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MISSED THIS? Read Section 18.2 (Page), 18.3 (Page): Watch KCV 18.2B, IWES 18.2. 18.3. Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3 and 0.0012 M in H₂CO3. (pKal for H₂CO3 at body temperature is 6.1.) 0.11 mol HCO3 The addition of the acid converts a stoichiometric amount of the conjugate base to the acid. Write an equation showing the neutralization reaction and then set up a table to track the changes: H3O+ (aq) + HCO3(aq) → H₂O(1) + Before addition≈ 0.00 mol 0.11 mol Addition After addition H Part C (0.11 - 2) mol (5.6 x 10-3+2) mol The pH is 7.0 after the addition of HCl. Substitute the quantities of the acid and conjugate base after the addition into the Henderson-Hasselbalch equation and solve the equation for a. Note that the ratio of moles the same as the ratio of concentrations because the volume for both terms is the same. Therefore, 0.00 mol pH = MHCI pKal + log 6.1+ log Rearranging to solve for a gives = 7.6 x 10-3. Thus, the number of moles of HCl added is 7.6 x 10-3 mol. Convert moles to grams using the molar mass of hydrochloric acid as a conversion factor [base] [acid] 0.11-x 5.6 x 10 ³ + x -3. = 7.6 x 10-³ mol HCI x = 0.28 g HCI → H₂CO3(aq) 5.6 x 10-3 mol ? Given the volume from Part B, what mass of NaOH could be neutralized before the pH rose above 7.9? Express your answer to two significant figures. ΠΙ ΑΣΦ 36.46 g HC1 1 mol HCI

MISSED THIS? Read Section 18.2 (Page), 18.3 (Page): Watch KCV 18.2B, IWES 18.2. 18.3. Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3 and 0.0012 M in H₂CO3. (pKal for H₂CO3 at body temperature is 6.1.) 0.11 mol HCO3 The addition of the acid converts a stoichiometric amount of the conjugate base to the acid. Write an equation showing the neutralization reaction and then set up a table to track the changes: H3O+ (aq) + HCO3(aq) → H₂O(1) + Before addition≈ 0.00 mol 0.11 mol Addition After addition H Part C (0.11 - 2) mol (5.6 x 10-3+2) mol The pH is 7.0 after the addition of HCl. Substitute the quantities of the acid and conjugate base after the addition into the Henderson-Hasselbalch equation and solve the equation for a. Note that the ratio of moles the same as the ratio of concentrations because the volume for both terms is the same. Therefore, 0.00 mol pH = MHCI pKal + log 6.1+ log Rearranging to solve for a gives = 7.6 x 10-3. Thus, the number of moles of HCl added is 7.6 x 10-3 mol. Convert moles to grams using the molar mass of hydrochloric acid as a conversion factor [base] [acid] 0.11-x 5.6 x 10 ³ + x -3. = 7.6 x 10-³ mol HCI x = 0.28 g HCI → H₂CO3(aq) 5.6 x 10-3 mol ? Given the volume from Part B, what mass of NaOH could be neutralized before the pH rose above 7.9? Express your answer to two significant figures. ΠΙ ΑΣΦ 36.46 g HC1 1 mol HCI

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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<Chapter 18 Problem Set Exercise 18.55 Enhanced - with Feedback MISSED THIS? Read Section 18.2 (Page), 18.3 (Page); Watch KCV 18.2B, IWES 18.2, 18.3. Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3 and 0.0012 Min H₂CO3. (pKal for H₂CO3 at body temperature is 6.1.) Part A What is the pH of blood plasma? Express your answer to one decimal place. pH = 7.4 Submit Previous Answers Part B MHCI= 0.28 g pH MacBook Pro ✓ Correct To find the pH of blood plasma, determine which component is the acid and which is the base and substitute their concentrations into the Henderson-Hasselbalch equation to calculate the pH. H2CO3 is the acid and HCO3 is the base. Therefore, you can calculate the pH as follows: = = pKal + log 6.1 + log = 7.4 [base] [acid] < 0.024 0.0012 ? 5 of 11 Help Review I Constants I Periodic Table J If the volume of blood in a normal adult is 4.7 L, what mass of HCl could be neutralized by the buffering system in blood before the pH fell below 7.0 (which would result in death)? Express your answer to two significant figures. >
Transcribed Image Text:<Chapter 18 Problem Set Exercise 18.55 Enhanced - with Feedback MISSED THIS? Read Section 18.2 (Page), 18.3 (Page); Watch KCV 18.2B, IWES 18.2, 18.3. Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3 and 0.0012 Min H₂CO3. (pKal for H₂CO3 at body temperature is 6.1.) Part A What is the pH of blood plasma? Express your answer to one decimal place. pH = 7.4 Submit Previous Answers Part B MHCI= 0.28 g pH MacBook Pro ✓ Correct To find the pH of blood plasma, determine which component is the acid and which is the base and substitute their concentrations into the Henderson-Hasselbalch equation to calculate the pH. H2CO3 is the acid and HCO3 is the base. Therefore, you can calculate the pH as follows: = = pKal + log 6.1 + log = 7.4 [base] [acid] < 0.024 0.0012 ? 5 of 11 Help Review I Constants I Periodic Table J If the volume of blood in a normal adult is 4.7 L, what mass of HCl could be neutralized by the buffering system in blood before the pH fell below 7.0 (which would result in death)? Express your answer to two significant figures. >
<Chapter 18 Problem Set Exercise 18.55 Enhanced - with Feedback MISSED THIS? Read Section 18.2 (Page), 18.3 (Page); Watch KCV 18.2B, IWES 18.2, 18.3. Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3 and 0.0012 Min H₂CO3. (pKal for H₂CO3 at body temperature is 6.1.) Part A What is the pH of blood plasma? Express your answer to one decimal place. pH = 7.4 Submit Previous Answers Part B MHCI= 0.28 g pH MacBook Pro ✓ Correct To find the pH of blood plasma, determine which component is the acid and which is the base and substitute their concentrations into the Henderson-Hasselbalch equation to calculate the pH. H2CO3 is the acid and HCO3 is the base. Therefore, you can calculate the pH as follows: = = pKal + log 6.1 + log = 7.4 [base] [acid] < 0.024 0.0012 ? 5 of 11 Help Review I Constants I Periodic Table J If the volume of blood in a normal adult is 4.7 L, what mass of HCl could be neutralized by the buffering system in blood before the pH fell below 7.0 (which would result in death)? Express your answer to two significant figures. >
Transcribed Image Text:<Chapter 18 Problem Set Exercise 18.55 Enhanced - with Feedback MISSED THIS? Read Section 18.2 (Page), 18.3 (Page); Watch KCV 18.2B, IWES 18.2, 18.3. Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3 and 0.0012 Min H₂CO3. (pKal for H₂CO3 at body temperature is 6.1.) Part A What is the pH of blood plasma? Express your answer to one decimal place. pH = 7.4 Submit Previous Answers Part B MHCI= 0.28 g pH MacBook Pro ✓ Correct To find the pH of blood plasma, determine which component is the acid and which is the base and substitute their concentrations into the Henderson-Hasselbalch equation to calculate the pH. H2CO3 is the acid and HCO3 is the base. Therefore, you can calculate the pH as follows: = = pKal + log 6.1 + log = 7.4 [base] [acid] < 0.024 0.0012 ? 5 of 11 Help Review I Constants I Periodic Table J If the volume of blood in a normal adult is 4.7 L, what mass of HCl could be neutralized by the buffering system in blood before the pH fell below 7.0 (which would result in death)? Express your answer to two significant figures. >
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