oria
Uploaded by
12 SLIDES
307 VUES
120LIKES

Understanding Concentration and Dilution of Solutions: Molarity, Calculations, and Examples

DESCRIPTION

This guide explains the concepts of concentration and dilution in solutions. Concentration refers to the amount of solute in a solution, expressed in various units such as molarity (M), parts per million (PPM), and percentages by mass or volume. The relationship between concentrated and dilute solutions is represented by the equation MC × VC = MD × VD, where MC and MD are molarities, and VC and VD are volumes. The document includes practical examples, calculations for diluting solutions, and step-by-step procedures for preparing specific molarity solutions.

1 / 12

Télécharger la présentation

Understanding Concentration and Dilution of Solutions: Molarity, Calculations, and Examples

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. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. TOPIC: Concentrationand DilutionDo Now:

  2. Parts of a Solution • Solute= dissolved substance • Solvent= dispersing medium

  3. We can determine how much solute and solvent make up a solution = CONCENTRATION • Concentration = A measurement that describes how much solute is in a given amount of solvent or solution. • Many, many different units to express concentration. • Molarity • PPM (parts per million) • % by mass • % by volume

  4. Molarity (M) Molarity (M) = moles of solute liters of solution CAN USE THIS TO HELP CALCULATE moles M liters

  5. So why do aqueous solutions need .1M or 3M in front?!?!?!

  6. VS

  7. Dilution-which one has a higher molarity?

  8. Amount of solute is constantAmount of solvent increases Dilution = add water = less concentrated Amount solute in concentrated solution EQUALS Amount solute in dilute solution

  9. MC x VC = MD x VD (C = concentrated D = dilute) MolarityC x VolumeC = MolarityD x VolumeD

  10. 300ml of 2.5M NaOH is diluted to 750ml. Find the molarity of the diluted solution MC x VC = MD x VD 300ml x 2.5M = 750ml x MD So how much water did we have to add to delete the 2.5 M solution? water ?M 750 -300 _ 450ml 1M 2.5M 2.5M 300ml 750ml

  11. Example: We are doing a lab and the procedure calls for 300ml 1.2 M NaOH. However, all we have is a bottle of 5.5M NaOH. We have to dilute it!!!! The Equation: MC x VC = MD x VD 5.5 M x VC = 1.2 M x 300ml V1 = (1.2 M x 300 ml) 5.5 M V1 = 0.065 L = 65 mL So what does 65 ml tell us?!

  12. To prepare the 1.2 M NaOH solution, you pour 65 mL of 5.5 M NaOH into your container and add water to get 300 mL final volume (300-65 = 235 ml water added)

More Related