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8. (4 pts) The biological catalyst carbonic anhydrase converts carbon dioxide to carbonic acid, an essential...
Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid...
Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0010 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. H2CO3(aq) = HCO3- (aq) + H+ (aq) Ka, = 4.3 x 10-7 27 Concentration =
please show full work for understanding purposes:) 5. (4 pts) Calculate the pH of a 0.0025 M aqueous solution of s...
please show full work for understanding purposes:)
5. (4 pts) Calculate the pH of a 0.0025 M aqueous solution of strontium hydroxide, Sr(OH). Sr(OH)2 = Srz + 20H .0025 - x + x + 2x o rood .0025 - Kb = (2x² 4 = 6.5*103 0.0025 ) pH = 6. (6 pts) Calculate the pH of a 0.175 M NH; aqueous solution. K. for NH, is 1.8 x 10. pH = 180 7. (10 pts) Determine the pH of a...
One of the most important buffering systems in the biological realm is the carbonic acid (H2CO3)/carbonate...
One of the most important buffering systems in the biological realm is the carbonic acid (H2CO3)/carbonate ion (HCO3- ) system that maintains the pH of blood plasma to a relatively constant value. In blood at 37°C, the Ka of carbonic acid is 8x10-8. Suppose that the concentrations of the buffer components in the blood plasma are: [HCO3-] = 0.24 M and [H2CO3] = .12 M. Calculate the pH of blood.
21. What are the characteristics of the carbonic acid-bicarbonate buffer system (select all that apply? a...
21. What are the characteristics of the carbonic acid-bicarbonate buffer system (select all that apply? a CO2 is eliminated by the lungs b. Neutralizes HCl acid to yield carbonic acid and salt c. H2CO3 formed by neutralization dissociates into H2O and CO2 d. Shifts H+ in and out of cell in exchange for other cations such as potassium and sodium e. Free basic radicals dissociate into ammonia and OH-, which combines with Ho to form water 22. What are characteristics...
please explain how you got these answers!! and me 17) (5 pts) Calculate the pH of...
please explain how you got these answers!!
and me 17) (5 pts) Calculate the pH of a solution that is 0.15 Min ammonia (NH3) and 0.40 ammonium chloride, given the ionization constant of the base, kb, NH3 = 1.76 X 10 equilibrium reaction: NH3(aq) + H20 (1) 2 NH4(aq) + OH' (aq) A) 5.18 B) 8.82 C) 9.25 D) 9.50 E) 9.63 18) (5 pts) By far the most important buffer for maintaining acid-base balance in the blood is the...
What is the answer to question 15, 16, 17 and 18, and also how did you...
What is the answer to question 15, 16, 17 and 18, and also how
did you calculate it
15) (5 pts) equilibrium information below: Calculate the initial pH of the solution given the following reaction and Ca(OH)2(s) Ca+(aq) +20H-(ag) with Kso 1.3 x 105 A) 12.1 B) 11.8 C) 10.3 D) 8.2 E) None of these choices are correct 2x 13x6 (x) 2. 6.3x106 (x) 2 -0.0036 -10002 0.0072 16) (5 pts) How many moles of sodium acetate (conjugate base)...
Calculations The following calculations are necessary to complete your Report Sheet. Consult the table on page...
Calculations The following calculations are necessary to complete your Report Sheet. Consult the table on page 119 for appropriate K and K, values. Complete these calculations on your Report Sheet for complete credit. I. pH of Strong and Weak Acids 1. Calculate the pH of a 0.10 M hydrochloric acid solution, HCl(aq). 2. Calculate the pH of a solution prepared by diluting 5.00 mL of 0.10 M hydrochloric acid, HCl (aq), in enough water to make a 50.0 mL solution....
(8 pts) Carbon dioxide in the atmosphere dissolves in water to establish an equilibrium that can...
