Unit 10- Acids & Bases Section Flashcards
What model is used for acid/base identification?
Bronsted-Lowry Model
According to the Bronsted-Lowry model, acids are proton _____ and bases are proton _____.
Donors- Acceptors ADBA (Acids donate, Bases accept)
Acids will always turn into a ______.
Conjugate Base
Bases will always turn into a ______.
Conjugate Acid
Write an equilibrium expression that represents the autoionization of water.
Kw= [H+][OH-]= 1.00x10^-14
pH= _____
-log[H+]
pOH= _____
-log[OH-]
pH+pOH=
14
[H+]=
10^-pH
[OH-]=
10^-pOH
When determining the number of significant figures of pH and pOH, it’s the _____.
Numbers after the decimal point that matter.
If the pH of what we’re adding to water is smaller than it, the pH is _____.
7
The difference between strong acids/bases and weak acids/bases is the _____.
% ionization
What are the strong acids?
HClO4, HI, HBr, HCl, H2SO4, HNO3
Strong acids ionize _____.
Completely
Weak Acids are only partially _____.
Ionized
The stronger the acid, the weaker the corresponding conjugate _____.
Base
The equilibrium always lies to the side of the _____ acid and _____ base.
Weaker-Weaker
The strongest acid that can exist in aqueous solution is _____.
H3O+
The strongest base that can exist in aqueous solution is _____.
OH-
What are the strong bases?
LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
Polyprotic Acids are acids with _____
Multiple ACIDIC hydrogens
Give some examples of monoprotic acids.
HC2H3OH-HCl-HF-HNO3
Give some examples of diprotic acids.
H2SO4-H2CO3-H2CrO4
Give some examples of triprotic acids
H3PO4-H3PO3
What do the prefixes of the acids tell us?
It tells us how many hydrogens are coming off
For every reaction of polyprotic acids we have, we have a different _____
Equilibrium Constant
For monoprotic acids, we can write _____ equation, for diprotic acids, we can write _____ equations, for triprotic acids, we can write _____ equations.
1-2-3
If you have a polyprotic acid and you’re asked about the pH, you only need _____.
One ICE Chart
For polyprotic acids, the x is the second equation will always be equivalent to the _____.
Second Equilibrium Constant
% Dissociated=
Amount Dissociated (M)/ Initial Concentration (M) x100
For a weak acid, the percent dissociation _____ as the acid becomes more dilute.
Increases
When electrons are localized, the bases will be _____
Stronger
If you have a conjugate of a _____ substance, the thing can go back.
Weak
What are the steps in determining whether salts are acidic, basic, or neutral?
First, you separate the two ions and add/subtract a hydrogen depending on the ion. Then, depending on which substance is a strong acid or a base, you determine it.
Kw=
Ka.Kb
When thinking about the strength of acids, it is important to look at two factors:
The strength of the H-X bond and the polarity of the H-X bond.
When electrons are localized, the acids will be _____.
Weaker; so, for example, in HClO4, since the electrons are going to be around all of the oxygens as opposed to HClO in which all the electrons are going to be around 1 oxygen, the Ka value of HClO4 will be significantly larger than that of HClO’s
