QUESTION 1 A buffer is composed of ammonia (NH3) and ammonium chloride (NH4Cl). When base is added to the buffer, which of the following reactions occurs? a. b. c. d. 
 1 points QUESTION 2 Arterial blood gases (ABGs) were drawn on your patient. The following are the some of the results: Respiratory Rate (RR) 10 breaths/min; pH 7.3; and Pressure of CO2 58 torr. The following questions are a basic step-by-step guide in evaluating ABGs. a. If the normal range is 12 - 24 breaths/min , is this patient breathing within a normal range, hyperventilating, or hypoventilating? b. Is this pH level on the acidic or basic side of the normal range? c. Is this pressure of CO2 level within normal range, high, or low? d. With the above findings, what is this patient experiencing? 3 points QUESTION 3 Ascorbic acid (Vitamin C), H2C6H6O6, has a pKa of 4.10. A solution is 0.10 M in ascorbic acid and 0.20 M in sodium ascorbate, NaHC6H6O6. What is the approximate pH of the solution? a. 4.10 b. slightly less than 4.10 c. slightly more than 4.10 d. The solution will have a pH of exactly 7. 
 1 points QUESTION 4 Both the kidneys and the carbon dioxide-carbonic acid cycle help regulate blood pH. True False 1 points QUESTION 5 Buffer Number Acid Component Base Component pKa 1 H2C2O4 1.19 2 C3H5O3 – 3.86 3 HC2H3O2 4.74 4 NH3 NH4 + 9.74 Using the above table, fill in the blank with the appropriate integer (1 ,2, 3,...) indicating the buffer and/or the letter indicating the formula below. A. H3C2O4 + B. HC2O4 – C. C3H4O3 2– D. HC3H5O3 E. C2H3O2 – F. H2C2H3O2 G. C3H5O3 – In Buffer 1, the missing base component is _________________________. 1 points QUESTION 6 Buffer Number Acid Component Base Component pKa 1 H2C2O4 1.19 2 C3H5O3 – 3.86 3 HC2H3O2 4.74 4 NH3 NH4 + 9.74 Using the above table, fill in the blank with the appropriate integer (1 ,2, 3,...) indicating the buffer and/or the letter indicating the formula below. A. H3C2O4 + B. HC2O4 – C. C3H4O3 2– D. HC3H5O3 E. C2H3O2 – F. H2C2H3O2 G. C3H5O3 – In Buffer 2, the missing acid component is_______________________. 1 points QUESTION 7 Buffer Number Acid Component Base Component pKa 1 H2C2O4 1.19 2 C3H5O3 – 3.86 3 HC2H3O2 4.74 4 NH3 NH4 + 9.74 Using the above table, fill in the blank with the appropriate integer (1 ,2, 3,...) indicating the buffer and/or the letter indicating the formula below. A. H3C2O4 + B. HC2O4 – C. C3H4O3 2– D. HC3H5O3 E. C2H3O2 – F. H2C2H3O2 G. C3H5O3 – Buffer ______________________ would be the most effective buffer in basic solutions. 1 points QUESTION 8 Buffer Number Acid Component Base Component pKa 1 H2C2O4 1.19 2 C3H5O3 – 3.86 3 HC2H3O2 4.74 4 NH3 NH4 + 9.74 Using the above table, fill in the blank with the appropriate integer (1 ,2, 3,...) indicating the buffer and/or the letter indicating the formula below. A. H3C2O4 + B. HC2O4 – C. C3H4O3 2– D. HC3H5O3 E. C2H3O2 – F. H2C2H3O2 G. C3H5O3 – In Buffer 2,_________________________ would react with added acid. 1 points QUESTION 9 Buffer ______________________is involved in preventing blood pH fluctuations due to hypo- and hyperventilation. 1 points QUESTION 10 Consider the following three buffer reactions. Buffer 1: protein–H+ and protein Buffer 2: H2CO3 and HCO3 – Buffer 3: H2PO4 – and HPO4 2– Fill in the blank with the appropriate integer (1, 2, or 3) to indicate the buffer system described. Buffer__________________is found in both plasma and red blood cells. 1 points QUESTION 11 Consider the following three buffer reactions. Buffer 1: protein–H+ and protein Buffer 2: H2CO3 and HCO3 – Buffer 3: H2PO4 – and HPO4 2– Fill in the blank with the appropriate integer (1, 2, or 3) to indicate the buffer system described. Buffer______________________ is the most effective regulator for a pH of 7.2. 1 points QUESTION 12 Consider the following three buffer reactions. Buffer 1: protein–H+ and protein Buffer 2: H2CO3 and HCO3 – Buffer 3: H2PO4 – and HPO4 2– Fill in the blank with the appropriate integer (1, 2, or 3) to indicate the buffer system described. Buffer 1 works in conjunction with buffer ____________________to regulate the pH of intracellular fluid. 1 points QUESTION 13 Consider the following three buffer reactions. Buffer 1: protein–H+ and protein Buffer 2: H2CO3 and HCO3 – Buffer 3: H2PO4 – and HPO4 2– Fill in the blank with the appropriate integer (1, 2, or 3) to indicate the buffer system described. Buffer______________________can have a variable pKa value. 1 points QUESTION 14 Consider the image which depicts the reaction between CH3COOH and H2O. Reactants: Products: If the composition of the equilibrium mixture is as represented below CH3COOH is classified as a. strong acid b. weak acid c. strong base d. weak base 
 1 points QUESTION 15 Consider the image which depicts the reaction between CH3COOH and H2O. Reactants: Products: If the composition of the equilibrium mixture is as represented below CH3COOH is classified as a. nonelectrolyte b. strong electrolyte c. weak electrolyte 
 1 points QUESTION 16 Excess phosphorus is excreted by the kidneys. What effect does this have on the pH of blood plasma? a. has no effect b. causes a decrease c. causes an increase 
 1 points QUESTION 17 Which of the following buffers is the predominant buffer in human blood? a.protein–H+/protein b.H2PO4 –/HPO4 2– c.H2CO3/HCO3 – d.All of the above are involved. 
