Chapter 2 Lecture 3 - Properties of Water, Acids and Bases, pH, Measures of Concentration

Question 1

What percentage of the body is comprised of water?

Answer 1

50-75%

Question 2

What percentage of the blood is comprised of water?

Answer 2

92%

Question 3

Why is water so important?

Answer 3

Atoms are joined by polar-covalent bonds, molecules are v shape

Question 4

Solvent

Answer 4

Dissolves a solute

Question 5

Solute

Answer 5

Dissolved in the solvent

Question 6

Is water a solvent or a solute

Answer 6

solvent

Question 7

Why can substances dissolve in water

Answer 7

It is polar

Question 8

How does water play a major role in chemical reactions

Answer 8

Ionizes acids and salts, as well as itself. These ions can then be used in other reactions

Question 9

Acid

Answer 9

Proton donor, any substance that releases H+ ions

Question 10

Base

Answer 10

Proton acceptor or any substance that binds to or accepts H+ or releases OH-. DOES NOT HAVE TO DONATE OH-

Question 11

Buffer

Answer 11

Solution of acid base pairs in which acid and base components occur in similar concentrations

Question 12

How to calculate pH

Answer 12

ph=-log[H+]

Question 13

What is the molarity of H+ in water

Answer 13

1.0x10^-7

Question 14

What is the difference in H+ concentration between any two values on the pH scale

Answer 14

10x

Question 15

What is the normal pH of human blood

Answer 15

7.4

Question 16

Function of buffers

Answer 16

resist changes in pH, convert strong (completely dissociated) acids or bases to weak, slightly dissociated ones

Question 17

Carbonic acid - Bicarbonate system

Answer 17

H2O+CO2 Carbonic Acid (H2CO3) Biarbonate ion (HCO3-) + H+

Question 18

Weight per volume

Answer 18

Weight of solute in given volume of solution

Question 19

Ex. of weight per volume

Answer 19

serum cholesterol (200mg/dL)

Question 20

Percentage (concentration)

Answer 20

weight of solute as % of volume of a solution (volume/volume)

Question 21

Molarity

Answer 21

of moles of a chemical per liter of a solution

Question 22

Milliquivalents per liter

Answer 22

used to express electrolyte concentration. Takes into account mM concentrations as well as charge