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Chemistry 20 > Solutions > Flashcards

Solutions Flashcards

1
Q

Matter:

A

Anything with mass and volume.

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2
Q

Substance:

A

Matter with constant composition. All particles have the same properties. Eg. Water, helium

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3
Q

Mixture:

A

Matter with variable composition, made from two or more substances. Eg. Sand, soil

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4
Q

Element:

A

A substance made of atoms with the same atomic number. Eg. Lead, sodium

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5
Q

Compound:

A

A substance made from two or more elements chemically combined. Eg. Carbon dioxide

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6
Q

Homogenous Mixture:

A

A mixture made up of particles that are uniformly distributed. Eg. Saltwater

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7
Q

Heterogeneous Mixture:

A

A mixture made up of particles that are not uniformly distributed. Eg. Raisin bran

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8
Q

Solution:

A

Formed by dissolving a solute into a solvent.

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9
Q

Solute:

A

The dissolved substance in a solution which may be solid, liquid, or gas.

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10
Q

Solvent:

A

The medium containing a solute which can be any state of matter.

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11
Q

True or false: All mixtures are solutions but not all solutions are mixtures

A

False.

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12
Q

True or False: Not all mixtures are solutions, but all solutions are mixtures.

A

True.

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13
Q

Why is water a common solvent?

A

Because it is a polar molecule.

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14
Q

Hydration:

A

When H2O molecules gradually surround the ions.

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15
Q

Dissociation:

A

The separation of ions from each other.

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16
Q

Solvation:

A

The surrounding of solute particles by solvent.

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17
Q

The dissolving process:

A

Molecules become more spread out, energy is lost or gained.

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18
Q

Is dissolving a chemical or physical change?

19
Q

The steps of dissolving:

A

The solute breaks (endothermic), the solvent breaks (endothermic), the particles of both attract and create solvent bonds (exothermic).

20
Q

Miscible:

A

Liquids that dissolve in each other in all proportions.

21
Q

Immiscible:

A

Liquids that do not dissolve in other liquids at all.

22
Q

What is saturation at a molecular level?

A

Ions are crystallizing at the same rate that solid crystals dissolve.

23
Q

Electrolytes:

A

Solutions that conduct electricity and must contain ions.

24
Q

Factors that affect the rate of dissolving:

A

Particle size, temperature, nature of the particle, agitation/stirring.

25
Q

Factors that affect the solubility of substances in a solvent:

A

Temperature, pressure, miscibility.

26
Q

What factor most affects the solubility of a solid?

A

Temperature.

27
Q

What factor most affects the solubility of a gas?

28
Q

High solubility ionic compounds and bases dissociation:

A

Will dissociate into two ions when placed in water.

29
Q

Low solubility ionic compounds and bases dissociation:

A

Will not dissolve or dissociate in water.

30
Q

Strong Acids:

A

The 6 strong acids ionize completely to produce hydrogen ions and an anion

31
Q

Weak acids:

A

Do not ionize completely in water.

32
Q

High solubility molecular compound solubility:

A

Dissolve in water but do not dissociate

33
Q

High solubility molecular compounds:

A

H bonded compounds and sugar, group 17 elements.

34
Q

Low solubility molecular compound solubility:

A

Do not dissolve in water and do not dissociate.

35
Q

Low solubility molecular compounds:

A

No h-bonds.

36
Q

How to calculate grams per litre:

A

mass of solute/volume of solute

37
Q

How to calculate percent by mass (%m/v):

A

mass of solute (g)/volume of solution (mL) x 100

38
Q

How to calculate parts per million (ppm):

A

mass of solute (g)/volume of solution (mL) x 1000000

39
Q

How to calculate molar concentration (mol/L):

A

moles of solute (mol)/volume of solution (L)

40
Q

How to calculate mole ratio:

A

moles of required/moles of given

41
Q

What are the steps for preparing a solution?

A
  1. Calculate the required mass of solute
  2. Weigh (x) grams of solute and put in a clean, dry beaker
  3. Dissolve (x) grams with half the amount of the final volume of distilled water
  4. Transfer the solution into a volumetric flask using a funnel and rinse everything out
  5. Fill the volumetric flask up to the line with an eyedropper
  6. Stopper and invert.
42
Q

What is the formula for dilution?

A

C1V1 = C2V2

43
Q

What are the steps for the preparation of a solution by the dilution of a solution of higher concentration?

A
  1. Calculate the volume of concentrated solution required
  2. Transfer the concentrated solution into a dry beaker. Use a graduated cylinder for measuring (x) millilitres of concentrated solution
  3. Pipet the solution into a clean, dry 100 mL volumetric flask
  4. Add distilled water to the line using an eyedropper
  5. Stopper and invert
44
Q

When writing the equations for a chemical reaction, what are the three different steps?

A

Nonionic, total ionic, and net ionic.

Chemistry 20 (6 decks)

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