Matter as "Solutions, Acids, and Bases" Flashcards
1
Q
What is “solute”?
A
- The small, minor component added in the solvent to dissolve.
2
Q
What is a “solvent”?
A
- The medium in which the solute is dissolved in.
3
Q
What is “dissolving”?
A
- Chemical process
- Individual particles of the solute disperse throughout a solvent
4
Q
What is “dissociation”?
A
- Separating an ionic compound -> to ion
5
Q
What is “ionization”?
A
- Neutral atom or molecule turns into ion
- Acids ionize in water
6
Q
What is “electrolytes”
A
- Conduct electricity
7
Q
What compounds are electrolytes?
A
- Ionic
- Acids
- Base
8
Q
What is the Process of Dissolving?
A
- Bonds between particles in the solute break
- Some inter molecular forces between the particles of the solvent break.
- Particles of the solute and solvent attract -> new chemical bond
9
Q
Difference between Endothermic VS Exothermic dissolving.
A
- Endo : More energy ABSORBED to break the bonds
- Exo: More energy RELEASED when the solute solvent bonds form.
10
Q
What is a “saturated solution”?
A
- solution is at MAX concentration
- no more solute will dissolve
- dynamic equilibrium
11
Q
What is “solubility”?
A
- the concentration of a saturated solution
- depends on temp, pressure, and chemical properties like polarity
12
Q
Solubility of states
A
- Solids: High solubility, High temp
- Gases: High solubility, Low temp, High pressure
- Liquids: High solubility, High temp
13
Q
Solubility of Ionic Compounds
A
- most dissolve in water
- Greater than 0.1 mol/L = high solubility
- Less than 0.1 mol/L = low solubility
14
Q
Solubility of Molecular Compounds
A
- polar compounds have higher solubility
- nonpolar have low solubility
- hydrogen bonding have higher solubility
15
Q
Dynamic Equilibrium
A
- Some solids are dissolving, some are crystallizing
- Meaning, no net change
- Solubility equilibrium is established by adding solute to solvent or mixing two solutions.
16
Q
What is “concentration”?
A
- Ration comparing solute to solution
- C = n/V
17
Q
What is “molar concentration”?
A
- chemical amount of solute dissolved in one liter of solution.
- Can use by brackets. [NaCl]
- Can be represented by “M”
18
Q
What is “percent concentration”?
A
- number of units of solute per 100 units of solution
- pick mL & g ORR L & kg
19
Q
What is “part per million concentration”?
A
- number of units of mass of the solute per million units of solution
- mg/L
- mg/kg
20
Q
Molar concentration of ions in solution after ______ or ______ is ______ to the mole ratio of the balanced equation.
A
- dissociation
- ionization
- proportional
21
Q
What is “standard solution” ?
A
- solution of an accurately known concentration
22
Q
What is “dilution”?
A
- Adding water to decrease the concentration of a solution
23
Q
Acids in Empirical and Arrhenius Theory
A
Empirical: Blue to Red and are electrolytes.
Arrhenius: Ionize to form Hydrogen ions
H+
24
Q
Bases in Empirical and Arrhenius Theory
A
Empirical: Red to Blue, and are electrolytes.
Arrhenius: Dissociate to form Hydroxide.
OH - ions
25
How to identify acid and bases from chemical formula?
- Acids will start with H with an anion after, OR end in COOH
- Bases will have OH as the anion.
26
How to write Acids in classical and IUPAC acid name?
- ends with an "ide" do -> hydro ___ ic acid
- end with an "ate" do -> ___ic acid
- end with an "ite" do -> ___ous acid.
IUPAC: Just add aqueous
27
How to remember the acid name?
ide - Crush: "ide (hi)" You: "Hi...ick..."
ate - You: (ate something icky)
ite - Homie: "ight" meaning "out" (ous)
28
Steps to prepare solution
1. Calc mass of solid required
2. Now measure the mass you require using a balance
3. Dissolve with half the amount of water
4. Transfer to a volumetric flask using a funnel
5. Add water with eye dropper
6. Invert to shake
29
In modern Arrhenius theory, acids that react with water produce?
- Hydronium ions and conjugate base
30
In modern Arrhenius theory, bases that react with water produce?
- Hydroxide ions and conjugate acid
31
H20 + H20?
- H30 + OH
32
Ionic Hydroxide
- Base
- Dissociate
33
Molecular compounds
- Acid
- React with water
34
Ionic compounds
- Dissociate first
- Take anion and react with water
35
Metallic oxide
- Basic
- React with water
- Dissociate
36
Non-metallic oxide
- Acidic
- React with water
- Take the new product and react with water again
37
Aqueous solutions, at 25C, they can be classified as.
- Neutral. pH = 7
- Acidic. pH <7
- Basic. pH >7
38
pH/pOH = ?
-log[ ]
39
[H30/OH] = ?
10^ - pH/pOH
40
SA & SB Major Entities
- Products and Water
41
WA & WB Major Entities
- Reactants
42
Monoprotic
- One Hydrogen Atom
- One charge
43
Polyprotic
- More than one Hydrogen Atom
- >1 charge
- Keep going until monoprotic
- Reaction with water decreases with each step (gets weaker)
44
Major Entities in high & low solubility in Ionic Compounds
- High: Separate
- Low: Stay
45
Major Entities in high & low solubility in Molecular
- High: Stay
- Low: Stay
46
Major Entities in high & low solubility in Bases
- High: Separate
- Low: Stay
47
Major Entities in high solubility in Strong Acids
- High: Separate
48
Major Entities in high solubility in Weak Acids
- High: Stay
