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solubility Flashcards

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1
Q

Define Matter.

A

Anything that takes up space and has mass.

Matter is the substance of which physical objects are made.

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2
Q

Define Mass.

A

A property of an object that measures the amount of matter it contains.

Mass is often measured in grams or kilograms.

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3
Q

Describe the difference between Quantitative and Qualitative Properties.

A
  • Quantitative Properties: Numerical factors that are affected
  • Qualitative Properties: Physical descriptions about appearance

Quantitative properties can be measured, while qualitative properties are observed.

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4
Q

What are Physical Properties?

A

A property that can be seen or measured without changing a chemical property.

Examples include color, texture, and state.

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5
Q

What are Chemical Properties?

A

A characteristic of a substance that can only be observed or measured during a chemical reaction.

Examples include flammability and reactivity.

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6
Q

Give examples of Physical Properties.

A
  • Color
  • Texture
  • Feel
  • Transparency
  • State (liquid, solid, gas)

These properties can be observed without altering the substance.

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7
Q

Give examples of Chemical Properties.

A
  • pH
  • Solubility
  • Flammability
  • Toxicity
  • Reactivity
  • Melting point

These properties are observed during a chemical change.

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8
Q

Name three properties to differentiate Salt and Sugar.

A
  • Taste
  • Solubility
  • Melting point

These properties can help identify each substance.

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9
Q

Describe the difference between Mass and Volume.

A
  • Mass: Measures the amount of matter in an object
  • Volume: The space an object takes up

Mass is measured in grams, while volume is measured in liters or cubic centimeters.

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10
Q

How would you measure the mass of a red/brown metal rod?

A

Directly with a scale or indirectly by multiplying volume by density.

Direct measurement is preferred for accuracy.

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11
Q

How would you measure the mass of salt?

A

Using a graduated cylinder to measure the weight of the salt indirectly.

Subtract the weight of the empty cylinder from the full weight.

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12
Q

How would you measure the volume of a wooden block?

A

Directly by measuring length, width, and height, then multiplying them.

This gives the volume in cubic centimeters.

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13
Q

How would you measure the volume of a red/brown metal rod?

A

Indirectly by measuring water displacement in a graduated cylinder.

The rise in water level indicates the volume of the rod.

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14
Q

What is the formula for Density?

A

Density = mass / volume

Density is expressed in units such as kg/m³ or g/cm³.

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15
Q

If you put copper and aluminum in water, which will sink?

A
  • Copper
  • Aluminum

Both have densities greater than water.

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16
Q

If you put oak and Styrofoam in water, which will float?

A
  • Oak
  • Styrofoam

Both have densities less than water.

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17
Q

What is the order of liquid layers from top to bottom when mixing ethyl alcohol, vegetable oil, and seawater?

A
  • Ethyl alcohol
  • Vegetable oil
  • Seawater

This order is based on their respective densities.

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18
Q

What is the density of carbon dioxide gas if 0.196 g fills a volume of 100 mL?

A

0.00196 g/mL

Calculated by dividing mass by volume.

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19
Q

What is the density of a block of wood with a mass of 27 g and dimensions of 3.0 cm on each side?

A

1 g/cm³

Volume is calculated as 3x3x3=27 cm³.

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20
Q

What is the difference between a chemical change and a physical change?

A
  • Physical change: Does not depend on a chemical reaction
  • Chemical change: Depends on a chemical reaction

Physical changes can often be reversed, while chemical changes cannot.

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21
Q

Give three examples of Chemical Changes.

A
  • Oxidation
  • Combustion
  • Rotting

These processes involve a change in the substance’s chemical structure.

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22
Q

What is the Law of Conservation of Mass?

A

Mass cannot be created or destroyed in a chemical reaction.

Important for understanding chemical reactions and balancing equations.

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23
Q

Define Pure Substances.

A

A substance by itself that has not been mixed with anything.

Pure substances have consistent properties throughout.

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24
Q

Define Mixtures.

A

A type of matter made up of two or more substances that are physically combined.

Mixtures can be homogeneous or heterogeneous.

