Data collected Experimental Procedure Weigh accurately about 0.51g of KHP and pour into a clean dry beaker. Add 50mL of distilled water and swirl until the solid has dissolved. Vol of NaOH pH added • Using a calibrated pH meter, measure the initial pH of the solution. • Titrate by adding successive portions of about 1mL of the NaOH solution from the buret. 21 6. (mL) 22 6.24 4 22.2 6.31 1 4.05 22.4 6.4 Record the buret reading and the pH after each addition. Decrease portions to 0.2mL when the pH increase by more than 0.3 pH units. • Continue the titration until the pH is about 11.5- 12 2 4.18 22.6 6.46 4.29 22.8 6.58 4 4.41 23 6.71 4.51 23.2 6.89 4.6 23.4 7.23 4.65 23.6 8.55 Procedure for Part One 8 4.77 23.8 9.38 4.86 Standardization of NaOH solution: 24.1 9.93 10 4.93 KHC3H,04 + NaOH → KNAC3H404 + H2O 24.4 10.32 11 5 24.6 10.55 • The exact molarity of the NaOH solution can be determined from the mass of KHP, its molar mass and the total volume of NaOH at the equivalence point determined from the graph. 12 5.08 13 5.15 25 10.84 14 5.23 26 11.19 15 5.31 27 11.38 16 5.38 28.05 11.5 17 5.47 29 11.58 Questions 18 5.58 30 11.66 19 5.69 31 11.72 1. Find equivalence point the data points. 2. Calculate molarity of the NaOH solution from the result (equivalence point). 3. Find volume and pH at the halfway point. 20 5.82 32 11.77 4. Using pKa, find Ka for KHP.
Data collected Experimental Procedure Weigh accurately about 0.51g of KHP and pour into a clean dry beaker. Add 50mL of distilled water and swirl until the solid has dissolved. Vol of NaOH pH added • Using a calibrated pH meter, measure the initial pH of the solution. • Titrate by adding successive portions of about 1mL of the NaOH solution from the buret. 21 6. (mL) 22 6.24 4 22.2 6.31 1 4.05 22.4 6.4 Record the buret reading and the pH after each addition. Decrease portions to 0.2mL when the pH increase by more than 0.3 pH units. • Continue the titration until the pH is about 11.5- 12 2 4.18 22.6 6.46 4.29 22.8 6.58 4 4.41 23 6.71 4.51 23.2 6.89 4.6 23.4 7.23 4.65 23.6 8.55 Procedure for Part One 8 4.77 23.8 9.38 4.86 Standardization of NaOH solution: 24.1 9.93 10 4.93 KHC3H,04 + NaOH → KNAC3H404 + H2O 24.4 10.32 11 5 24.6 10.55 • The exact molarity of the NaOH solution can be determined from the mass of KHP, its molar mass and the total volume of NaOH at the equivalence point determined from the graph. 12 5.08 13 5.15 25 10.84 14 5.23 26 11.19 15 5.31 27 11.38 16 5.38 28.05 11.5 17 5.47 29 11.58 Questions 18 5.58 30 11.66 19 5.69 31 11.72 1. Find equivalence point the data points. 2. Calculate molarity of the NaOH solution from the result (equivalence point). 3. Find volume and pH at the halfway point. 20 5.82 32 11.77 4. Using pKa, find Ka for KHP.
Data collected Experimental Procedure Weigh accurately about 0.51g of KHP and pour into a clean dry beaker. Add 50mL of distilled water and swirl until the solid has dissolved. Vol of NaOH pH added • Using a calibrated pH meter, measure the initial pH of the solution. • Titrate by adding successive portions of about 1mL of the NaOH solution from the buret. 21 6. (mL) 22 6.24 4 22.2 6.31 1 4.05 22.4 6.4 Record the buret reading and the pH after each addition. Decrease portions to 0.2mL when the pH increase by more than 0.3 pH units. • Continue the titration until the pH is about 11.5- 12 2 4.18 22.6 6.46 4.29 22.8 6.58 4 4.41 23 6.71 4.51 23.2 6.89 4.6 23.4 7.23 4.65 23.6 8.55 Procedure for Part One 8 4.77 23.8 9.38 4.86 Standardization of NaOH solution: 24.1 9.93 10 4.93 KHC3H,04 + NaOH → KNAC3H404 + H2O 24.4 10.32 11 5 24.6 10.55 • The exact molarity of the NaOH solution can be determined from the mass of KHP, its molar mass and the total volume of NaOH at the equivalence point determined from the graph. 12 5.08 13 5.15 25 10.84 14 5.23 26 11.19 15 5.31 27 11.38 16 5.38 28.05 11.5 17 5.47 29 11.58 Questions 18 5.58 30 11.66 19 5.69 31 11.72 1. Find equivalence point the data points. 2. Calculate molarity of the NaOH solution from the result (equivalence point). 3. Find volume and pH at the halfway point. 20 5.82 32 11.77 4. Using pKa, find Ka for KHP.
Using the attached screenshot, determine the equivalence point using the data provided.
This is based upon the acid-base titration lab, information attached.
find equivalence point (volume and pH)
calculate molarity of NaOH solution from result (given mol KHP = mol NaOH and mass provided)
find pKa (using volume and pH at halfway point)
find mean pKa to calculate Ka for KHP
Transcribed Image Text:Data collected
Experimental Procedure
Weigh accurately about 0.51g of KHP and pour
into a clean dry beaker. Add 50mL of distilled
water and swirl until the solid has dissolved.
Vol of
NaOH
pH
added
Using a calibrated pH meter, measure the initial
pH of the solution.
Titrate by adding successive portions of about
1mL of the NaOH solution from the buret.
Record the buret reading and the pH after each
addition. Decrease portions to 0.2mL when the
pH increase by more than 0.3 pH units.
Continue the titration until the pH is about 11.5-
12
21
6.
(mL)
22
6.24
4
22.2
6.31
1
4.05
22.4
6.4
2
4.18
22.6
6.46
3
4.29
22.8
6.58
4
4.41
23
6.71
5
4.51
23.2
6.89
4.6
23.4
7.23
7
4.65
23.6
8.55
Procedure for Part One
8
4.77
23.8
9.38
9
4.86
Standardization of NaOH solution:
24.1
9.93
10
4.93
KHC3H,O4 + NaOH → KNAC3H,04 + H2O
24.4
10.32
11
12
5.08
24.6
10.55
The exact molarity of the NaOH solution can be
determined from the mass of KHP, its molar mass
and the total volume of NaOH at the equivalence
point determined from the graph.
25
10.84
13
5.15
14
5.23
26
11.19
15
5.31
27
11.38
16
5.38
28.05
11.5
17
5.47
29
11.58
Questions
18
5.58
30
11.66
19
5.69
31
11.72
1. Find equivalence point from the data points.
2. Calculate molarity of the NaOH solution from
the result (equivalence point).
3. Find volume and pH at the halfway point.
20
5.82
32
11.77
4. Using pka, find Ka for KHP.
Definition Definition Method of quantitative analysis for determining the concentration of an acid or base by exactly neutralizing it with a standard solution of base or acid having known concentration.
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