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Chemistry 20: Unit C - Solutions, Acids & Bases > Chapter 5: Solutions > Flashcards

Chapter 5: Solutions Flashcards

1
Q

What’s a solution?

A

Homogeneous mixture

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2
Q

What does a solution include?

A
  • A solute

- A Solvent

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3
Q

What is a Solute?

A

Substance that is dissolved.

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4
Q

What is a Solvent?

A

Substances that does the dissolving.

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5
Q

What is a Homogeneous mixture?

A

It’s when all sections look like one.

Another definition to define homogeneous is uniform composition of solvent and one or more solutes.

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6
Q

What is a Heterogeneous mixture?

A

It’s when a mixture in which the components can be seen.

Another definition to define heterogeneous is the composition of components varies throughout the mixture

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7
Q

What is an Aqueous Solution?

A

It is when they have water as the solvent.

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8
Q

What is an Electrolyte?

A

Substances which dissolve in water to form solutions that conduct electric current.

Another definition to define Electrolyte is if its aqueous solution or molten state is able to conduct electricity.

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9
Q

Does electrolytes break in cations and ion form to allow current to flow?

A

Yes

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10
Q

What is an Non-Electrolyte?

A

Substances which dissolve in water and don’t conduct electric current.

Another definition to define Non-Electrolyte is if it does not conduct electricity.

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11
Q

Does non-electrolytes have no ions and no current flows?

A

Yes

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12
Q

What are Molecular Acids?

A

Capable of conduct electricity because some of the molecules break into the hydronium ion and anion.

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13
Q

Why is water important?

A
  • It is the universal solvent.
  • It has the ability to dissolve many different ionic compounds and some polar molecular compounds.
    This happens because water is a polar compound.
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14
Q

What happens for intramolecular bonds? (Ionic Compound)

A

The bonds of the compound break and separate into their cation and anion forms.

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15
Q

What happens for intermolecular bonds? (Polar Molecule)

A

The bonds of the molecule break and separate then disperse.

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16
Q

What is the dissociation (ionization) equation?

A

It is something which demonstrates the separation of an ionic compound that dissolves in water.

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17
Q

What is Dissociaton?

A

It describes the separation that happens when an ionic compound dissolves.

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18
Q

What is Ionization?

A

It is when a neutral atom or molecule is converted to an ion.

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19
Q

What are the 2 requirements of dissociation or ionization?

A
  1. Compound must be ionic.

2. Compound must be soluble in water.

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20
Q

What are Acids?

A

Substances which ionize in water to form hydrogen ions.

They are responsible for the acidic properties.

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21
Q

What are Bases?

A

Substances which ionize-dissociate in water to form hydroxide ions.

They are responsible for the basic properties.

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22
Q

What are the Properties of Acids?

A
  • Taste sour.
  • pH less than 7.
  • They react with active metals (group 1) to manufacture hydrogen gas.
  • They neutralize bases.
  • They turn litmus red.
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23
Q

What are the Properties of Bases?

A
  • Taste bitter.
  • pH greater than 7.
  • Feel slippery to the touch.
  • They neutralize acids.
  • They turn litmus blue.
24
Q

What is Endothermic?

A

They absorb heat.

Reaction or system absorbs (takes in) energy from its surroundings.

Temperature of the surroundings decrease.

System obtains or gets energy and the surroundings lose.

Processes that requires energy.

25
Q

Which uses energy to break bonds between

reactants?

A

Endothermic

26
Q

When energy is released which creates new bonds?

A

Exothermic

27
Q

What is Exothermic?

A

They release heat.

Reaction or system releases (gives off) energy to its surroundings.

Temperature of the surroundings increase.

System loses energy and surroundings get.

Processes that release energy.

28
Q

What is an Endothermic Reaction?

A
  • More energy absorbed than released.
  • More energy absorbed to break bonds compared to quantity of energy released to form bonds.
  • Reaction where there is more energy absorbed to break the bonds of the reactants compared to the amount of energy released when creating the new bonds of the products.
29
Q

What is Exothermic Reaction?

A
  • More energy released than absorbed.
  • More energy released when forming bonds then was absorbed when breaking bonds.
  • Reaction where there is more energy released when making the bonds of the products then was absorbed when breaking the bonds of the reactants.
30
Q

What 2 things happens during a solution?

A

Chemicals - more easily handled.

Carrying out reactions - more controllable.

31
Q

Important Thing to Know

A

For a reaction to take place collisions must occur or happen between the reactant atoms, ions or molecules involved.

32
Q

I think a Thing to Know

A

In a solution a much greater number of collisions can therefore happen and the reaction can proceed faster and more efficient pace.

33
Q

What is Concentration?

A

A measure of the amount of solute compared to the amount of solvent.

34
Q

How can solutions be described?

A

They can be described as concentrated and diluted.

35
Q

Includes a large portion of solute compared to another solution. What is this?

A

Concentrated

36
Q

Includes a small portion of solute compared to another solution. What is this?

A

Diluted

37
Q

What is Parts per Million (ppm)?

A
  • Very dilute solutions.

- Mass of a solute present in a million units of mas of a he solution.

38
Q

What is Molar Concentration?

A

An SI unit expressing concentration as moles per litre of solution. (mol/L)

39
Q

What is Dilution?

A

A solution can be made less concentrated by simply adding more solvent.

40
Q

What is Solubility?

A

The amount of a substance that dissolves in a given amount of solvent at a given temperature to produce a saturated solution.

41
Q

What is a Saturated Solution?

A

A solution in which no additional solute will dissolve, at a specific temperature.

42
Q

What does a Saturated Solution contain?

A

It contains both a dissolved and undissolved solute.

43
Q

What is Crystallization?

A

The opposite (reverse) of dissociation.

44
Q

When does equilibrium happen?

A

When the rate of dissociation and crystallization are the same

45
Q

Does Pure Elements have a low solubility in water or high?

A

Low Solubility

46
Q

Does solids (compounds) have a high solubility or low?

A

High Solubility

47
Q

Which liquid dissolve completely in water in any proportion? Also which liquid is said to be miscible with water?

A

Polar liquids

48
Q

Which liquid doesn’t dissolve in water to any extent? Also which liquid is said to be immiscible with water?

A

Nonpolar liquids

49
Q

Is this statement correct? Diluting a solution DOES NOT change the # of moles of solute originally in the solution.

A

Yes

50
Q

To prepare a standard solution what are the rules?

A
  1. Collect the mass of solute using the electronic balance.
  2. Dissolve the mass in 40 mL to 50 mL of dissolved water.
  3. Transfer the contents from the beaker into the volumetric flask and then add distilled water to the flask until the 100 mL is reached.
51
Q

What are the ways to prevent and clean up acid and base spills?

A
  1. Dilute it - adding water decreases the concentration of hydronium and hydroxide - not prepared
  2. Neutralize it - adding a weak acid or base to react and produce salt and water - best practice
52
Q

What is the Neutralization equation?

A

acid + base = salt + water

53
Q

What is Neutralization Reaction?

A
  • It involves hydronium and hydroxide ions reacting to form water.
  • Since the only products are salt and water, the substances do not have acidic or basic properties.
54
Q

What is the meaning of Acid-Base Indicators?

A

It is when some chemicals change when placed in an acid or a base.

55
Q

What is the Generic symbol for indicators?

A

ln

56
Q

What is the Generic formula for indicators in the acid form?

A

Hln

Chemistry 20: Unit C - Solutions, Acids & Bases (4 decks)

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