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Perryland Chemistry - Theory (2005 Standards) > Unit 8 - Solutions > Flashcards

Unit 8 - Solutions Flashcards

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1
Q

What is the solubility of Potassium Nitrate at 50 C?

A

86 g Potassium Nitrate

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2
Q

Is the solution unsaturated, saturated, or supersaturated, if I have 30 g of Potassium Nitrate in 100 g of Water at 30 C?

A

Unsaturated

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3
Q

Is the solution unsaturated, saturated, or supersaturated, if I have 60g of Potassium Nitrate in 100g of Water at 30 C?

A

Supersaturated

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4
Q

How much solute will not dissolve if I have 80g of Potassium Nitrate in 100g of Water at 30C?

A

35g Potassium Nitrate

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5
Q

How much more solute could I dissolve if I have 10g of Potassium Nitrate in 100g of Water at 30C?

A

~32g of Potassium Nitrate

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6
Q

How much solute would crystallize out of solution once a solution of 85g of Potassium Nitrate in 100g of Water at 50C is cooled to 20C?

A

55g Potassium Nitrate

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7
Q

Molarity

A

Expressions of Concentration ( [] )

The amount of a component in a given area or volume.

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8
Q

Solute

A

The component being dissolved.

The component in the smallest amount.

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9
Q

Solvent

A

The component doing the dissolving.

The component in the largest amount.

Water is the universal solvent.

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10
Q

Concentrated

A

A relatively large amount of solute.

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11
Q

Dilute

A

Relatively small amount of solute.

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12
Q

Solution

A

Solute + Solvent

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13
Q

How to determine if a solution is unsaturated, saturated, or supersaturated.

A

Add more solute and observe the results.

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14
Q

Unsaturated

A

Contains less solute than it can at that temperature.

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15
Q

Saturated

A

Contains as much solute as it can at that temperature.

If you add more solute it will not dissolve.

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16
Q

Supersaturated

A

Contains more solute than it should at that temperature. Ussually the solution is heated to allow that much solute to dissolve and then cooled back down.

If you add solute to a supersaturated solution the “super” part (amount over the saturation point) will crystallize out of solution.

17
Q

Solubility Curve

A

Used to determine the mass of solute in 100g (100ml) of water at a given temperature.

18
Q

Molarity

A

M

19
Q

What is the molarity of a solution made by dissolving 2.5g of NaCl in enough water to make 125 ml of solution?

A
20
Q

Percent Mass

A
21
Q

Calculate the concentration of the solute in the diluted solution: 1.00mL of 0.50M NH4Cl diluted to 250.0mL

A

M1V1 = M2V2

M1 = (M2V2)/(V1)

M1 = (0.5 M x 1 ml)/(250 ml)

M1 = 0.0020M

22
Q

Calculate the volume required to prepare the diluted solution: Given 6.0M NaOH; need 5.0L of 0.10M NaOH.

A

M1V1 = M2V2

V1 = (M2V2)/(M1)

V1 = 0.083L

23
Q

What is the molarity of a solution in which 58 g of NaCl are dissolved in 1.0 L of solution?

A

1.0 M

24
Q

What is the molarity of a solution in which 10.0 g of AgNO₃ is dissolved in 500 ml of solution?

A

0.118 M AgNO₃

25
Q

How many grams of KNO₃ should be used to prepare 2.00 L of a .500 M solution?

A

101 g KNO₃

26
Q

To what volume should 5.0 g of KCl be made in order to prepare a .25 M solution?

A

0.27 L KCl

27
Q

Colligative Properties

A

properties that depend on the concentration of solute, but not on the chemical identity of the solute.

(Vapor Pressure Lowering, Boiling Point Elevation, Freezing Point Depression, and Osmotic Pressure)

28
Q

“Like Dissolves Like”

A

Not everything will dissolve in everything. Polar solvents dissolve polar solutes. Nonpolar solutes dissolve nonpolar solutes. Water is polar so it dissolves polar solutes.

29
Q

The Dissolving Process

A
  1. The solvent surrounds the outer surface of the solute.
  2. Individual Solute Ions are “stripped” away from the surface due to their attraction to the solvent particles.
  3. This exposes more particles to the solvent and thus the process continues.
30
Q

How can you make things dissolve faster?

A
  1. Agitation (stirring)
  2. Temperature
  3. Increase Surface Area (Grind or Crush)

Perryland Chemistry - Theory (2005 Standards) (13 decks)

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