Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
18 Cards in this Set
- Front
- Back
|
According to Arrhenius, what is the definition of an acid and a base ?
|
1. Acid: A substance that when dissolved with water, it increases the concentration of hydrogen ions
2. Base: A substance that when dissolved with water, it increases the concentration of hydroxide ions |
|
|
What is a Bronsted-Lowry acid and base ?
|
1. Acid: A substance that willingly donates a proton
2. Base: A substance that willingly receives/accepts a proton |
|
|
What are species called that can both act as an acid or a a base ?
|
Amphiprotic or amphoteric.
|
|
|
How does the Bronsted-Lowry concept enlarge Arrhenius' concept ?
|
1. Expands it to include substances that only contain H+ ions
2. Includes ions and molecules 3. Enables us to write acid-base reactions that are not just restricted to aqueous solutions 4. Allows some species to sometimes be both an acid or a base |
|
|
What is the conjugate acid and base of water ?
|
Acid - H+ or H3O+
Base- OH- |
|
|
True or false: It is safe to assume that weak acids will yield weak conjugate bases.
|
True.
|
|
|
True or false: In any acid-base reaction, the equilibrium will favor the reaction that gives the proton to the weakest base.
|
False. It will favor the reaction that gives it to the strongest base.
|
|
|
What is self-ionization in water ?
|
A process where two water molecules react with one another to form one hydronium ion and one hydroxide ion.
|
|
|
What is the ion product constant ?
|
1.0 x 10^-14 = Kw = [H+][OH-].
|
|
|
What is the equation for pH and pOH respectively ?
|
pH = -log[H+]
pOH = -log[OH-] |
|
|
What will pH + pOH always equal ?
|
14.
|
|
|
How would you calculate [H+] from pH ?
|
[H+] = 10^-pH.
|
|
|
True or false: In a very strong poliprotic acid, the [H+] = [acid].
|
False. This is true for a very strong monoprotic acid.
|
|
|
Give the expression for the acid dissociation constant.
|
k = ([H+][A-]) / [HA]
|
|
|
What can you deduce from a large Ka value ?
|
That the acid is strong because it almost dissociated completely.
|
|
|
True or false: The acid strength of an acid decreases with an increasing negative charge.
|
True.
|
|
|
True or false: The acid strength of an acid decreases with an increase in number of oxygen atoms inside that molecule.
|
False. The acid strength increases.
|
|
|
What is the definition of a Lewis acid and base, respectively ?
|
1.Acid- A electron pair acceptor/receiver
2. Base- An electron pair donator |
