Top2-Ch2-P54-58Reverse

Question 23

Answer 23

Picture of hydronium in action

Question 24

equilibrium of a reaction

See formula below defined in terms of the [reactants] and [products] at equilibrium:

Remember: The equilibrium constant is fixed for any given chemical reaction at a specific temperature.

Answer 24

K_eq gives the position of ?

Give the formula

Question 25

Answer 25

See worked solution of calculating the equilibrium constant with the ion product of water constant at 25°C

Question 26

neutral pH

See picture below for calculation.

Answer 26

When there are exactly equal concentrations of H+ and OH-, as in pure water, the solution is said to be at ?

Explain the calculation for this.

Question 27

1. constant
2. ^-7 M
3. [OH^-]

Answer 27

1. ion product of water (Kw) is _____,
2. So… whenever [H⁺] is >1 x 10^-7 M, [OH^-] must be ______.
3. So, using the ion product of water we can calculate [H⁺] if we know _____, and vice versa

Question 28

Answer 28

What is the concentration of OH^- in a solution in which the H⁺ concentration is 0.00013 (1.3 x 10^-4) M?

Question 29

1. donors
2. acceptors

Answer 29

1. Acids are proton ____
2. Bases are proton _____

Question 30

conjugate acid base pair.

Answer 30

A proton donor and its corresponding proton acceptor make up a

Question 31

aqueous solution.

Answer 31

Each acid has a characteristic tendency to lose its proton in an

Question 32

proton

HCl

Answer 32

The stronger the acid, the greater its tendency to lose its ____? Give an example of a molecule that gives up a proton readily.

Question 33

H⁺

pH formula is below. Note in formula pH must be expressed in molar terms

Answer 33

The pH scale is a convenient method of designating the concentration of __ in any aqueous solution.

The term pH is defined by the expression:

Question 34

Answer 34

pH scale table.

Question 35

Answer 35

pH of some aqueous solutions

Question 36

7.4

Answer 36

What is the normal pH of blood?

Question 37

Acidosis is an increased acidity in the blood and other body tissue. It usually refers to acidity of the blood plasma.
Acidosis is said to occur when arterial pH falls below 7.35

Answer 37

What is Acidosis

Question 38

It refers to a condition reducing hydrogen ion concentration of arterial blood plasma (alkalemia), ie pH increase. Generally, alkalosis is said to occur when pH of the blood exceeds 7.45

Answer 38

What is Alkalosis?

Question 39

ionised

Answer 39

Strong acids and strong bases are completely _____ in dilute aqueous solutions.

Question 40

equilibrium constant (Keq)

Answer 40

The tendency of any acid (HA) to lose its proton and form its conjugate base (A-) can be defined by it’s ____ ____.

Question 41

ionisation constants, K_a (or dissociation constants).

Answer 41

Equilibrium constants for ionisation reactions are called ?

explain example formula

Question 42

large

small

Answer 42

Strong acids have a _____ Ka, and weak acids a ____ Ka

Question 43

Answer 43

pKa is analogous to pH and is defined as

Question 44

pKa

Answer 44

The stronger the tendency to dissociate a proton, the stronger the acid and the lower its ___.

Question 45

50%

Answer 45

pKa is the pH at which there is ___ ionisation, so [HA]=[A-]