Type of acid in unknown: H3A Molar mass for unknown acid: 192.140 g/mol Balanced chemical equation for neutralization of acid with NaOH X | X' |- EEE fel e Ilf Normal BIIIU Is Table view List view Table 6. Calculations for percent by mass Sample 1 Sample 2 Sample 3 1] Mass sample (g) 26.334 29.157 27.111 [2] Burette reading of NaOH, initial (mL) 3.21 1.48 1.22 [3] Burette reading of NaOH, final (mL) 22.77 23.42 20.99 14] Volume of NaOH, dispensed (mL) [5] Molar concentration of NaOH (part A) [6] Mass of acid in sample (g) 7 Percentage by mass in sample (%) [8] Average percentage by mass of acid
Type of acid in unknown: H3A Molar mass for unknown acid: 192.140 g/mol Balanced chemical equation for neutralization of acid with NaOH X | X' |- EEE fel e Ilf Normal BIIIU Is Table view List view Table 6. Calculations for percent by mass Sample 1 Sample 2 Sample 3 1] Mass sample (g) 26.334 29.157 27.111 [2] Burette reading of NaOH, initial (mL) 3.21 1.48 1.22 [3] Burette reading of NaOH, final (mL) 22.77 23.42 20.99 14] Volume of NaOH, dispensed (mL) [5] Molar concentration of NaOH (part A) [6] Mass of acid in sample (g) 7 Percentage by mass in sample (%) [8] Average percentage by mass of acid
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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please can someone please help me with this
![Ooldtion
Table 1. Measurements for standardization of NaOH
Trial 1
Trial 2
Trial 3
1] Tared mass of KHC3H4O4 (9)
0.374
0.325
0.357
12] Burette reading of NaOH, initial (mL)
4.59
3.61
4.03
[3] Burette reading of NaOH, final (mL)
22.03
18.77
21.17
Part B. Molar Concentration of an Acid Solution
Enter the number corresponding to the type of acid you have
1. HA
3
2. H2A
3. H3A
Enter the unknown number.
21
Table 2. Measurements for titration of unknown acid
Trial 1
Trial 2
Trial 3
[1] Volume of acid (mL)
25.0
25.0
25.0
[2] Burette reading of NaOH, initial (mL)
2.13
2.48
3.68
[3] Burette reading of NaOH, final (mL)
24.10
24.52
25.56
Part C. Percentage by Mass of an Unknown Solid
Enter the number corresponding to the type of acid you have
1. HA
3
2. H2A
3. H3A
Enter the unknown number.
30
Molar mass of the unknown acid
192.14
Table 3. Measurements for titriation of solid
Trial 1
Trial 2
Trial 3
[1] Mass of sample (g)
26.334
29.157
27.111
[2] Burette reading of NaOH, initial (mL)
3.21
1.48
1.22
[3] Burette reading of NaOH, final (mL)
22.77
23.42
20.99](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F48bba008-5eee-4157-b489-6f90113c3fbd%2Fbb752b96-3f02-42af-8e14-69afa62cc8d6%2Fv7xlnz_processed.png&w=3840&q=75)
Transcribed Image Text:Ooldtion
Table 1. Measurements for standardization of NaOH
Trial 1
Trial 2
Trial 3
1] Tared mass of KHC3H4O4 (9)
0.374
0.325
0.357
12] Burette reading of NaOH, initial (mL)
4.59
3.61
4.03
[3] Burette reading of NaOH, final (mL)
22.03
18.77
21.17
Part B. Molar Concentration of an Acid Solution
Enter the number corresponding to the type of acid you have
1. HA
3
2. H2A
3. H3A
Enter the unknown number.
21
Table 2. Measurements for titration of unknown acid
Trial 1
Trial 2
Trial 3
[1] Volume of acid (mL)
25.0
25.0
25.0
[2] Burette reading of NaOH, initial (mL)
2.13
2.48
3.68
[3] Burette reading of NaOH, final (mL)
24.10
24.52
25.56
Part C. Percentage by Mass of an Unknown Solid
Enter the number corresponding to the type of acid you have
1. HA
3
2. H2A
3. H3A
Enter the unknown number.
30
Molar mass of the unknown acid
192.14
Table 3. Measurements for titriation of solid
Trial 1
Trial 2
Trial 3
[1] Mass of sample (g)
26.334
29.157
27.111
[2] Burette reading of NaOH, initial (mL)
3.21
1.48
1.22
[3] Burette reading of NaOH, final (mL)
22.77
23.42
20.99
![Type of acid in unknown: H3A
Molar mass for unknown acid: 192.140 g/mol
Balanced chemical equation for neutralization of acid with NaOH
: BIIIU
X X' |- EEI= fel
Normal
Is
Table view
List view
Table 6. Calculations for percent by mass
Sample 1
Sample 2
Sample 3
1] Mass sample (9)
26.334
29.157
27.111
[2] Burette reading of NaOH,
initial (mL)
3.21
1.48
1.22
[3] Burette reading of N2OH,
final (mL)
22.77
23.42
20.99
14] Volume of NaOH,
dispensed (mL)
[5] Molar concentration of
NaoH (рart A)
[6] Mass of acid in sample
(9)
7 Percentage by mass in
sample (%)
[8] Average percentage by mass of acid](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F48bba008-5eee-4157-b489-6f90113c3fbd%2Fbb752b96-3f02-42af-8e14-69afa62cc8d6%2Fga265h9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Type of acid in unknown: H3A
Molar mass for unknown acid: 192.140 g/mol
Balanced chemical equation for neutralization of acid with NaOH
: BIIIU
X X' |- EEI= fel
Normal
Is
Table view
List view
Table 6. Calculations for percent by mass
Sample 1
Sample 2
Sample 3
1] Mass sample (9)
26.334
29.157
27.111
[2] Burette reading of NaOH,
initial (mL)
3.21
1.48
1.22
[3] Burette reading of N2OH,
final (mL)
22.77
23.42
20.99
14] Volume of NaOH,
dispensed (mL)
[5] Molar concentration of
NaoH (рart A)
[6] Mass of acid in sample
(9)
7 Percentage by mass in
sample (%)
[8] Average percentage by mass of acid
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