(8 pts) Carbon dioxide in the atmosphere dissolves in water to establish an equilibrium that can increase the acidity of aqueous solutions in the environment. This equilibrium is CO2(g) = CO2 (aq), Kn= 3.1 x 10-2 at 25°C. Kh is called the Henry's law constant, which relates the solubility of the gas CO2 in the aqueous solution, [CO2), to the partial pressure of CO2 over the solution, p(CO2): [CO2] (M)= Kn · p(CO2) (atm) During the preceding decades, the atmospheric...
Which of the following statements is true of weak acids dissolved in water: They...
Which of the following statements is true of weak acids dissolved in water: They are completely ionized in water They are totally unionized in water They are partially ionized in water The dissociation constant is a function of pH QUESTION 13 Which of the following is a hydroxide ion? H3O+ OH- HOOH CH3OH2+ QUESTION 14 The following molecule is an example of which class...
A buffer solution is able to maintain a constant pH when small amounts of acid or...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0010 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. H2CO3(aq) = HCO3- (aq) + H+ (aq) Ka, = 4.3 x 10-7 27 Concentration =
please show full work for understanding purposes:)
5. (4 pts) Calculate the pH of a 0.0025 M aqueous solution of strontium hydroxide, Sr(OH). Sr(OH)2 = Srz + 20H .0025 - x + x + 2x o rood .0025 - Kb = (2x² 4 = 6.5*103 0.0025 ) pH = 6. (6 pts) Calculate the pH of a 0.175 M NH; aqueous solution. K. for NH, is 1.8 x 10. pH = 180 7. (10 pts) Determine the pH of a...
21. What are the characteristics of the carbonic acid-bicarbonate buffer system (select all that apply? a CO2 is eliminated by the lungs b. Neutralizes HCl acid to yield carbonic acid and salt c. H2CO3 formed by neutralization dissociates into H2O and CO2 d. Shifts H+ in and out of cell in exchange for other cations such as potassium and sodium e. Free basic radicals dissociate into ammonia and OH-, which combines with Ho to form water 22. What are characteristics...
please explain how you got these answers!!
and me 17) (5 pts) Calculate the pH of a solution that is 0.15 Min ammonia (NH3) and 0.40 ammonium chloride, given the ionization constant of the base, kb, NH3 = 1.76 X 10 equilibrium reaction: NH3(aq) + H20 (1) 2 NH4(aq) + OH' (aq) A) 5.18 B) 8.82 C) 9.25 D) 9.50 E) 9.63 18) (5 pts) By far the most important buffer for maintaining acid-base balance in the blood is the...
What is the answer to question 15, 16, 17 and 18, and also how
did you calculate it
15) (5 pts) equilibrium information below: Calculate the initial pH of the solution given the following reaction and Ca(OH)2(s) Ca+(aq) +20H-(ag) with Kso 1.3 x 105 A) 12.1 B) 11.8 C) 10.3 D) 8.2 E) None of these choices are correct 2x 13x6 (x) 2. 6.3x106 (x) 2 -0.0036 -10002 0.0072 16) (5 pts) How many moles of sodium acetate (conjugate base)...
Calculations The following calculations are necessary to complete your Report Sheet. Consult the table on page 119 for appropriate K and K, values. Complete these calculations on your Report Sheet for complete credit. I. pH of Strong and Weak Acids 1. Calculate the pH of a 0.10 M hydrochloric acid solution, HCl(aq). 2. Calculate the pH of a solution prepared by diluting 5.00 mL of 0.10 M hydrochloric acid, HCl (aq), in enough water to make a 50.0 mL solution....
(8 pts) Carbon dioxide in the atmosphere dissolves in water to establish an equilibrium that can increase the acidity of aqueous solutions in the environment. This equilibrium is CO2(g) = CO2 (aq), Kn= 3.1 x 10-2 at 25°C. Kh is called the Henry's law constant, which relates the solubility of the gas CO2 in the aqueous solution, [CO2), to the partial pressure of CO2 over the solution, p(CO2): [CO2] (M)= Kn · p(CO2) (atm) During the preceding decades, the atmospheric...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
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