Dilution solution
Download
1 / 36

Dilution Solution - PowerPoint PPT Presentation


  • 56 Views
  • Uploaded on

Dilution Solution. Solution Dilution. What’s the “concentration” of red triangles?. 500 mL. 10 M 5 M. What’s the “concentration” of red triangles?. 500 mL. 10 10 All of the above. 1 g. 1 g. 1 g. 1 g. 1 g. Concentration is….

loader
I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
capcha
Download Presentation

PowerPoint Slideshow about ' Dilution Solution' - merry


An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
Dilution solution

Dilution Solution

Solution Dilution



What s the concentration of red triangles1
What’s the “concentration” of red triangles?

500 mL

10

10

All of the above

1 g

1 g

1 g

1 g

1 g


Concentration is
Concentration is…

…any statement of the relationship between the amount of stuff (“solute”) dissolved in a solvent/solution.



Units units units
UNITS! UNITS! UNITS!

The units are your friend – ALWAYS! The units tell you how to measure your “stuff”.

So, if I’ve got Molarity (M), I probably want to measure the volume…


If i have
If I have…

Then I want to measure…

GRAMS of solution!


Concentration is always just a conversion factor between the way you measured the solution and how much solute you’ve got!

The SOLUTE is almost always the thing you care about. The solvent/solution is just the carrier.


When you mix things
When you mix things… way you measured the solution and how much solute you’ve got!

…you “dilute” them.

But the concentration is still just the ratio of the amount of solute and the amount of solution.


If i add 1 l of water
If I add 1 L of water way you measured the solution and how much solute you’ve got!

1 g

1 g

500 mL

1 g

1 g

1 g

1 L


Volumes add. way you measured the solution and how much solute you’ve got!

Pick your favorite concentration unit:

Etc.

Chemistry is all about

MOLES! MOLES! MOLES!

So something like Molarity is usually our fav

1500 mL

1 g

1 g

1 g

1 g

1 g


This is true whenever i mix things
This is true whenever I mix things way you measured the solution and how much solute you’ve got!

2g

2g

1 g

1 g

2g

2g

2g

1 L

500 mL

1 g

2g

2g

2g

1 g

1 g

10

8


If i mix them
If I mix them… way you measured the solution and how much solute you’ve got!

2g

2g

2g

2g

2g

The concentration is…?

Etc.

2g

2g

2g

1500 mL

1 g

1 g

1 g

1 g

1 g


It s tough when they are invisible
It’s tough when they are invisible… way you measured the solution and how much solute you’ve got!

…so make them visible.

A picture paints 1000 words (…so why can’t I paint you?).

If you can draw it so you can see it, it makes pretty good common sense.


50 mL of 0.215 M Na way you measured the solution and how much solute you’ve got!2SO4 is mixed with 200 mL of 0.500 M PbSO4. What is the concentration of Na2SO4 after mixing?

I think I’ll draw a picture!


This is true whenever i mix things1
This is true whenever I mix things way you measured the solution and how much solute you’ve got!

200 mL

50 mL

0.215 M Na2SO4

0.5 M PbSO4


It s a question of how many there are
It’s a question of how many there are… way you measured the solution and how much solute you’ve got!

MOLES IS NUMBER!

But how many “moles” do I have?

0.01075 mol

250 mL


M is just a conversion factor
M is just a conversion factor way you measured the solution and how much solute you’ve got!

Notice I multiply 50 mL by the concentration not 250 mL.

Why? (you may ask)

Because the concentration applied to THAT solution.


This is true whenever i mix things2
This is true whenever I mix things way you measured the solution and how much solute you’ve got!

250 mL

50 mL

0.215 M Na2SO4


Conservation of moles
Conservation of moles… way you measured the solution and how much solute you’ve got!

In general, there’s no such thing. But in a dilution there is…

Moles at the beginning = moles at the end!

It’s just the volumes that change.


Plug and chug
Plug and chug way you measured the solution and how much solute you’ve got!

This sometimes gets written in algebraic form:

M1V1= M2V2

Or sometimes

C1V1=C2V2

It still boils down to:

Moles in “solution 1” = Moles in “solution 2”


Plug and chug1
Plug and chug way you measured the solution and how much solute you’ve got!

This sometimes gets written in algebraic form:

M1V1= M2V2

Notice that the Molarity of a solution is coupled with the volume of that solution.


That s why the 0 215 m goes with the 50 ml that s the solution that has that concentration
That’s why the 0.215 M goes with the 50 mL – that’s the solution that has that concentration.

250 mL

50 mL

0.215 M Na2SO4


0.215 M Na the solution that has that concentration.2SO4 (50 mL) = M2 (250 mL)

M2=0.043 M Na2SO4


That s why the 0 215 m goes with the 50 ml that s the solution that has that concentration1
That’s why the 0.215 M goes with the 50 mL – that’s the solution that has that concentration.

250 mL

50 mL

0.215 M Na2SO4

0.043 M Na2SO4


The units must cancel
The units must cancel… the solution that has that concentration.

…but it doesn’t matter what they are…

C1V1 = C2V2

As long as the “C”s are in the SAME units and the “V”s are in the SAME units, everything is fine.


Question
Question the solution that has that concentration.

When 50.00 mL of 0.125 M silver (I) nitrate is mixed with 50.00 mL of 0.250 M sodium sulfate a greyish solid forms. If I recover 0.813 g of solid, what is the yield of the reaction?


Limiting reactant problem
Limiting reactant problem the solution that has that concentration.

How do I know?

I have limited amounts of each reactant.

When 50.00 mL of 0.125 M silver (I) nitrate is mixed with 50.00 mL of 0.250 M sodium sulfate a greyish solid forms. If I recover 0.813 g of solid, what is the yield of the reaction?

Where do I start?


Always a balanced equation
ALWAYS A BALANCED EQUATION! the solution that has that concentration.

When 50.00 mL of 0.125 M silver (I) nitrate is mixed with 50.00 mL of 0.250 M sodium sulfate a greyish solid forms.

AgNO3 (aq) + Na2SO4(aq) → ???

What type of reaction is this?

Double replacement – two ionic reactants!


Always a balanced equation1
ALWAYS A BALANCED EQUATION! the solution that has that concentration.

AgNO3 (aq) + Na2SO4(aq) → Ag+ + NO3- + Na+ + SO42-

AgNO3 (aq) + Na2SO4(aq) → Ag2SO4 + NaNO3

2 AgNO3 (aq) + Na2SO4(aq) → Ag2SO4 + 2 NaNO3

2 AgNO3 (aq) + Na2SO4(aq) → Ag2SO4(s) + 2 NaNO3 (aq)


2 agno 3 aq na 2 so 4 aq ag 2 so 4 s 2 nano 3 aq
2 AgNO the solution that has that concentration.3 (aq) + Na2SO4(aq) → Ag2SO4 (s) + 2 NaNO3 (aq)

When 50.00 mL of 0.125 M silver (I) nitrate is mixed with 50.00 mL of 0.250 M sodium sulfate a greyish solid forms. If I recover 0.813 g of solid, what is the yield of the reaction?

These numbers don’t compare! Apples and oranges.

It’s not how much you have, it’s how much you need.


2 agno 3 aq na 2 so 4 aq ag 2 so 4 s 2 nano 3 aq1
2 AgNO the solution that has that concentration.3 (aq) + Na2SO4(aq) → Ag2SO4 (s) + 2 NaNO3 (aq)

These numbers compare!

The silver nitrate runs out first!


2 agno 3 aq na 2 so 4 aq ag 2 so 4 s 2 nano 3 aq2
2 AgNO the solution that has that concentration.3 (aq) + Na2SO4(aq) → Ag2SO4 (s) + 2 NaNO3 (aq)

This is the “theoretical yield” – what I get if everything goes perfectly. In this reaction, it didn’t!


I only got 0 813 g of product
I only got 0.813 g of product! the solution that has that concentration.

When 50.00 mL of 0.125 M silver (I) nitrate is mixed with 50.00 mL of 0.250 M sodium sulfate a greyish solid forms. If I recover 0.813 g of solid, what is the yield of the reaction?


ad