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BIOCHEM LAB > EXPT 1: pH and BUFFER SOLUTIONS > Flashcards

EXPT 1: pH and BUFFER SOLUTIONS Flashcards

1
Q

is a measure of the concentration of
hydrogen ions (H+
) in a solution.

A

PH

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2
Q

: a scale used to measure the
concentration of H+
ions in a solution, ranging
from 0 (strongly acidic) to 14 (strongly basic).

A

pH scale

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3
Q

pH is calculated using the formula

A

pH = -log[H+]

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4
Q

is the concentration of hydrogen
ions in moles per liter (M).

A

[H+] Acid

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5
Q

are mixtures of a weak acid
and its conjugate base, or a weak base and its
conjugate acid, that resist changes in pH

A

Buffer solutions

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6
Q

substances that donate H+
ions (protons) when dissolved in water.

A

Acid

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7
Q

a pair of
substances that differ by one proton.

A

Acid/conjugate-base pair
Base/conjugate-acid pair

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7
Q

substances that accept H+
ions (protons) when dissolved in water.

A

Bases

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8
Q

substances that increase the
concentration of H+
ions in a solution.

A

Acids

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8
Q

substances that increase the
concentration of OH ions in a solution.

A

Bases

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8
Q

completely dissociate in water,
releasing all their H+
ions.

A

Strong Acids

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9
Q

completely dissociate in
water, releasing all their OH ions.

A

Strong Base

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9
Q

partially dissociate in water,
releasing some of their H+
ions.

A

Weak Acids

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10
Q

partially dissociate in water,
releasing some of their OH ions.

A

Weak Base

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10
Q

substances that change color
in response to changes in pH.

A

PH indicators

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11
Q

a qualitative method that uses
a pH indicator to determine if a solution is
acidic or basic.

A

Litmus paper

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11
Q

a quantitative method that uses a
device to measure the pH of a solution

A

PH meters

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12
Q

a quantitative method that uses a
pH indicator to measure the pH of a solution.

A

PH paper

13
Q

is a mixture of a weak acid and its conjugate base, or a weak base and its
conjugate acid, that resists changes in pH.

A

Buffers

14
Q

consists of
carbonic acid (H2CO3) and its conjugate base, bicarbonate (HCO3-)

A

Carbonate buffer system

15
Q

Function of the carbonate buffer system

A

regulates the pH of the blood by neutralizing excess H+ ions.

16
Q

contain amino acids with acidic or basic side chains can act as buffers.

A

Proteins

16
Q

consists of dihydrogen phosphate (H2PO4-) and its conjugate base, hydrogen phosphate, HPO4 2-

A

Phosphate buffer system

17
Q

have a carboxyl group (-COOH),

A

Amino Acids

17
Q

Function of Phosphate buffer system

A

regulates the pH of the cytosol of cells.

18
Q

is deprotonated
when it reacts with OH to produce its conjugate base and water, decreasing the pH

A

The carboxyl group

19
Q

is protonated when it reacts with H3O+ to produce its conjugate base and water, increasing the pH.

A

The amino group

20
Q

is a mathematical equation that relates the pH of
a buffer solution to the concentrations of the
weak acid and its conjugate base.

A

The Henderson-Hasselbalch equation

21
Q

a measure of the concentration of
hydroxide ions (OH-) in a solution

A

pOH

22
Q

pH and pOH are related by the equation:

A

pH + pOH = 14

23
Q

acid dissociation constant

A

pKa

24
Q

concentration of the conjugate base

A

[A-]

25
Q

concentration of the weak acid

A

[HA]

26
Q

concentration of hydrogen ions in moles per liter (M)

A

[H+]

27
Q

is crucial for proper
bodily functions, as even small changes can
lead to severe consequences.

A

Regulation of Blood pH

28
Q

play a vital role in regulating blood pH by controlling the amount of carbon
dioxide (CO2) in the blood.

A

The lungs

29
Q

the lungs decrease the rate and volume of
breathing to retain more CO2 in the body. This helps to increase the acidity of the blood.

A

Decreasing ventilation

29
Q

the lungs
increase the rate and volume of breathing to
eliminate more CO2 from the body .This helps to reduce the acidity of the blood.

A

Increasing ventilation

30
Q

an organ that also play a crucial role in
regulating blood pH by controlling the amount
of acid and bicarbonate in the blood.

A

The kidneys

31
Q

The kidneys also reclaim
bicarbonate ions from the glomerular filtrate, which helps to increase the alkalinity
of the blood.

A

Reclaiming HCO3

32
Q

The kidneys excrete excess
hydrogen ions (H+) from the blood, which helps to reduce the acidity of the blood.

A

Excreting acid

33
Q

plays a crucial role in maintaining acid-base balance
in the bloodstream

A

The carbonic acid buffer system

34
Q

act as a third type of blood buffer, containing both proton acceptors and
donors.

A

Protein buffer system

35
Q

Understanding these buffer systems is essential in diagnosing and managing various
acid-base disorders

A

Clinical correlations

BIOCHEM LAB (6 decks)

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