Top2-Ch2-P54-58 Flashcards
Picture of hydronium in action
Keq gives the position of ?
Give the formula
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.
See worked solution of calculating the equilibrium constant with the ion product of water constant at 25°C
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.
neutral pH
See picture below for calculation.
- ion product of water (Kw) is _____,
- So… whenever [H+] is >1 x 10-7 M, [OH-] must be ______.
- So, using the ion product of water we can calculate [H+] if we know _____, and vice versa
- constant
- -7 M
- [OH-]
What is the concentration of OH- in a solution in which the H+ concentration is 0.00013 (1.3 x 10-4) M?
- Acids are proton ____
- Bases are proton _____
- donors
- acceptors
A proton donor and its corresponding proton acceptor make up a
conjugate acid base pair.
Each acid has a characteristic tendency to lose its proton in an
aqueous solution.
The stronger the acid, the greater its tendency to lose its ____? Give an example of a molecule that gives up a proton readily.
proton
HCl
The pH scale is a convenient method of designating the concentration of __ in any aqueous solution.
The term pH is defined by the expression:
H+
pH formula is below. Note in formula pH must be expressed in molar terms
pH scale table.
pH of some aqueous solutions
What is the normal pH of blood?
7.4
What is Acidosis
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
What is Alkalosis?
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
Strong acids and strong bases are completely _____ in dilute aqueous solutions.
ionised
The tendency of any acid (HA) to lose its proton and form its conjugate base (A-) can be defined by it’s ____ ____.
equilibrium constant (Keq)
Equilibrium constants for ionisation reactions are called ?
explain example formula
ionisation constants, Ka (or dissociation constants).
Strong acids have a _____ Ka, and weak acids a ____ Ka
large
small
pKa is analogous to pH and is defined as
The stronger the tendency to dissociate a proton, the stronger the acid and the lower its ___.
pKa
pKa is the pH at which there is ___ ionisation, so [HA]=[A-]
50%
