39) One of the buffers that contribute to pH stability in human blood is carbonic acid (H₂CO3). Carbonic acid is a weak acid that, when placed in an aqueous solution, dissociates into a bicarbonate ion (HCO3-) and a hydrogen ion (H+). (See figure.) H₂CO3 Carbonic acid HCO3 Bicarbonate ion H+ Hydrogen ion If the pH of blood drops, one would expect A) a decrease in the concentration of H2CO3 and an increase in the concentration of HCO3- B) the concentration of bicarbonate ions (HCO3-) to increase C) the HCO3- to act as a base and remove excess H+ by the formation of H2CO3 D) the HCO3- to act as an acid and remove excess H+ by the formation of H₂CO3 Answer: C

39) One of the buffers that contribute to pH stability in human blood is carbonic acid (H₂CO3). Carbonic acid is a weak acid that, when placed in an aqueous solution, dissociates into a bicarbonate ion (HCO3-) and a hydrogen ion (H+). (See figure.) H₂CO3 Carbonic acid HCO3 Bicarbonate ion H+ Hydrogen ion If the pH of blood drops, one would expect A) a decrease in the concentration of H2CO3 and an increase in the concentration of HCO3- B) the concentration of bicarbonate ions (HCO3-) to increase C) the HCO3- to act as a base and remove excess H+ by the formation of H2CO3 D) the HCO3- to act as an acid and remove excess H+ by the formation of H₂CO3 Answer: C

Biology (MindTap Course List)

11th Edition

ISBN:9781337392938

Author:Eldra Solomon, Charles Martin, Diana W. Martin, Linda R. Berg

Publisher:Eldra Solomon, Charles Martin, Diana W. Martin, Linda R. Berg

Chapter2: Atoms And Molecules: The Chemical Basis Of Life

Section2.6: Acids, Bases, And Salts

Problem 1C

See similar textbooks

Similar questions

At a pH of 7.40, the carbonic acid ratio is ________. a. 35:1 b. 4:1 c. 20:1 d. 3:1
An aqueous solution contains 0.448 M dimethylamine ((CH3)2NH).How many mL of 0.240 M hydroiodic acid would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 10.500? ______________ml
5. A 60-year old woman was admitted to the hospital with a diagnosis of pneumonia. She had beenon a thiazide diuretic for 6 months previously for treatment of heart failure. Her lab results were:K+ 2.1 mMpH 7.64PCO2 32 mm Hg PO2 75 mm Hg HCO3- 33 mMClassify her acid-base disturbance. Hint: graph it out on the pH-HCO3- diagram
Based on the pH of your drug, if your drug was in a high concentration in the blood, how would it affect the pH of your blood. Would it cause acidosis or alkalosis, and how would you treat this? the drug name is captopril and the pH is 2.65
1. The Henderson-Hasselbalch equation for the blood bicarbonate system is: pH = 6.1 + log b. Calculate the ratio for a blood pH of 8.8. c. Is this patient experiencing acidosis or alkalosis? Why? d. What can the body do to restore normal blood pH levels? Why is the body at a pH outside of the prime buffering zone of the bicarbonate system
For an acid HA, the concentrations of HA and A are 0.075 and 0.025, respectively, at pH 6.0. What is the p K a value for HA?
If 0.752 moles of (NH3OH)Cl is dissolved in 1 L of water what is the pH of the solution?
The pH of human blood is buffered at 7.35 to 7.45. If the [OH-] of the blood sample is 6.3x10-6, calculate its pH value. Is the patient’s pH within the range? Or is experiencing acidosis or alkalosis condition?
Based on the Henderson-Hasselbalch equation (shown below), calculate the pH when half of a solution of acetic acid is dissociated to acetate (the pKa of acetic acid is 4.76). A. 1.00 B. 3.76 C. 4.76 D. 5.76
The weak acid HA is 2% ionized (dissociated) in a 0.20 M solution. (a) What is Ka for this acid? (b) What is the pH of this solution?
1. A woman who had been vomiting for 3 days was taken to the emergency department at University of Chicago by her family. The following blood measurements were obtained: pH = 7.6; PCO2 = 48 mmHg; and HCO3- = 37 mEq/L. A) Name the acid-base disorder you suspect that she has? And explain why you have selected this acid- base disorder. B) Provide a physiologic explanation for Gastrointestinal, Respiratory, and Renal changes that are taking place to either cause or compensate for the acid-base disorder.
Consider a buffer solution that contains 0.55 M NH2CH2CO2H and 0.35 M NH2CH2CO2Na. pKa(NH2CH2CO2H)=9.88. a. Calculate its pH. b. Calculate the change in pH if 0.155 g of solid NaOH is added to 250 mL of this solution. c. If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+ can be neutralized by 250 mL of the initial buffer.