 1 points QUESTION 18 If a patient were in diabetic ketoacidosis (DKA), would you expect their pH level to be high or low? 3 points QUESTION 19 In the reverse reaction, __________________________ion functions as an acid. 1 points QUESTION 20 Joshua has had high blood pressure for a number of years. At Joshua’s last checkup, his doctor orders tests to measure the amount of creatinine in Joshua’s blood and urine. Creatinine is a compound that forms whenever muscles break down creatine, a chemical that helps supply energy for muscle contractions. a.) Does everyone have creatine in their circulating blood? b.) Does everyone secrete creatinine in their urine? Why or why not? 3 points QUESTION 21 Metabolic acidosis resulting from vigorous exercise is associated with increased production of which of the following? a. citric acid b. lactic acid c. formic acid d. phosphoric acid 
 1 points QUESTION 22 The buffer solution in the flask was prepared using one of the substances shown below. citric acid (pKa 3.08) NaH2PO4 (pKa 7.21) NH4Cl (pKa 9.25) Using the pH meter and solution shown in the image below, complete the following statements using one of the terms below. increase decrease remain constant citric acid NaH2PO4 NH4Cl The buffer solution in the beaker could be prepared using__________. 1 points QUESTION 23 The buffer solution in the flask was prepared using one of the substances shown below. citric acid (pKa 3.08) NaH2PO4 (pKa 7.21) NH4Cl (pKa 9.25) Using the pH meter and solution shown in the image below, complete the following statements using one of the terms below. increase decrease remain constant citric acid NaH2PO4 NH4Cl If KOH were added to the buffer solution the pH of the solution would __________. 1 points QUESTION 24 The buffer solution in the flask was prepared using one of the substances shown below. citric acid (pKa 3.08) NaH2PO4 (pKa 7.21) NH4Cl (pKa 9.25) Using the pH meter and solution shown in the image below, complete the following statements using one of the terms below. increase decrease remain constant citric acid NaH2PO4 NH4Cl If HNO3 were added to the buffer solution the pH of the solution would __________. 1 points QUESTION 25 The following reaction represents the self-ionization of ammonia (NH3). NH3(aq) + NH3(aq) NH2 –(aq) + NH4 +(aq) amide ammonium Fill in the blanks with the appropriate terms from those listed below. ammonia ammonium amide In this reaction, the conjugate base of ammonia is the _______________________ ion. 1 points QUESTION 26 Very rapid breathing can lead to a condition know as respiratory acidosis. True False 1 points QUESTION 27 When carbonated beverages are bottled or canned, the partial pressure of carbon dioxide above this liquid is maintained at a high pressure. This procedure cause the pH of the beverage to a. remain constant. b. increase. c. decrease. 
 1 points QUESTION 28 Which of the following is a cause of respiratory acidosis? a. intense exercise b. a poor diet c. hyperventilation d. hypoventilation 
 1 points QUESTION 29 Which of the following is excreted by the kidneys to regulate the effect of excess protein in the diet? a. NH4 + b. HCO3 – c. H3O+ d. H2PO4 – 
 1 points QUESTION 30 Which of the following is true of a buffer prepared with equal concentrations of an acid and its conjugate base? a. pH = 7 b. pH = pKa c. The pH depends on the concentration of the buffer. d. none of the above 
 1 points QUESTION 31 Which of the following solutions can function as a buffer? a. a solution containing HC2H3O2 and NaC2H3O2 b. a solution containing H2CO3 and NaHCO3 c. a solution containing NH3 and NH4Cl d. all of the above 
 1 points QUESTION 32 Which of the following substances can react with both HCl and NaOH?. a. CH3CH2NH2 b. KCl c. Ca(HCO3)2 d. H2C2O4 
 1 points QUESTION 33 Which of the following substances is amphiprotic? a. HCO3 – b. HPO4 3– c. H2PO4 – d. All are amphiprotic. 
 1 points QUESTION 34 Which of the following will determine the pH of a buffer made using acetic acid (HC2H3O2) and sodium acetate (NaC2H3O2)? a. the ratio of the concentrations of C2H3O2 – and HC2H3O2 b. the amount of water present c. the concentration of HC2H3O2 d. the concentration of C2H3O2 –

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