Environmental Chemistry Lesson # 1

Slides:

Advertisements

Similar presentations

Solution Concentration Concentration = quantity of solute quantity of solution (not solvent) There are 3 basic ways to express concentration: 1) percentages,

Advertisements

Concentration.  Distinguish between dilute and concentrated.  Calculate molarity.  Describe how to prepare solutions of given concentrations.  Calculate.

Concentration of Solutions. Concentrations of Solutions (Section 2.5) Concentration = quantity of solute quantity of solution A solution is dilute if.

Volumetric Analysis Concentration of Solutions. Remember: Solution – A mixture of a solute and a solvent Solvent – The liquid in which the solute is dissolved.

COMMUNICATING CONCENTRATION: Section 5.3.  Most solutions are similar in that they are colorless and aqueous, so there is no way of knowing, by looking.

Molarity and Dilutions

Solutions are homogeneous mixtures consisting of two or more components. The major component of a solution is known as the solvent and the minor component.

Lesson 2.  Concentrations indicate the amount of any substance dissolved in a liquid.  Square brackets, [ ], are often used as an abbreviation for the.

Concentration. Solution Concentration Concentration = quantity of solute quantity of solution There are 3 basic ways to express concentration: 1) Percentages.

Concentration. Differentiate among, and give examples of, the use of various representations of concentration. Include: g/L, % w/w, % w/v, % v/v, ppm,

Solution Concentration. Calculations of Solution Concentration: Mass Percent Mass percent Mass percent is the ratio of mass units of solute to mass units.

Examples-Molarity and Dilutions. Example What is the molarity of a solution that contains 4.5 moles of sucrose in L of water?

Concentration & Consumer Products LG: I can perform concentration calculations involving units commonly used in consumer products.

Solution Concentration Notes

Preparing Solutions LG: I can use formulas for concentration to prepare standard solutions from a solid.

SOLUCIONES. A solution is a homogeneous mixture, at the molecular level, of two or more substances. Simple solutions usually consist of one substance,

Unit 10B Review Reg Chem When a solution sits out over a long period of time and water evaporates the concentration of the solution __________.

Units of Concentration

Solution Concentration Section 14.2 Concentration - amount of solute dissolved in a specific amount of solvent concentrated - a lot of solute dilute.

Preparing a Molar Solution

Concentration/Dilution

AP/IB Chemistry Chapter 4: Aqueous Solutions and Solution Stoichiometry.

Title: Lesson 12 Solutions Learning Objectives: – Understand the relationship between concentration, volume and moles – Pose and solve problems involving.

Solution Concentration

Molarity, Dilution, and pH

Molarity = Molarity ( M ) moles solute liters of solution

DETERMINATION OF AN UNKNOWN DIPROTIC ACID THROUGH VOLUMETRIC ANALYSIS

Section 15.2 Describing Solution Composition 1. To understand mass percent and how to calculate it Objective.

4.4 Solution Concentration and Stoichiometry. Solution Key Terms What type of mixture is also considered a solution? Give an example. – A homogeneous.

III. Molarity Topic 9 The Mole. A. Molarity Concentration of a solution. total combined volume substance being dissolved.

Solutions and Concentration (p )

CHEMISTRY 111/112 Solutions. Solution Formation Solutions are homogeneous mixtures that may be solid, liquid or gaseous The composition of the solvent.

CONCENTRATION OF SOLUTIONS. Solute + The amount of solution can be expressed by: - mass m (g, kg) or - volume V (cm 3, mL, dm 3, L, m 3 ) m = V x  -

Solution Concentrations & Preparation. Defining a Solution Solutions: are __________ mixtures that contain at least one ______ and one _______. Homogeneous.

Ch. 5 - Solutions. A. Concentration The amount of solute in a solution. Describing Concentration % by mass - medicated creams % by volume - rubbing alcohol.

Concentration  A measure of how much solute is dispersed throughout the solvent  Molarity (M), molality (m), and mole fraction ( χ ), mass percent.

Solutions and Concentration (p ) Mr. Hoover, edited by Ms. Bacic

PP & 8.7 Concentration and Preparing Dilutions.

Dilution of Solutions.

Solutions & Solubility Concentration. Concentrations of Solutions Concentration of a solution is a measure of the amount of solute that is dissolved in.

Stock Solutions Different experiments require solutions of various different molarities. It would not be practical to have multiple bottles of each type.

