a.
To determine:
The direction of equilibrium during high concentrations of oxygen in binding of hemoglobin and oxygen.
Introduction:
In a reversible reaction, the difference is energy is very less between reactants and products. Products formed from the collision of reactants can again dissociate to form reactants, that is, reaction is favorable in both the directions. The reactions of such type are said to be in equilibrium when the rate of forward reaction becomes equal to the rate of backward reaction.
b.
To determine:
The direction of equilibrium when the concentration of hydrogen ions is high in binding of hemoglobin and oxygen.
Introduction:
In a reversible reaction, the difference is energy is very less between reactants and products. Products formed from the collision of reactants can again dissociate to form reactants, that is, reaction is favorable in both the directions. The reactions of such type are said to be in equilibrium when the rate of forward reaction becomes equal to the rate of backward reaction.
c.
To determine:
The direction of equilibrium when concentration of carbon dioxide is built up in the bloodstream.
Introduction:
In a reversible reaction, the difference is energy is very less between reactants and products. Products formed from the collision of reactants can again dissociate to form reactants, that is, reaction is favorable in both the directions. The reactions of such type are said to be in equilibrium when the rate of forward reaction becomes equal to the rate of backward reaction.
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
General, Organic, and Biological Chemistry (3rd Edition)
- Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.arrow_forwardWhat are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 105)? What is the pH of the solution?arrow_forwardSome of the substances commonly used in stomach antacids are MgO, Mg(OH)2, and Al(OH)3. a. Write a balanced equation for the neutralization of hydrochloric acid by each of these substances. b. Which of these substances will neutralize the greatest amount of 0.10 M HCl per gram?arrow_forward
- What is An for the equilibrium system: Na2CO3 (s) + CO2 (g) + H2O (g) =2 NaHCO3 (s)? O 2 О 1 O -2 O 1arrow_forwardWhy is only increasing the pH of the ocean not enough to restore the ocean’s equilibrium? How does decreasing the pH decrease carbonate (CO₃²⁻) concentration? Some calcifiers can use bicarbonate (HCO₃⁻) to make their shells. How will they be affected by the decrease in pH?arrow_forwardHydrazoic acid, HN3, has an acid dissociation constant of 2.5 x 10-5. Calculate the equilibrium concentrations of all substances if the initial concentration of HN3 is 0.0750 M. Determine the pH of the solution. Would a 0.0750 M solution of HBr have a higher or lower pH than the 0.0750 M HN3 solution? Explain why.arrow_forward
- Tooth enamel, Ca5(PO4)3OH, establishes the following equilibrium: Ca5(PO4)3OH(s) <=> 5Ca2+(aq) + 3PO 3–(aq) + OH–(aq) 4 Which of the following, when added to the above equilibrium system, will cause the position of equilibrium to shift to the right? A.H+(aq) B. OH–(aq) C. Ca2+(aq) D. Ca5(PO4)3OH(s)arrow_forwardH2AO4 is a weak acid. What is [AO42 in a 0.30 M H2AO4 solution? [Ka1 = 6.2 x 10-; Ka2 = 5.2 x 10-10 OA21 x 10-5 M OB 5.2 x 10-7 M OC0.60 M OD 6.2 x 10-7 M OE 0.30 M OF 6.2 x 10-10 M OG5.2 x 10-10 Marrow_forward2. Determine the acid type for HBr. O Brønsted-Lowry Ahrrenius not an acid Lewisarrow_forward
- Which of the following is the structure of oxalic acid? HO. HO. HO. HO. HO, HO. %3D IV B) || C) II O A)I O D) IVarrow_forwardA 0.0560-g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H*, CH3COO¯, and CH3COOH at equilibrium. (K, for acetic acid = 1.8 × 10.)arrow_forward3. What is the pH of a 0.0075 mol L·' HCl solution? What is [OH]in this solution? 4. Each of the following salts were dissolved in water to give a 0.10 mol.L·' solution. Rank the solutions from lowest to highest pH. Their respective pKb values are indicated in brackets. Na2S (-5), Na3PO4 (1.68), NaF (10.86), NaCH3CO0 (9.26), AIC13arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning