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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 +

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 77QAP: Two students were asked to determine the Kb of an unknown base. They were given a bottle with a...
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w Insert Format Tools Add-ons Help 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
Transcribed Image Text:w Insert Format Tools Add-ons Help 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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