Acids and Bases Flashcards
Acids
Ahhenius definition: Molecular compound that dissociates in water to generate H+/H3O+ ions
Monoprotic acid
Acid that can donate only one proton (H+ ion) per molecule in solution
ex. HCL, HNO3 (nitric acid), CH3COOH (acetic acid)
Diprotic acids
Can donate two protons H+ ions per molecule in solution, usually in two steps
ex. H2CO3 (carbonic acid) and H2C2O4 (oxalic acid)
Triprotic Acids
Acid that can donate three H+ proton per molecule in a solution one at a time
ex.
Phosphoric acid (H3PO4)
Cotroc acod (H3C6H5O7
Polyprotic acids
Any acid that can donate more than 1 H+ and includes all diprotic and polyprotic ions
Strong acids
HCl
HBr
HI
HNO3
H2SO4
HClO4
Hi, HI, BRing NO SOda CLOse
How to name binary acids (acids that consist of two elements H and a nonmetal)
- Anions are either monotomic or non-oxyanions
- “Hydro” + base name + ic acid
ex. HI - Hydroiodic acid
How to name oxyacids
- Anions are oxyanions (NO3^-, ClO4^-)
-ate turns to -ic acid
ex. H2CO3 = Carbonic acid - site turns to -ous acid
H2SO3 = Sulfurous acid
Base
Species that is H+ acceptor
Arrhenius definition: A base is a compound that generates OH (hydroxide) ions when placed in water
Strong bases
Compounds that release strong OH- ions in a solution and are soluble in water
Group 1 cations
LiOH
NaOH
KOH
RbOH
CsOH
Ca(OH)2
Sr(OH)2
Ba(OH)2
What is the difference between strong and weak acids
The strong acids due to completely ionizing, due to every strong acid molecule donating their H+ ion. Weak acids do ionize only partially and leaves unionized molecules in the reaction.
As result there is an equilibrium where the reactions are reversible.
Difference between strong and weak bases
Strong bases fully dissociate which means they fully release all OH- ions when dissolved resulting in a high OH concentration
On the other hand weak bases dissociate partially which means only some molecules release OH, leaving a lower OH concentration
Spectator ions
Ions that do not change during a reaction
Identified when they are found on both sides of a full ionic equation
How do you identify spectator ions and precipitates based on the solubility rules
You can identify precipitates by identifying ions that are exceptions and insoluble in water
You can identify spectator ions by identifying ions are soluble
Weak acids
HF
HNO2
HClO
HCN
HC2H3O2
NH4+ (Ammonium)
Weak bases
NaF
NaNO2
KClO
KCN
NaC2H3O2 (Sodium acetate)
NH3 (Ammonia)
What is pH
Scale that measures acidity or basicity of a solution, indicating the concentration of H+ in a solution
Ranges from 0-14 with lower values indicating higher acidity and higher values indicating greater basicity
What is the pH of acidic solutions
pH < 7 (High H+, low OH-
What is the pH of neutral solutions
pH = 7 (like pure water, where H+ = OH-)
What is the pH of basic solution
pH > 7 (low H+, high OH-)
Conjugate Acid-Base Pairs
The conjugate of an acid is the base that forms when the acid loses a proton (H⁺).
Conversely, the conjugate of a base is the acid that forms when the base gains a proton.
For Acids (Finding the Conjugate Base):
When an acid donates a proton (H⁺), it turns into its conjugate base.
To find the conjugate base of an acid, remove one H⁺ from the acid formula.
Example: For the acid HCl, if it donates an H⁺, it becomes Cl⁻, which is the conjugate base of HCl.
Conjugate bases have the ability to accept the the H+ back thus it is a base
For Bases (Finding the Conjugate Acid)
When a base accepts a proton (H⁺), it turns into its conjugate acid.
To find the conjugate acid of a base, add one H⁺ to the base formula.
Example: For the base NH₃ (ammonia), if it gains an H⁺, it becomes NH₄⁺ (ammonium), which is the conjugate acid of NH₃.
BAAD
Bases Accept Acids Recieve
Bronsted Lowry definition of acids and bases
Acids are H+ donators
Bases are H+ acceptors
Lewis acid definition
An electron pair acceptor
Lewis base definition
An electron base donor
What is the net ionic equation and what does it tell us?
Simplified version of a chemical reaction that shows the species that participate in the chemical reaction by removing the spectator ions
In acid-base reactions it shows the transfer of H+ or OH ions
In precipitations reactions: It shows only the ions that form an insoluble compound which is the preciptate
What is a precipitation reaction?
An insoluble ionic compound that forms upon mixing two aqueous solutions of ionic compounds
To get, swap the ions so the cation from one compound partners with the anion from the other compound
Predict precipitates using the solubility rules
How do you write complete ionic equations
Write balanced molecular equation
- Use correct chemical formulas
- Determine states of compounds based on wording (species dissolved in water are (aq)) and precipitates that form are (s) and solubility rules
Write complete ionic equation
- Go species by species and dissociate strong electrolytes present in aqueous solutions
- weak acids and nonelectrolytes do not get separated
Write net ionic equation
- Cancel spectator ions
- Make sure balanced coefficients are expressed in lowest whole number
Dissociate species that a
nonelectrolytes and undissolved solids associated.
Unique aspect of Mercury Hg when given in a chemical equation
It forms Hg2^2+ to gain stability
