Solubility Unit 4 Flashcards

1
Q

What are solutions composed of

A

Solute and solvent

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2
Q

Solute

A

Substance that is dissolved

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3
Q

Solvent

A

Substance that does the dissolving

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4
Q

Saturated solution

A

A solution that cannot dissolve additional solute under normal conditions

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5
Q

Super saturated solution

A

A solution that has dissolved more solute than normal after conditions have been changed

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6
Q

Soluble

A

If more than 1g of solute is dissolved per 100g of solvent

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7
Q

Not soluble

A

If less than 0.1g of solute dissolves per 100mL H2O

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8
Q

Slightly soluble

A

When between 0.1-1g of solute dissolves per 100mL of H2O

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9
Q

Molarity and symbol

A

_M

The moles of solute per 1L of solution

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10
Q

Molarity equation

A

=moles of solute
L of solution

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11
Q

Ppm
Ppb

A

Parts per million
Parts per billion

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12
Q
A
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13
Q

Molality

A

Moles of solute/kg of solvent

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14
Q

Turn 3ppm of AgCl to moles

A
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15
Q

Concentration of 0.015M AgCl2 in ppm

A
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16
Q
A
17
Q

Ksp

A

Solubility product constant

18
Q

Ksp definition

A

The equilibrium constant for the dissolving of a solid in H2O

19
Q

Ksp expression for CaCl2

A

(Ca+2). (Cl-)2

20
Q

What does ksp indicate

A

How much solute is dissolved

The larger the ksp the more soluble a substance is

21
Q
A
22
Q

Molarity triangle and moles triangle

A
23
Q

What does ksp tell us

A

How many ions can be in the solution before ppt forms

24
Q

Ksp= (A+) (B-)

A

Saturated

25
Q

Ksp> (A+) (B-)

A

Unsaturated

26
Q

Ksp< (A+) (B-)

A

Super saturated/ppt forms

27
Q

Find MAX solution

A
28
Q

When does ppt form

A

When the ion product (A+) (B-) is greater than the ksp value

29
Q

When can you predict if ppt forms

A

When 2 solutions are mixed together

30
Q
A
31
Q

Selective precipitation

A

Removing a specific ion from a mixture of ions

32
Q

Example of selective precipitation

A
33
Q

Spectator ions

A

Ions that don’t participate

34
Q

Net ionic equation example

A