Chem Lesson 4: 14.1 - 14.3 Flashcards
Bronsted Lowry Acid
Give up a proton (H+)
Bronsted Lowry Base
Accepts/Receives a proton (H+)
Conjugate Base
The species that remains when an acid donates a H+
Conjugate Acid
When a base accepts a proton (H+)
Acid Ionization
Reaction between a Bronsted Lowry acid and water
Base Ionization
Reaction between a Bronsted Lowry base and water
Amphiprotic
Capable of accepting and donating protons (polyatomic)
Autoionization
When two of the same molecules react to yield ions.
Water breaking down into hydronium and hydroxide.
H2O(l) + H2O(l) —> <— H3O+(aq) + OH-(aq)
Kw (Definition)
Ion product constant for water (equlibrium)
Let’s us to see the concentrations of either the [OH-] and/or [H3O+] in water.
Kw (temp and value)
25c and 1.0*10^-14
Amphoteric Elements (how can you tell by looking at molecule if it can be both and Acid or Base?)
H—-^- (Start with H and end with a neg charge)
H2O or NH3
Neutral Solution
Contains equal concentrations of hydronium (or H+) and hydroxide ions.
Acidic Solutions
Contains higher concentrations of hydronium (or H+) than hydroxide.
Basic Solution
Contains higher concentration of hydroxide (OH-) in comparison with hydronium (or H+)
PH
Measures the concentration of H+ ions in solution in comparison to hydroxide ions. (Tells us how acidic a solution is).
POH
Measures the concentration of hydroxide ions in a solution in comparison to H+. (Tells us how basic a solution is)(OH-)
PH and POH vs [H+] [OH-]
-PH and POH tells us how basic/acids a solution is. (The concentrations of each compared to each other)
-[H+] [OH-] tells us how many moles of H+ OH- are in a solution.
PH (equation)
PH = -log[H+]
POH (equation)
PH = -log[OH-]
Find Molar of H given PH (equation)
H = 10^-PH
Find Molar OH given PH (equation)
OH = 10^-PH
Sig Fig log rule (PH and OH)
Keep as many decimal places are there sig figs in the question when working with log
PH < 7
More acidic. (More H+ than OH-)
PH > 7
More basic. (More OH- than H+)
PH Scale rule/equation (How much more basic is 9 to 7 on the PH scale?)
10^deltaPH
10^9-7 = 10 ^2 = 100 times
PH + POH = 14 (can only be used at what temp?)
At 25c
Strong Acids (def)
Ionize to a great extent in water to create hydronium. More readily to give up an proton.
Strong Acids Mnemonic
So I Brought No Clean Clothes
Strong Bases (Period Table) - what do they exclude as well?
Group 1 and group 2 cations, besides the first and last in each group.
The stronger the acid or base the x its conjugate partner. (x = weaker or stronger?)
Weaker
Ka * Kb = Kw = 1.0*10^-14
The weaker the acid or base the x its conjugate partner. (x = weaker or stronger?)
Stronger
Ka * Kb = Kw = 1.0*10^-14
Percent Ionization Equation
([Ions (H+,OH-,H3O+)] / Original Molecule) * 100
Acid Ionization Constant (Ka)
Equilibrium constant for an acid (product/reactant).
-Used to determine the strength of a weak acid. (The higher the constant the stronger the acid)
Ka (Equation)
Concentration of ions (product)/Concentration of unionized acid
Base Ionization Constant (Kb)
Equilibrium constant for a base (product/reactant).
-Used to determine the strenght of a base. (Higher the number the stronger the base)
Strong Acids and Base (definition)
Acids and bases that ionize completely in water to form electrically charged atoms and molecules.(Nothing left over from the reactant)
Neutralization Reaction
When an acid reacts with a base.
Relative Trends of Strong Acids/Bases and their Conjugate Bases/Acids
Strong Acid —> Neutral
Conjugate Base
Strong Base —> Neutral Conjugate Acid
Leveling Effect (Acid)
Acids stronger than H3O+ can’t be used in water or it will interact. (Can’t use acids stronger than the conjugate acid of the solvent).
Leveling Effect (Base)
Bases stronger than OH- can’t be used in water or it will interact. (Can’t use Bases stronger than the conjugate base of the solvent).
Aqueous solution (means combing with what?)
H2O (water)
Atomic Number
Number of protons in the nucleus which determines it’s chemical properties
Mass Number
Some of number of Protons and Neutrons.
Solute
Substance that is dissolved in a solution.
Solvent
What the solute is dissolved in to form a solution.
Strong Acids/Bases
Breakups (ionizes) completely into it’s conjugate base/acid in water.
(More product than reactant)
Weak Acids/Bases
Only a small amount breakups (ionizes) into it’s conjugate base/acid in water. <5%
(More reactant than product)
(They don’t readily want to accept or give up protons).
Why do strong acids/bases produce neutral conjugates
The resulting cation and anion are so weak that they don’t react in water (readily accept protons).
The stronger the base or acid the (x) it’s conjugate is?
Weaker
Dissociation (Ionic Compound)
When an Ionic Compound breaks apart in a solution (water)
Covalent Compound
Compounds that are combined through the sharing of electrons.
Ionic Compound
Compounds made from ionic bonds (electron transfer).
Bases are x and Acid are x compounds?
(Covalent or ionic)
Bases are Ionic and Acids are covalent.
Balancing Neutralization Reactions (Tip) Balance what first?
Balance the Base and Acid First.
Arrhenius Base
Base that gives off OH- ions (hydroxide).
Two Acid types
Oxoacid and Binary
Oxoacid
Acid that contains hydrogen, oxygen, and one other element.
Oxoacid strength Trends
- More oxygen more acidic. (Most important).
- More electronegative the stronger it is. (Bottom left to top right).
Oxobase (strength trend)
Opposite of oxoacid
Binary Acid
Acid composed of two elements.
(Hydrogen and non-metal).
Electronegativity (bottom left to top right).
The tendency of an atom to attract electrons towards itself.
Binary Acid (Acidity trend)
- Acid strength increases as you go down a group. (size/atomic radius). Most important factor.
- Increase when going left to right across a period because of electronegativity. (Use if they’re in the same period).
Binary Base Trend
- Basicity Increase as we go up period. (Smaller the atomic radius)
- Basicity Increase as we go to the left across the period table.
(Less electronegativity).
Why the more electronegative and acid becomes the stronger it is?
Electronegativity is the tendency for an electron to become more negative and acids do that by giving up H+ ions.
Binary Acid Trend Acidity
Across a period and down increases acidity. (So see which non H is the most to the right and down).
Because the atomic radius increases and the attraction of the H+ ion to it’s nucleus isn’t as much so it’s more likely to lose it.
When PH the solution becomes more..?
Acidic
When POH increases the solution becomes more…?
Basic
Strong Base PH
> 10
Strong Acid PH
1 or less
Autoionization of water (endo or exo)
Endothermic
How does an increase or decrease in temp affect Autoionization
Increase in heat moves reaction to the right so the concentration of H+ and OH- increases which in turn increases the KW.
Affects of Temp on Autoionization of Water
When temp PH decreases but the solution remains neutral.
% Ionization Equation for OH or H+
Ionization % = [OH]/[initial solution] %100
When to use Ice Tables
When the amount of reactant or product must be determined from the amount of the other reactant or problem.
Is PH at equilibrium?
Yes
Mass Percent Equation
(Mass of concentration/Mass of solution) * 100
