Concept explainers
(a)
Interpretation:
The cause of respiratory acidosis should be explained.
Concept Introduction:
The normal blood pH ranges from 7.35 and 7.45, if the pH of blood is less than the limited value; acidosis condition occurs that leads to depression.
Mild acidosis can cause dizziness, fainting and disorientation but severe acidosis can lead to coma. This can also cause death if the pH value is very far away from the normal range. There are two types of acidosis namely, respiratory acidosis and the other is
(b)
Interpretation:
The cause of metabolic acidosis should be explained.
Concept Introduction:
The normal blood pH ranges from 7.35 and 7.45, if the pH of blood is less than the limited value; acidosis condition occurs that leads to depression.
Mild acidosis can cause dizziness, fainting and disorientation but severe acidosis can lead to coma. This can also cause death if the pH value is very far away from the normal range. There are two types of acidosis namely, respiratory acidosis and the other is metabolic acidosis.
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Chapter 8 Solutions
Introduction to General, Organic and Biochemistry
- Use the equation below to answer the following questions.CO2 + H2O ⇄ H2CO3 ⇄ H+ + HCO3 Tom is holding his breath underwater. What happens to the carbon dioxide content of his blood, and how does this change affect his blood acidity? Notice that the arrows go in both directions, indicating that the reaction can proceed in both directions. If Tom consumes a large amount of lemon juice, increasing the H+ concentration in his blood, what do you think will happen to the amount of CO2 in his blood? Only consider the equation above in your answer.arrow_forwardIdentify the Lewis acid and Lewis base in each equation:arrow_forwardDraw the structures of the conjugate bases of the following acids: (a) COO I CH || HC (c) I COOH COO™ I H-C-H NH (b) (d) COOH H-C-H NH COO™ H-C-CH₂-COOH NHarrow_forward
- Draw the structures of the conjugate bases of the following acids:arrow_forwardCalculate the equilibrium constant for the acid–base reaction between the reactants in each of the following pairs: (a) HCl + H2O (b) CH3COOH + H2O (c) CH3NH2 + H2O (d) CH3N+H3 + H2Oarrow_forwardConsider the following equilibrium between pentanoic acid and its conjugate base: | CH3CH,CH,CH2C0- H20 + H30+ CH;CH2CH,CH,C-OH Will lowering the pH shift the equilibrium to the right or to the left?arrow_forward
- (a) Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) calculate the Kb values for the CHCOO- and ClO- .arrow_forwardWrite a net ionic equation to show that caffeine, C3H10N402, behaves as a Bronsted-Lowry base in water. BL base BL acid BL acid BL base + H2O +arrow_forwardCan you please answer Question 2 a,b please thanksarrow_forward
- 6-82 (Chemical Connections 6C) A solution contains 54 mEq/L ofCI- and 12 mEq/L of HCO3-. If Na+ is the only cation present in the solution, what is the Na+ concentration in milliequivalents per liter?arrow_forward5. Given the general equation illustrating the reaction of the acid HA in water, HA(aq)+H2O(l)H3O+(aq)+A(aq)explain why water is considered a base in the Brønsted-Lowry model.arrow_forwardHow do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.arrow_forward
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