Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Solutions > Flashcards

Solutions Flashcards

1
Q

Arrhenius

A

Ionic compounds dissolve in water to conduct electricity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Why are ionic compounds so soluble in water?

A

When a substance dissolves in solution, particles of the substance separate from each other (breaks down into its ions)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Electrolytes

A

When electrolytes dissolve in solution both positive and negative charged particles are present

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Non-electrolytes

A
  • When non-electrolytes are dissolved in solution, neutral particles separate
  • neutral particles don’t conduct electricity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Dissociation

A
  • Separation of ions that occurs when an ionic compound dissolves in water
  • Do not show water as reactant or product
  • Pos. + Neg. = electrolytes
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Bases

A
  • Bases are ionic hydroxide compounds that dissociate in water and form a cation and hydroxide anion

Ex: NAOH (s) -> Na+ (aq) + OH- (aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Acids

A
  • Considered molecular compounds but conduct electricity in solution
  • Acids ionize into positive hydrogen ions (H+) and negative ions when dissolved in water
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Ionization

A
  • Process when neutral atom or molecule is converted to an ion
  • only applies to acids beginning with hydrogen
  • Pos. hydrogen ions + negative anions = electrolytes
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Endothermic reactions

A
  • Absorb energy from their surroundings
  • Require energy

Ex. Breaking bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Exothermic reactions

A
  • Release energy to their surroundings

Ex. Forming new bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Saturated Solution

A
  • A solution that contains the maximum amount of dissolved solute in the presence of a undissolved solute.
  • Some undissolved solute mist be present
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Super saturated solution

A
  • Solution that contains more dissolved solute than its solubility at a given temperature
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

2 ways to make a solution

A
  1. Preparing solutions from a solid to make a standardized solution
  2. Preparing solutions from a standardized solution using dilution
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Standard solution

A
  • Pre-made solution that has an accurate known concentration
  • Made by adding a known mass of a solid to a known volume of a solvent
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Stock Solution

A

Initially concentrated solution from which samples are taken and diluted
(standard solution)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Prepare standard solution by dilution

A
  • Use stock solution and add solvent to decrease concentration to desired lvl
  • Adding solvent to solution does not change quantity of solute (Mass of solute before and after is the same)
17
Q

Amount concentration

A
  • Chemical amount of solute dissolved in one litre of solution
  • c =n/v
    (mol/L)
18
Q

Concentration of ions

A
  • Dissociation/Ionization allow us to determine the amount concentration of ions or compounds
  • [unknown]=[known] x mol unknown/ mol known
19
Q

What happens to the concentration of a solution when more solute or solvent is added?

A

Solute- more concentrated

Solvent- decreased

20
Q

Concentrated solution

A

A solution that contains a large amount of solute, more than the amount it can dissolve

21
Q

Parts per million formulas

A

1 ppm = 1mL/L = 1mg/kg

ppm = g(10^6)/g

22
Q

Collision-reaction theory

A

Easiest way to get entities of a compound to collide w/ each other to form new entities is to dissolve them in solution

23
Q

Spectator Ions (net ionic equation)

A

Identical entities that don’t take part in the chemical reaction

24
Q

Equivalence Point

A

The point at which the exact theoretical amount of titrant has been added to completely react with the sample

25
Q

Endpoint

A

Th epoint during a titration when there is a sudden observable change

26
Q

pH Titration Curve

A

A graphic description of the reaction between acids and bases showing the progress of the reaction

  • y axis represents volume of titrant added
  • x-axis represents pH

Chemistry (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions