Section 1
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The greater the value of Kp, the ________ the extent of the dissociation of the acid and the _______ the acid
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Cards (59)
Section 1
(50 cards)
The greater the value of Kp, the ________ the extent of the dissociation of the acid and the _______ the acid
Greater Stronger
HA
Symbolization for a weak acid
Amphoteric
A substance that can function as an acid and a base.
You can find the pH of a strong acid from its...
Concentration
Strong acids never reach ________. (2)
Equilibrium There is no equilibrium constant
Solubility Determination
A salt can be considered soluble if more than 1 gram of the salt can be dissolved in 100 milliliters of water.
Common way to cause a pressure shift on a reaction
Change the volume of the container
Le Chatelier's Principle
States that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.
Diprotic Acid
an acid that can donate two protons per molecule
Buffers are made from...
Salt Weak acid or base
Arrhenius model
States that an acid releases H+ ions and a base releases OH- ions
For a polyprotic acid, the titration curve will have as many...
Bumps as there are hydrogen ions to give up
pH Scale
measurement system used to indicate the concentration of hydrogen ions (H+) in solution; ranges from 0 to 14
Ksp
Solubility product
Conjugate acid base pair
consists of two substances related to each other by donating and accepting of a single hydrogen ion
Acid Dissociation Constant
An equilibrium expression used to measure weak-acid strength, given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations, with each term raised to the power of its stoichiometric coefficient. Denoted Ka.
At Equilibrium, DeltaG=
0
Bronsted-Lowry definition of a base
Substance that is capable of accepting a proton
If Q is less than K...
The reaction shifts to the right
Equilibrium Constant
Ratio of concentrations of the products to the concentrations of the reactants at the point of equilibrium, where each reactant and product in the expression is raised to the power of its stoichiometric coefficient. Commonly denoted by Keq.
A change in _______ will also affect the ________ _______ of the reaction.
Temperature Equilibrium constant
Lewis Acid
An atom, ion, or molecule that accepts an electron pair to form a covalent bond.
Q (2)
Concentration or Pressure
Bronsted Lowry Model
an acid is a hydrogen-ion donor and a base is a hydrogen ion to a base
Equilibrium Expression
the expression obtained by multiplying the product concentrations and dividing by the multiplied reactant concentrations, with each concentration raised to a power represented by the coefficient in the balanced equation
The acid with the most H+'s will give up H+ more easily, making it a _____ _____.
Stronger Acid
Oxyacid
An acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal
When DeltaG is positive, K must be
Less than 1 Reactants will be favored at equilibrium
When solving for equilibrium, omit _______ and _______.
Solids and liquids
Reaction Quotient
Ratio of the concentrations of the products to the concentrations of the reactants at any point during the reaction aside from equilibrium, where each reactant and product in the expression is raised to the power of its stoichiometric coefficient. Commonly denoted by Q.
Half-Equivalence Point
Enough base has been added to convert exactly half of the acid into conjugate base Concentration of acid is equal to the conjugate base (pH=pKa)
Percent dissociation
the ratio of the amount of a substance that is dissociated at equilibrium to the initial concentration of the substance in a solution, multiplied by 100
You can only use ________ or _______ of reactions at ________ to calculate K.
Concentrations Pressures Equilibrium
Temperature and Equilibrium Constant Relationship
Increasing temp decreases the value of the EC Causes there to be a larger amount of reactants at equilibrium than products Decreasing temp increased the value of the EC Causes there to be a larger amount of products at equilibrium than reactants
Common Ion effect
A weak acid and its conjugate base can remain in solution together without neutralizing each other
Chemical Equilibrium
In a chemical reaction, the state in which the rate of the forward reaction equals the rate of the reverse reaction, so that the relative concentrations of the reactants and products do not change with time.
Determining the equilibrium in a reaction when temperature is changed (2)
1. Rewrite equation by adding heat to the correct side 2. If temp is increased, the reaction will shift away from the added energy. If the temp is decreased, the reaction will shift toward the added energy.
When DeltaG is negative, K must be...
Greater than 1 Products will be favored at equilibrium
When the external pressure is decreased, the reaction will...
Shift to the side with more gas molecules
Law of Mass Action
The rate of a chemical reaction is proportional to the product of the concentrations of the reactants
Kp
Partial Pressure constant
Bronsted-Lowry definition of an acid
Substance that is capable of donating a proton
If Q=K...
The reaction is at equilibrium
Amphoteric
Substance with the ability to act as a acid or base
Equilibrium position
The relative concentrations of reactants and products of a reaction that has reached equilibrium; indicates whether the reactants or products are favored in the reversible reaction
If Q is greater than K...
The reaction shifts to the left
When external pressure is increased, the reaction will...
Shift to the side with fewer gas molecules
Common Amphoteric Molecules (3)
H2PO4 HSO4 H2O
If both sides of the reaction have an equal amount of moles of gas, then...
Changing the pressure/volume has no effect on the reaction
Polyprotic Acids
Acids with more than one H+. (H2SO4, H3PO4, etc.)
Section 2
(9 cards)