Solutions and Concentrations Notes Page 5. SOLUTIONS A homogenous mixture of two or more substances.

Moles and Solutions - Concentrations

Chemistry 20  concentration: a ratio that compares the quantity of solute to the quantity of solution  A dilute solution has a relatively small quantity.

{ Solutions (1.5) Year 11 DP Chemistry Rob Slider.

Solution Concentration.  Lesson Objectives  Describe the concept of concentration as it applies to solutions, and explain how concentration can be increased.

Molarity & Dilutions. Molarity Concentration – Measure of the amount of solute that is dissolved in a given quantity of solvent Dilute solution – Contains.

Concentration & Consumer Products

Solution Concentration

Introduction to Solutions & Concentration

Molarity (M): State the ratio between the number of moles of solute & the volume of solution (in liters). Molarity (M) =

Solutions and Molarity

Concentration of Solutions

Calculating Concentrations 2

CONCENTRATION OF SOLUTIONS

Introduction to Solutions & Concentration

Molarity & Dilution.

Solution Concentration

Bellwork Friday Draw and finish filling in the mole road map to the right.

Solutions and Solubility

Solution Concentrations

Quantitative Analysis

Concentration & Dilution

Unit A: Chemistry Topic: Calculating Concentrations

Solution Concentration

Concentration of Solutions :

Molarity (M): State the ratio between the number of moles of solute & the volume of solution (in liters). Molarity (M) =

Presentation transcript:

Environmental Chemistry Lesson # 1 Measuring Solutions

Definitions Solution – a homogeneous mixture of two or more substances. Solvent – the substance in which substances are dissolved Solute – the substance(s) being dissolved

Concentration Concentration is the quantity of a given solute in a solution. The more solute, the more concentrated the solution. A solution with little solute is said to be dilute. Concentration can be expressed as a percent or in moles. Concentration = Quantity of Solute Quantity of Solution

Percentage Concentration Percentage concentration means the percentage of solute compared to the total volume of the solution, where the solute can be measured by volume (mL) or weight (g). Volume by volume is %V/V, and weight by weight is % W/W, and weight by volume is % W/V. c = vsolute x 100% or c = msolute x 100% or c = msolute x 100% vsolution msolution vsolution

Example 1 A mixture contains 140 mL of pure acetic acid in a 500 mL bottle of solution. What is the percentage by volume concentration of acetic acid?

Example 2 A hydrogen peroxide solution contains 3 g of H2O2 in every 100 mL of solution. Calculate the percentage weight by volume concentration of the solution.

Example 3 A sterling silver ring has a mass of 12.0 g and contains 11.1 g of pure silver. What is the percentage weight by weight concentration of silver in the metal?

Molar Concentration Molar concentration is the amount of solute, in moles, dissolved in one litre of water. C = amount of solute (in moles) amount of solution (in litres) *Note that C is capitalized to denote a molar quantity, just as molar mass is M, whereas mass is m.

Example 4 A stoichiometric calculation produced 0.186 mol of sodium hydroxide in 0.250 L of solution. Calculate the molar concentration of sodium hydroxide

Example 5 A solution contains 5.85 g of sodium chloride dissolved in 5.00 L of solution. Calculate the molar concentration of sodium chloride.

Example 6 In a solution containing 21.2 g sodium carbonate in 1.50 L of solution, calculate the concentration of the solution.

Example 7 What mass of potassium hydroxide is required to prepare 600 mL of a solution with a concentration of 0.225 mol/L?

Dilution A concentrated standard solution is called a stock solution. Adding water to this solvent decreases the concentration to a desired level, and is known as dilution. For example, hydrochloric acid as a stock solution normally has a concentration of 10 mol/L, whereas what you use in the lab is usually a diluted 1 mol/L solution. Calculating the new concentration or volume required to make a certain solution is straightforward, as the mass or amount of solute does not change, even with the addition of water. Concentration is inversely related to the solution’s volume (concentration decreases with increasing volume, and vice versa). CiVi = CfVf *Where i is the initial concentration and volume (of the stock solution), and f is the final concentration and volume (of the dilute solution)

Example 8 Water is added to 0.200 L of 2.40 mol/L NH3 (aq) cleaning solution, until the final volume is 1.00 L. Find the molar concentration of the final, diluted solution.

Example 9 A student is instructed to dilute some concentrated hydrochloric acid (36%) to make 4.00 L of 10% solution. What volume of hydrochloric acid solution should the student initially measure to do this?