Acids and Bases

Question 1

Acids

Answer 1

Ahhenius definition: Molecular compound that dissociates in water to generate H+/H3O+ ions

Question 2

Monoprotic acid

Answer 2

Acid that can donate only one proton (H+ ion) per molecule in solution

ex. HCL, HNO3 (nitric acid), CH3COOH (acetic acid)

Question 3

Diprotic acids

Answer 3

Can donate two protons H+ ions per molecule in solution, usually in two steps

ex. H2CO3 (carbonic acid) and H2C2O4 (oxalic acid)

Question 4

Triprotic Acids

Answer 4

Acid that can donate three H+ proton per molecule in a solution one at a time

ex.
Phosphoric acid (H3PO4)
Cotroc acod (H3C6H5O7

Question 5

Polyprotic acids

Answer 5

Any acid that can donate more than 1 H+ and includes all diprotic and polyprotic ions

Question 6

Strong acids

Answer 6

HCl
HBr
HI
HNO3
H2SO4
HClO4

Hi, HI, BRing NO SOda CLOse

Question 7

How to name binary acids (acids that consist of two elements H and a nonmetal)

Answer 7

• Anions are either monotomic or non-oxyanions
• “Hydro” + base name + ic acid

ex. HI - Hydroiodic acid

Question 8

How to name oxyacids

Answer 8

• Anions are oxyanions (NO3^-, ClO4^-)
  -ate turns to -ic acid
  ex. H2CO3 = Carbonic acid
• site turns to -ous acid
  H2SO3 = Sulfurous acid

Question 9

Base

Answer 9

Species that is H+ acceptor

Arrhenius definition: A base is a compound that generates OH (hydroxide) ions when placed in water

Question 10

Strong bases

Answer 10

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

Question 11

What is the difference between strong and weak acids

Answer 11

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.

Question 12

Difference between strong and weak bases

Answer 12

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

Question 13

Spectator ions

Answer 13

Ions that do not change during a reaction

Identified when they are found on both sides of a full ionic equation

Question 14

How do you identify spectator ions and precipitates based on the solubility rules

Answer 14

You can identify precipitates by identifying ions that are exceptions and insoluble in water

You can identify spectator ions by identifying ions are soluble

Question 15

Weak acids

Answer 15

HF
HNO2
HClO
HCN
HC2H3O2
NH4+ (Ammonium)

Question 16

Weak bases

Answer 16

NaF
NaNO2
KClO
KCN
NaC2H3O2 (Sodium acetate)
NH3 (Ammonia)

Question 17

What is pH

Answer 17

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

Question 18

What is the pH of acidic solutions

Answer 18

pH < 7 (High H+, low OH-

Question 19

What is the pH of neutral solutions

Answer 19

pH = 7 (like pure water, where H+ = OH-)

Question 20

What is the pH of basic solution

Answer 20

pH > 7 (low H+, high OH-)

Question 21

Conjugate Acid-Base Pairs

Answer 21

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.

Question 22

For Acids (Finding the Conjugate Base):

Answer 22

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

Question 23

For Bases (Finding the Conjugate Acid)

Answer 23

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.

Question 24

BAAD

Answer 24

Bases Accept Acids Recieve

Question 25

Bronsted Lowry definition of acids and bases

Answer 25

Acids are H+ donators

Bases are H+ acceptors

Question 26

Lewis acid definition

Answer 26

An electron pair acceptor

Question 27

Lewis base definition

Answer 27

An electron base donor

Question 28

What is the net ionic equation and what does it tell us?

Answer 28

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

Question 29

What is a precipitation reaction?

Answer 29

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

Question 30

How do you write complete ionic equations

Answer 30

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.

Question 31

Unique aspect of Mercury Hg when given in a chemical equation

Answer 31

It forms Hg2^2+ to gain stability