CHEM 282 Lecture Notes - Lecture 5: Bleeding, Extracellular Fluid, Carbonic Anhydrase

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17 Apr 2021

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The concept of acid base balance refers to the regulation of hydrogen ions in the body fluids. Bases- substances that bind free h+ in solution: the stronger the base, the easier it can bind h, when a strong base is added to solution, it decreases the concentration of free h+ ph designation. Ph= 7 is considered to be neutral (water) solutions with a ph< 7 are acidic as they have more free h+ and solutions with ph> 7 are basic because they have less free h+ If the blood is acidotic, then more h+ then k+ will be secreted. Under normal conditions there is an almost constant production or release of h+ into the body fluids and majority of this comes from metabolic activities. A chemical buffer is a mixture of two chemicals that interact in such a way to resist ph changes when either an acid or a base is added to the system.

Related Questions

Strong Acids and Bases: Since strong acids/bases completely dissociate in water, the concentration of the hydrogen ions/hydroxide ions is equal to the concentration of the acid/base.

1. What is the pH of a 0.001 M HCl solution?

2. What is the pH of a 10-4M NaOH solution?

3. What is the pH of a 0.0075 M HCl solution?

4. What is the hydrogen ion concentration in a solution with a pH of 3.75?

5. What is the hydroxide ion concentration in a solution with pH 10.4?

1.Write the equation that represents the reaction of pyruvic acid in water. (You will find the structure of pyruvic acid in the Common Acids in Biochemistry and Medicinetable. Omit states-of-matter from your answer.)

2.Label the conjugate acid-base pairs. (Omit states-of-matter from your answer. Separate substances in a list with a comma.)
Conjugate acid-base pair that includes pyruvic acid:

3.Conjugate acid-base pair that does not include pyruvic acid:

QUESTION 1

Which of the following substances is most acidic?

		Cowâs milk - pH 6.6
		Apple juice - pH 3.0
		Tomato juice - pH 4.5
		Distilled water - pH 7.0

2 points

QUESTION 2

A buffer is a substance that converts:

Alkaline solutions to neutral solutions.

Acidic solutions to alkaline solutions.

Strong bases or acids to weak bases or acids.

Acidic solutions to neutral solutions.

QUESTION 3

How does a solution of pH 7 compare to a solution of pH 10?

		pH 7 has more OH^- ions
		pH 7 is more basic
		pH 7 has a higher pH
		pH 7 has more H⁺ ions

2 points

QUESTION 4

According to the Arrhenius Theory of acids and bases, a base is:

A substance that decrease the amount of hydroxide ions present.

A substance that increases the amount of hydroxide ions present when it is dissolved in water.

A substance that increase the amount of hydrogen ions present.

A substance that increases the amount of hydrogen ions present when it is dissolved in water.

QUESTION 5

Which of the following are true regarding acid-base titrations?

		They are used to determine the concentration of an unknown acid or base.
		The acid or the base must be a standard solution with a known concentration
		The standard solution is titrated into the chemical with the unknown concentration.
		All of the above are true regarding acid-base titrations.

2 points

QUESTION 6

Which of the following is not an example of a neutralization reaction?

HCl + NaOH NaCl +H₂O

2 NaOH + H₂CO₃ Na₂CO₃ +2 H₂O

H₂SO₄ + 2 NH₄OH (NH₄)₂SO₄ + 2 H₂O

2 AgNO₃ + Zn 2Ag +Zn(NO₃)₂

QUESTION 7

Which acid base theory defines an acid as a proton donor and a base as a proton acceptor?

		Arrhenius Theory
		Bronsted-Lowery Theory
		Conjugate Pairs Theory
		Lewis Theory

2 points

QUESTION 8

The Arrhenius Theory states that acid-base reactions create a solution composed of a water and a salt. This is because mixing an acidic and basic solution together yields:

A neutral solution

A solution with a pH at or near 7

Both A and B are correct

QUESTION 9

Which of the following correctly defines a standard solution?

		A solution which always has the same molecular geometry.
		A solution in which the concentration is precisely known.
		A solution in which the volume is precisely known.
		A solution which always has different levels of solutes and solvents.

2 points

QUESTION 10

Acids naturally present in food are generally safe to eat because they are usually:

		Concentrated
		Dilute
		Weak
		Strong

None of the above are correct

CHEM 282 Lecture Notes - Lecture 5: Bleeding, Extracellular Fluid, Carbonic Anhydrase

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