Formät Tools Add-ons Normal text I U A E - E - E E X Arial 11 GD 2 3 6. solution Post Lab questions: 1. What is the normal pH range of blood? Is blood acidic, basic, or neutral? Write the formulas of the buffer components that are present in blood to maintain its pH. Solution is acidic, basic, or neutral? [H3O+ ] [OH-] PH 4.4x10^-8 4.56 x 10-2 7.35 basic 3.5 x 10-3 2.8x10^-7 7.45 basic 1.58x10^-8 6.3x10^-7 7.8 basic 1.0x10^-7 1.0x10^-7 7.0 neutral 3.0x10^-4 3.33 x 10-11 3.52 acidic 3. Calculate the molarity of the HCI solution if 0.074 mol of HCI is dissolved in water to make 2000 mL of solution. Also calculate the pH of this solution. Hint: In case of strong acids the [H30 + ] is the same as the molarity of the acid. Vol 2000ml=2.0001 Moles of HCI dissolved=0.074 mol. mol/vol Hence concentration of H3O+(H+)(H3O+)= Mol 0.037 Hence ph=-log (H3O+)=-log(0.037)+1-43 4. State one advantage and one disadvantage of the red cabbage indicator and of the pH meter used in this experiment +
Formät Tools Add-ons Normal text I U A E - E - E E X Arial 11 GD 2 3 6. solution Post Lab questions: 1. What is the normal pH range of blood? Is blood acidic, basic, or neutral? Write the formulas of the buffer components that are present in blood to maintain its pH. Solution is acidic, basic, or neutral? [H3O+ ] [OH-] PH 4.4x10^-8 4.56 x 10-2 7.35 basic 3.5 x 10-3 2.8x10^-7 7.45 basic 1.58x10^-8 6.3x10^-7 7.8 basic 1.0x10^-7 1.0x10^-7 7.0 neutral 3.0x10^-4 3.33 x 10-11 3.52 acidic 3. Calculate the molarity of the HCI solution if 0.074 mol of HCI is dissolved in water to make 2000 mL of solution. Also calculate the pH of this solution. Hint: In case of strong acids the [H30 + ] is the same as the molarity of the acid. Vol 2000ml=2.0001 Moles of HCI dissolved=0.074 mol. mol/vol Hence concentration of H3O+(H+)(H3O+)= Mol 0.037 Hence ph=-log (H3O+)=-log(0.037)+1-43 4. State one advantage and one disadvantage of the red cabbage indicator and of the pH meter used in this experiment +
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter16: Acids And Bases
Section: Chapter Questions
Problem 61QAP: . Which component of a buffered solution is capable of combining with an added strong acid? Using...
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Arial
BIUA
E E - E - E E
11
3
4
solution
Post Lab questions: 1. What is the normal pH range of blood? Is blood acidic, basic, or
neutral? Write the formulas of the buffer components that are present in blood to
maintain its pH.
[H3O+ ]
Solution is acidic,
basic, or neutral?
[OH-]
PH
4.4x10^-8
4.56 x 10-2
7.35
basic
3.5 x 10-3
2.8x10^-7
7.45
basic
1.58x10^-8
6.3x10^-7
7.8
basic
1.0x10^-7
1.0x10^-7
7.0
neutral
3.0x10^-4
3.33 x 10-11
3.52
acidic
3. Calculate the molarity of the HCI solution if 0.074 mol of HCI is dissolved in water to
make 2000 mL of solution. Also calculate the pH of this solution. Hint: In case of strong
acids the [H30 + ] is the same as the molarity of the acid.
Vol 2000ml=2.0001
Moles of HCI dissolved=0.074 mol.
mol/vol
Hence concentration of H3O+(H+)(H3O+)= Mol 0.037
Hence ph=-log (H3O+)=-log(0.037)+143
4. State one advantage and one disadvantage of the red cabbage indicator and of the pH
meter used in this experiment
+
étv
4
MacBook Air](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F379c46a6-3d97-4265-8b53-73306fc6c85c%2Fa2b6c6b2-ab7c-4309-b2b0-c534609b7c4d%2F2qgevak_processed.jpeg&w=3840&q=75)
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Last edit was seconds ago
100%
Normal text
Arial
BIUA
E E - E - E E
11
3
4
solution
Post Lab questions: 1. What is the normal pH range of blood? Is blood acidic, basic, or
neutral? Write the formulas of the buffer components that are present in blood to
maintain its pH.
[H3O+ ]
Solution is acidic,
basic, or neutral?
[OH-]
PH
4.4x10^-8
4.56 x 10-2
7.35
basic
3.5 x 10-3
2.8x10^-7
7.45
basic
1.58x10^-8
6.3x10^-7
7.8
basic
1.0x10^-7
1.0x10^-7
7.0
neutral
3.0x10^-4
3.33 x 10-11
3.52
acidic
3. Calculate the molarity of the HCI solution if 0.074 mol of HCI is dissolved in water to
make 2000 mL of solution. Also calculate the pH of this solution. Hint: In case of strong
acids the [H30 + ] is the same as the molarity of the acid.
Vol 2000ml=2.0001
Moles of HCI dissolved=0.074 mol.
mol/vol
Hence concentration of H3O+(H+)(H3O+)= Mol 0.037
Hence ph=-log (H3O+)=-log(0.037)+143
4. State one advantage and one disadvantage of the red cabbage indicator and of the pH
meter used in this experiment
+
étv
4
MacBook Air
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