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25
What is a **Homogeneous Substance**?
A mixture that is the same throughout and cannot be easily separated. ## Footnote Examples include solutions like saltwater.
26
What is a **Heterogeneous Substance**?
A mixture that can be easily separated and visually distinguished. ## Footnote Examples include salad or sand and salt.
27
What is an **Element**?
A pure substance that cannot be broken down into simpler substances. ## Footnote Elements are the building blocks of matter.
28
What is a **Compound**?
A mix of elements that are combined chemically. ## Footnote Compounds have different properties than the elements that compose them.
29
What is a **Solution**?
A homogeneous mixture where one substance is completely dissolved in another. ## Footnote Solutions are uniform in composition.
30
What is a **Suspension**?
A heterogeneous mixture where solid particles are mixed into a liquid but do not dissolve. ## Footnote Suspensions can settle over time.
31
What is a **Mechanical Mixture**?
A heterogeneous mixture where different parts can be seen. ## Footnote Examples include a mixture of sand and pebbles.
32
What are the **4 points of the Kinetic Molecular Theory**?
* All matter is made up of small particles called molecules * Molecules are constantly moving * Forces of attraction exist between particles * There are spaces between particles ## Footnote This theory explains the behavior of solids, liquids, and gases.
33
What happens to the total volume when mixing equal amounts of **methanol** and **water**?
It is not twice the volume because particles fit into each other. ## Footnote This is similar to marbles fitting into sand.
34
What is **pH**?
A scale to measure if something is an acid or a base. ## Footnote pH levels indicate acidity or basicity.
35
What is special about **red cabbage** as a pH indicator?
It contains anthocyanin, a pigment that changes color in response to acidity. ## Footnote This makes it useful for testing pH levels.
36
What are some **acid substances**?
* Vinegar * Hydrochloric acid * Nitric acid * Boric acid * Carbonic acid ## Footnote These substances have a pH below 7.
37
What are some **neutral substances**?
* Water ## Footnote Neutral substances have a pH of 7.
38
What are some **base substances**?
* Sodium hydroxide * Potassium hydroxide * Calcium hydroxide * Baking soda * Bleaching powder ## Footnote These substances have a pH above 7.
39
What does **solubility** test for?
Whether a substance dissolves in water. ## Footnote Soluble substances will mix with water, while insoluble will not.
40
What does **iodine** test for?
Presence of starch. ## Footnote Iodine turns blue-black in the presence of starch.
41
What does **vinegar** test for?
Presence of a base. ## Footnote Vinegar is an acid and reacts with bases.
42
What does a **positive reaction** indicate when testing for water?
Substance dissolves = soluble Substance does not dissolve = insoluble ## Footnote Soluble in water and insoluble in water are key terms in solubility.
43
What color does iodine turn in the presence of **starch**?
Golden brown liquid (iodine) turns black ## Footnote When iodine is dropped on bread, the iodine solution turns blue-black.
44
What is released when **vinegar** reacts with a base?
Gas is released (bubbles form) ## Footnote Example: Vinegar in baking soda will bubble.
45
What happens to **red litmus paper** in a base?
Turns blue ## Footnote Red litmus paper: baking soda = blue.
46
What happens to **blue litmus paper** in an acid?
Turns red ## Footnote Blue litmus paper: vinegar = red.
47
What does **pH paper** indicate?
Colour changes for each range of pH ## Footnote Used for testing pH in pools and/or fish tanks.
48
What color does **red cabbage juice** turn in an acid?
Red-pink ## Footnote Changes color depending on the pH of a substance.
49
What is the expected observation for **baking soda** in the solubility test?
Dissolves ## Footnote Expected to show no reaction in vinegar and very dark in iodine test.
50
What is the expected observation for **corn starch** in the iodine test?
Very dark ## Footnote Expected to show no reaction in vinegar and no color change.
51
What is the expected observation for **chalk** in the solubility test?
Nonsoluble ## Footnote Expected to show no reaction in vinegar and no color change.
52
What is the definition of **concentrated**?
In solution- a large mass of dissolved solute for a certain quantity of solvent ## Footnote This term describes the strength of a solution.
53
What is the definition of **solubility**?
The mass of a certain solute that can be dissolved in a certain volume or mass of solvent, at a certain temperature ## Footnote This term is crucial for understanding how substances interact in solutions.
54
What is the definition of **unsaturated**?
A solution that is not yet saturated- more solute can be added ## Footnote Indicates that the solution can still dissolve more solute.
55
What is the definition of **saturated**?
A solution in which no more of a solute will dissolve in a specific amount of solvent ## Footnote Even with plenty of stirring, no additional solute can dissolve.
56
What does **soluble** mean?
Able to dissolve in a particular solvent ## Footnote This term describes the property of a substance in relation to a solvent.
57
What is a **solute**?
A substance that can be dissolved in a solvent to form a solution ## Footnote The solute is the component that is dissolved.
58
What is a **solvent**?
A substance into which a solute dissolves to form a solution ## Footnote The solvent does the dissolving.
59
What does **super saturated** mean?
Heating a solvent to be able to add more solute to a saturated solution ## Footnote This process allows for more solute than normally possible at a given temperature.
60
What does **dilute** mean?
In solution- small mass of dissolved solute for a certain quantity of solvent ## Footnote This term indicates a weaker concentration of solute.
61
What is **concentration**?
Quantity of solute that is dissolved in a certain quantity of solvent ## Footnote This term is important for understanding the strength of a solution.
62
What does **insoluble** mean?
Unable to dissolve in a particular solvent ## Footnote This term describes substances that do not interact with a given solvent.
solubility
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