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Organic and Inorganic Chemistry > solutions - Sheet1 > Flashcards

solutions - Sheet1 Flashcards

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1
Q

Substance that does not conduct an electric current in water.

A

Nonelectrolyte

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2
Q

Elements, covalent compounds, and ionic compounds.

A

Pure substances

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3
Q

Dissociates completely in water to form ions.

A

Strong electrolyte

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4
Q

Most matter come into contact with is a mixture of two or more pure substances.

A

Mixtures

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5
Q

Does not have a uniform composition throughout the sample.

A

Heterogeneous mixture

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6
Q

Dissociates partially in water to form some ions, leaving mostly uncharged molecules.

A

Weak electrolyte

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7
Q

Has a uniform composition throughout the sample.

A

Homogeneous mixture

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8
Q

Homogeneous mixture that contains small particles; liquid solutions are transparent.

A

Solution

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9
Q

Substance present in a lesser amount in a solution.

A

Solute

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10
Q

Substance present in a larger amount in a solution.

A

Solvent

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11
Q

Homogeneous mixture with larger particles, often having an opaque appearance; particles cannot be filtered and do not settle out.

A

Colloid

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12
Q

Number of moles of charge that a mole of ions contributes to a solution.

A

Equivalent (Eq)

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13
Q

Heterogeneous mixture containing large particles suspended in a liquid; particles do not dissolve, can be filtered or separated using a centrifuge.

A

Suspension

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14
Q

In solutions that contain ions, there must be a balance between total positive and total negative charge.

A

Charge balance in solutions

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15
Q

Amount of solute that dissolves in a given amount of solvent, usually reported in grams of solute per 100 mL of solution (g/100 mL).

A

Solubility

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16
Q

Contains the maximum number of grams of solute that can dissolve.

A

Saturated solution

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17
Q

Contains less than the maximum number of grams of solute that can dissolve.

A

Unsaturated solution

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18
Q

Substance that conducts an electric current in water.

A

Electrolyte

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19
Q

Like dissolves like.

A

Solubility principle

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20
Q

Solubility of a gas in a liquid is proportional to the partial pressure of the gas above the liquid.

A

Henry’s law

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21
Q

Tells how much solute is dissolved in a given amount of solution.

A

Concentration of a solution

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22
Q

Number of grams of solute dissolved in 100 mL of solution.

A

Weight/volume percent concentration (w/v%)

23
Q

Solvation releases more energy than required to separate particles, resulting in heat release.

A

Exothermic process

24
Q

Separation of particles requires more energy than is released during solvation, resulting in heat absorption.

A

Endothermic process

25
Q

A compound is soluble if it contains one of the following cations: Group 1A cations: Li⁺, Na⁺, K⁺, Rb⁺, Cs⁺ or Ammonium, NH₄⁺.

A

Rule 1: Solubility of ionic compounds based on cations

26
Q

A compound is soluble if it contains one of the following anions: Halide ions: Cl⁻, Br⁻, I⁻ (except for salts with Ag⁺, Hg₂²⁺, Pb²⁺), Nitrate, NO₃⁻, Acetate, CH₃CO₂⁻, Sulfate, SO₄²⁻ (except for salts with Ba²⁺, Hg₂²⁺, Pb²⁺).

A

Rule 2: Solubility of ionic compounds based on anions

27
Q

An anion with the formula NO₃⁻.

A

Nitrate

28
Q

An anion with the formula CH₃CO₂⁻.

A

Acetate

29
Q

An anion with the formula SO₄²⁻, excluding certain salts.

A

Sulfate

30
Q

The specific measurement to be calculated.

A

Desired Quantity

31
Q

Used to calculate concentration of solute.

A

Percent Concentration Formula

32
Q

Solubility of solids increases with temperature.

A

Temperature Effect on Solubility

33
Q

Concentration unit for very small solute amounts.

A

Parts Per Million (ppm)

34
Q

Contains more solute than predicted at temperature.

A

Supersaturated Solution

35
Q

Decreases as temperature increases.

A

Gas Solubility

36
Q

Moles of solute per liter of solution.

A

Molarity (M)

37
Q

Solute with negligible vapor pressure.

A

Nonvolatile Solute

38
Q

Lower than that of pure solvent.

A

Vapor Pressure of Solution

39
Q

Increases when nonvolatile solute is added.

A

Boiling Point Elevation

40
Q

Lower freezing point with nonvolatile solute.

A

Freezing Point Depression

41
Q

Addition of solvent to decrease solute concentration.

A

Dilution

42
Q

Solvent moves through semipermeable membrane.

A

Osmosis

43
Q

Depend on solute concentration, not identity.

A

Colligative Properties

44
Q

Pressure preventing solvent flow into solution.

A

Osmotic Pressure

45
Q

Solutions with equal osmotic pressure.

A

Isotonic Solutions

46
Q

Lower osmotic pressure than body fluids.

A

Hypotonic Solution

47
Q

Higher osmotic pressure than body fluids.

A

Hypertonic Solution

48
Q

Swelling and rupture of red blood cells.

A

Hemolysis

49
Q

Shrinking of cells in hypertonic solution.

A

Crenation

50
Q

Filtering blood through semipermeable membrane.

A

Dialysis

51
Q

Removes waste products from bloodstream.

A

Kidney Function in Dialysis

52
Q

Solute that easily escapes into vapor phase.

A

Volatile Solute

53
Q

Amount of solute in a given volume.

A

Concentration of Solute

Organic and Inorganic Chemistry (3 decks)

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