Week 4 Day 1

Question 1

Le chatelier’s principle

Answer 1

can be used to predict the affect of change in conditions on a chemical equilibrium

K_eq= [C_eq]^c * [D_eq]^d/[A_eq]^a * [B_eq]^b

Question 2

Dissociation of water

Answer 2

[H⁺]=[OH^-] = 1.0 x 10^-7

Question 3

acid

Answer 3

molecule that donates a H⁺

Question 4

base

Answer 4

molecule that accepts an H⁺

Question 5

conjugate base

Answer 5

what is left after an acid has donated a proton

Question 6

conjugate acid

Answer 6

formed by a base accepting a hydrogen

Question 7

Henderson-Hasselbalch equation

Answer 7

pH = pK_a + log([A^-] / [HA])

Used to calculate the pH of a buffer and states the pH of a buffer is equal to the pK_a of the weak acid plus the log of the ratio of the concentration of the conjugate base [A^-], divided by the concentration of the acid [HA]

Question 8

buffer

Answer 8

a solution that can resist change in pH upon addition of acidic or basic components

Usually consists of a weak acid and its conjugate base

Question 9

Normal values:

pH

CO₂

HCO₃

Answer 9

pH: 7.4 (7.35-7.45)

CO₂: 40 mmhg (35-45)

HCO₃: 24 mM (20-28)

Question 10

acute respiratory acidosis

Answer 10

Increased CO₂

decreased pH

increased HCO₃^-

normal BE

Question 11

chronic respiratory acidosis

Answer 11

increased CO₂

close to normal pH

very increased HCO₃^-

> +2 BE

Question 12

acute metabolic acidosis

Answer 12

decreased CO₂

decreased HCO₃^- or increased H⁺

decreased pH

negative <-2 BE

Question 13

Chronic metabolic acidosis

Answer 13

decreased CO₂

decreased HCO₃^-

about normal pH

negative <-2 BE

Question 14

Acute respiratory alkalosis

Answer 14

decreased CO₂

decreased HCO₃^-

increased pH

normal BE

Question 15

chronic respiratory alkalosis

Answer 15

decreased CO₂

very decreased HCO₃^-

about normal pH

negative <-2 BE

Question 16

acute metabolic alkalosis

Answer 16

increased CO₂

increased HCO₃^-

increased pH

positive >+2 BE

Question 17

chronic metabolic alkalosis

Answer 17

increased CO₂

increased HCO₃^-

about normal pH

positive >+2 BE

Question 18

anion gap

Answer 18

Na⁺ - (Cl^- + HCO₃-)

high anion gap = addition of acid

normal anion gap = loss of base

Question 19

HCl

Answer 19

Hydrochloric acid

strong acid

Question 20

HBR

Answer 20

hydrobromic acid

Question 21

HI

Answer 21

hydroiotic acid

Question 22

HNO₃

Answer 22

nitric acid

Question 23

HClO₃

Answer 23

chloric acid

Question 24

HClO₄

Answer 24

perchloric acid

Question 25

H₂SO₄

Answer 25

sulfuric acid

Question 26

LiOH

Answer 26

lithium hydroxide

Question 27

NaOh

Answer 27

sodium hydroxide

Question 28

KOH

Answer 28

potassium hydroxide

Question 29

RbOh

Answer 29

rubidium hydroxide

Question 30

CsOH

Answer 30

cesium hydroxide

Question 31

Ca(OH)₂

Answer 31

calcium hydroxide

Question 32

Sr(OH)₂

Answer 32

strontium hydroxide

Question 33

Ba(OH)₂

Answer 33

barium hydroxide