of stoichiometry. We could get the same answer by working with moles (n = MV) and by using the balanced chemical equation

6. Titration showdown
Titration competition (best with a burette): find the concentration of an H2SO4 solution – it could be anywhere from 0-18 mol/L
You will use the NaOH that you prepared two weeks ago and your vast knowledge of titration procedures and formulas.
The wining team, is the team closest to the correct value.
The only restriction is : don’t put base in the burette – only acid.

7. For more lessons, visit www.chalkbored.com
Sources of error
NaOH was not exactly 0.10 mol/L
Calculation errors (e.g. converting mL to L)
Not rinsing and drying the beaker for the acid
Over titrating (ideally, 2 titrations should be done – one to get a rough estimate, and one to get the exact value).
Acid or base left on the side of the flask or on the tip of the burette (for greater precision, water is used to rinse the tip of the burette).
Errors reading volumes.
Using pipette (10 mL is measured from 0 mL to 10 mL, not from 10 mL to empty)
Using 10 mL of base vs mL
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