Solution. Solute. Solvent. homogeneous mixture; consists of solutes dissolved in a solvent. Dissolved particles; substance that is dissolved.



Solution

› homogeneous mixture;

consists of solutes dissolved in a solvent.



Solute

› Dissolved particles;

substance that is dissolved.



Solvent

› Substance in which

particles are dissolved.

 Solutions are always made up of a solvent and solute.

 The solvent is usually the substance in the greater quantity.

 Solutes and solvents can be gases, liquids, or solids.



Soluble: “will dissolve in”



Example: Salt and water



Insoluble: “will NOT dissolve”



Example: Sand and water

1) Gas-liquid solute-solvent.

› Example: Carbon dioxide gas is mixed with liquids.

› 2) Solid-liquid solute-solvent.

Example: Sweetened Hot tea- sugar and tea..

alloy

Pewter = 80% tin + 20% copper

Tin

Copper

What is the solvent?

What is the solute?

Copper

Tin

There’s more solvent than solute…

The larger amount is the solvent

Brass = Copper + Zinc Copper Zinc

What is the solvent?

Copper What is the

solute? Zinc

The solute is dissolved in

the solvent…

There is more

solvent than

solute…

24 karat gold 18 karat gold 14 karat gold Gold

Copper Silver

18/₂₄ atoms Au

24/₂₄ atoms Au ¹⁴/₂₄ atoms Au

What is the

solvent? Gold

What are the solutes?

Copper

and silver



Example: NaCl

dissolved in water.

› Which is the solute?

› Which is the solvent?

› What type of solute-solvent

combination is this?



Water that contains dissolved substances



Indicated by (aq)



Water is the universal solvent.

› Because it dissolves more substances

than any other liquid.



Hard Water

› Water that has high mineral content.

› Mixture of water and minerals such as

calcium, iron and magnesium

› Which is the solute?

› Which is the solvent?

› Think about minerals in your shower!



Amount of solute that dissolves in a given amount of solvent at a given temperature.



Max solubility- No more solute

can dissolve.

Solids dissolved Gases dissolved

in liquids in liquids

T^o Sol.

T^o Sol.

As T^o ,

solubility ___ As T^o ,

solubility ___

[O₂]

1. temperature of solvent

2. surface area of solute

3. stirring

the solution With more stirring,

rate

As temp. , rate

As size ,

rate

Concentration…a measure of solute-to-solvent ratio

concentrated dilute

Add water to dilute a solution; boil water off to concentrate it.

“lots of solute” “not as much solute”

“watery”

“not much solvent”

Saturated Solution:

Rock candy can be produced from

a saturated solution of sugar

water.

A solution that contains the maximum amount of solute for a certain

amount of solvent



Solutions Video

REMEMBER

ME ??????

I’M BAAACK !!!!!

moles of solute Molarity

liters of solution



Molarity: measurement of solution concentration

the amount of solute, in moles, dissolved in a liter of solvent

Units of concentration for solutions

molarity (M) = moles per liter

L mol

M 

1 Liter = 1000 mL Grams  Moles

Use Molar Mass

Determine the molarity of a solution containing 1 mol of HCl in 1 Liter of water.

L mol

M 

Calculate the molarity of a solution that contains 0.5 mol of NaCl in 1.5 L of water.

0.5 moles 1.5 liters

M = = 0.33M

Determine the molarity of a solution made by

dissolving 2 moles of HCl in 1500 milliliters of water.

2 moles 1.5 liters

M = = 1.33M

1 moles 1 liters

M = = 1M

1500 mL x 1 liter

1000 mL = 1.5 L

How many moles of HCl are there in 1 liter of a 3 M HCl solution?

L mol

M 

x moles 1 Liter 3 M =

x moles = (3 M)(1 Liter) = 3 moles HCl

Determine the volume of a solution containing 0.5 moles of HCl if its concentration is 2M.

2 M = 0.5 moles X Liters

(2 M)(X Liters) = 0.5 moles

X Liters 1

X Liters 1

2M 2M = 0.25 moles

Na¹⁺

How many moles of sodium hydroxide are needed to make1.35 L of a 2.5 M solution?

How many grams of sodium hydroxide are there in 3.38 mol?

Mol = M * L = 2.5 M (1.35 L )

= 3.38 mol



 





mol

1

g

3.38 mol 40.0 = 135 g NaOH OH^1– NaOH

L mol

M 

What is the molar mass of NaOH?

How many mol magnesium phosphate are needed to make 1.35 L of 2.50 M solution?

How many grams of magnesium phosphate are there in 3.38 mol?

mol = M*L = 2.50 M (1.35 L )

= 3.38 mol

Mg²⁺



 





mol

1

g 262.9

3.38 mol = 889 g Mg₃(PO₄)₂

PO₄^3– Mg₃(PO₄)₂

L mol

M 

What is the molar mass of Mg

(PO

)

?

Find molarity of a barium hydroxide solution if 58.6 g barium hydroxide are in 5.65 L of the

solution.

L mol

M 



 





g 171.3

mol

58.6 g 1

Ba

OH

Ba(OH)

= 0.342 mol

L 5.65

mol 0.342

 = 0.061 M Ba(OH)₂

What is the molar mass of Ba(OH)

?

L mol

M 

You have 10.8 g potassium nitrate. How many mL of solvent are needed to make a 0.14 M solution of Potassium nitrate?

K¹⁺ NO₃^1–

KNO₃



 





g 101.1

mol

10.8 g 1 = 0.1068 mol

M mol

L 

M 0.14

mol 0.1068

 _{= 0.763 L }



 





L 1

mL 1000

(convert to mL)

= 763 mL What is the molar mass of KNO₃?

L mol

M 