Question
In: Chemistry
A titration experiment is done with 1.37E-2 M NaOH to determine the acid concentration in 0.631...
A titration experiment is done with 1.37E-2 M NaOH to determine the acid concentration in 0.631 L of an unknown acidic solution. It was found that to reach the equivalence point 12.3 mL of strong base was needed. What was the pH of the original acidic solution?
Solutions
Expert Solution
By Molarity equation, M1V1 ( NaOH) = M2V2( unknown acid) 1.37*10^-2 * 12.3ml = M2* 631ml. So, M2= 2.6*10^-3. Concentration of acid= 2.6*10^-3. So, pH= -log[H3O+]= - log[ 2.6*10^-3]= 2.585. l
queen_honey_blossom answered 1 year agoRelated Solutions
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Experiment 2: Using the Secondary Standard to Determine the Concentration of an Acid 1. In an...
Experiment 2: Using the Secondary Standard to Determine the
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sodium hydroxide solution. Record the initial
burette reading. Place the Erlenmeyer
flask on the lower half of the
burette....
A titration is done using 1 M NaOH in the buret and 15mL of 1.8M HCL...
A titration is done using 1 M NaOH in the buret and 15mL of 1.8M
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A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1157 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 14.02 mL of the standard solution. What...
Exercise 1: Determining the Concentration of Acetic Acid Data Table 1. NaOH Titration Volume Initial NaOH...
Exercise 1: Determining the Concentration of Acetic Acid
Data Table 1. NaOH Titration Volume
Initial NaOH Volume (mL)
Final NaOH Volume (mL)
Total volume of NaOH used (mL)
Trial 1
7ml
0
7
Trial 2
7ml
0.4
6.7
Trial 3
7ml
0.6
6.5
Data Table 2. Concentration of
CH3COOH in Vinegar
Average volume of NaOH used (mL)
Concentration
CH3COOH in vinegar
(mol/L)
% CH3COOH
in vinegar
6.7
65mol/L
77%
Questions:
If the manufacturer of the vinegar used in the experiment...
For the titration of 75 mL of 0.10 M acetic acid with 0.10 M NaOH, calculate...
For the titration of 75 mL of 0.10 M acetic acid with 0.10 M
NaOH, calculate the pH. For acetic acid, HC2H3O2, Ka = 1.8 x 10-5.
(a) before the addition of any NaOH solution. (b) after 25 mL of
the base has been added. (c) after half of the HC2H3O2 has been
neutralized. (d) at the equivalence point.
You need to determine the concentration of a sulfuric acid solution by titration with a standard...
You need to determine the concentration of a sulfuric acid
solution by titration with a standard sodium hydroxide solution.
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of the original acid solution and dilute it to 250.0 mL. You then
take a 10.00 mL sample of the dilute acid solution and titrate it
with the standard solution. You need 12.23 mL of the standard
solution to reach the endpoint. What is the concentration of the...
You need to determine the concentration of a sulfuric acid solution by titration with a standard...
You need to determine the concentration of a sulfuric acid
solution by titration with a standard sodium hydroxide solution.
You have a 0.1689 M standard solution. You take a 25.00 mL sample
of the original acid solution and dilute it to 250.0 mL. You then
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solution to reach the endpoint. What is the concentration of the...
nitial data Enter the concentration of NaOH used in the titration. (M) 0.5 Enter the mass...
nitial data
Enter the concentration of NaOH used in the titration. (M)
0.5
Enter the mass of unknown acid you used in grams. (g)
0.75
pH vs Volume Measurements
Table 1. pH readings
Volume (mL)
pH
Initial measurement
0
1.43
Data point 1
0.99
1.23
Data point 2
2
1.41
Data point 3
2.97
1.5
Data point 4
3.99
1.59
Data point 5
4.99
1.69
Data point 6
5.99
1.79
Data point 7
6.98
1.89
Data point 8
7.99
2...
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