7 concentration part d
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This document discusses different ways to express the concentration of a solution. There are three main types: percentages, parts per million (ppm) and parts per billion (ppb), and molar concentrations. Percentages can be expressed as % volume/volume, % mass/mass, or % mass/volume. Ppm and ppb are used for very low concentrations and relate to parts per million or billion. Molar concentrations express the moles of solute per liter of solution. Calculations are provided for converting between these different concentration units.
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20 concentration of solutions
- Concentration can be expressed in several ways including mass/volume percent, mass/mass percent, volume/volume percent, parts per million (ppm), and molar concentration (mol/L).
- Mass/volume percent is the mass of solute divided by the volume of solution. Volume/volume percent is the volume of solute divided by the volume of solution.
- Mass/mass percent is the mass of solute divided by the mass of solution. Parts per million (ppm) and parts per billion (ppb) express very small concentrations.
- Molar concentration expresses the number of moles of solute per liter of solution and is the standard unit for expressing concentration in chemistry
2 concentration of solutions
This document defines and provides examples for different ways of expressing the concentration of solutions, including mass/volume percent (m/v%), mass/mass percent (m/m%), volume/volume percent (v/v%), parts per million (ppm), parts per billion (ppb), and molar concentration (mol/L). It also discusses how to calculate concentration using the various units and provides examples of dilution calculations.
5.3.1
This document discusses various concepts related to concentration and molarity including:
- Molarity is a measure of the amount of solute dissolved in a solvent and is expressed as moles of solute per liter of solution.
- Percent solutions express the amount of solute as a percentage of the total volume or mass of the solution.
- Parts per million (ppm) is a unit used to express very dilute solutions and is equivalent to milligrams of solute per liter of solution.
- Concentration is calculated by dividing the moles of solute by the total volume of solution and has units of molarity (M).
- To calculate the concentration of individual ions in an electrolyte
20 concentration of solutions
This document discusses various methods of expressing the concentration of solutions, including:
- Mass/volume percentage, which expresses the mass of solute per volume of solution.
- Mass/mass percentage, which expresses the mass of solute per total mass of solution.
- Volume/volume percentage, which expresses the volume of solute per total volume of solution.
- Parts per million (ppm) and parts per billion (ppb), which express very small concentrations.
- Molar concentration, which expresses the number of moles of solute per liter of solution and is the standard unit in chemistry.
Several sample problems are provided to demonstrate calculating concentrations using these various methods.
CONCENTRATION OF SOLUTIONS
Here are the key steps to solve this problem:
1) Convert grams of NH3 to moles using molar mass (65.3 g / 17 g/mol = 3.83 mol NH3)
2) Use balanced equation to determine moles of other substances (3.83 mol NH3 x 4/1 = 15.32 mol NO)
3) Use heat of reaction and moles of limiting reactant to determine heat (ΔH = -904 kJ/mol NH3 x 3.83 mol NH3 = -3,459 kJ)
Solution concentration
This document discusses key concepts related to solution concentration including:
- Solutions are homogeneous mixtures with a solvent as the major component and solute as the minor component.
- Concentration can be expressed in various ways such as percentage by weight or volume, molarity, and parts per million or billion.
- Dilute solutions have low concentrations while concentrated solutions have high concentrations.
- Molarity calculations allow converting between moles, liters, and grams of solutes and solvents in solutions.
- Dilution decreases concentration by adding more solvent while maintaining the same amount of solute.
Preparation of solutions
This document describes procedures for preparing various chemical solutions. It details how to make 3M nitric acid, 1.5M sulfuric acid, 0.5N phosphoric acid by dilution, and 5% and 25% sodium hydroxide solutions by dissolution. The key steps, materials, and dilution/dissolution formulas are provided. Safety tips are also listed at the end regarding handling chemicals and labeling prepared solutions.
Method of expressing of concentration
This presentation describes different expressing of concentration like normality, molarity, molality, formality.PPM, PPB etc.
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20 concentration of solutions
- Concentration can be expressed in several ways including mass/volume percent, mass/mass percent, volume/volume percent, parts per million (ppm), and molar concentration (mol/L).
- Mass/volume percent is the mass of solute divided by the volume of solution. Volume/volume percent is the volume of solute divided by the volume of solution.
- Mass/mass percent is the mass of solute divided by the mass of solution. Parts per million (ppm) and parts per billion (ppb) express very small concentrations.
- Molar concentration expresses the number of moles of solute per liter of solution and is the standard unit for expressing concentration in chemistry
2 concentration of solutions
This document defines and provides examples for different ways of expressing the concentration of solutions, including mass/volume percent (m/v%), mass/mass percent (m/m%), volume/volume percent (v/v%), parts per million (ppm), parts per billion (ppb), and molar concentration (mol/L). It also discusses how to calculate concentration using the various units and provides examples of dilution calculations.
5.3.1
This document discusses various concepts related to concentration and molarity including:
- Molarity is a measure of the amount of solute dissolved in a solvent and is expressed as moles of solute per liter of solution.
- Percent solutions express the amount of solute as a percentage of the total volume or mass of the solution.
- Parts per million (ppm) is a unit used to express very dilute solutions and is equivalent to milligrams of solute per liter of solution.
- Concentration is calculated by dividing the moles of solute by the total volume of solution and has units of molarity (M).
- To calculate the concentration of individual ions in an electrolyte
20 concentration of solutions
This document discusses various methods of expressing the concentration of solutions, including:
- Mass/volume percentage, which expresses the mass of solute per volume of solution.
- Mass/mass percentage, which expresses the mass of solute per total mass of solution.
- Volume/volume percentage, which expresses the volume of solute per total volume of solution.
- Parts per million (ppm) and parts per billion (ppb), which express very small concentrations.
- Molar concentration, which expresses the number of moles of solute per liter of solution and is the standard unit in chemistry.
Several sample problems are provided to demonstrate calculating concentrations using these various methods.
CONCENTRATION OF SOLUTIONS
Here are the key steps to solve this problem:
1) Convert grams of NH3 to moles using molar mass (65.3 g / 17 g/mol = 3.83 mol NH3)
2) Use balanced equation to determine moles of other substances (3.83 mol NH3 x 4/1 = 15.32 mol NO)
3) Use heat of reaction and moles of limiting reactant to determine heat (ΔH = -904 kJ/mol NH3 x 3.83 mol NH3 = -3,459 kJ)
Solution concentration
This document discusses key concepts related to solution concentration including:
- Solutions are homogeneous mixtures with a solvent as the major component and solute as the minor component.
- Concentration can be expressed in various ways such as percentage by weight or volume, molarity, and parts per million or billion.
- Dilute solutions have low concentrations while concentrated solutions have high concentrations.
- Molarity calculations allow converting between moles, liters, and grams of solutes and solvents in solutions.
- Dilution decreases concentration by adding more solvent while maintaining the same amount of solute.
Preparation of solutions
This document describes procedures for preparing various chemical solutions. It details how to make 3M nitric acid, 1.5M sulfuric acid, 0.5N phosphoric acid by dilution, and 5% and 25% sodium hydroxide solutions by dissolution. The key steps, materials, and dilution/dissolution formulas are provided. Safety tips are also listed at the end regarding handling chemicals and labeling prepared solutions.
Method of expressing of concentration
This presentation describes different expressing of concentration like normality, molarity, molality, formality.PPM, PPB etc.
Molarity and dilution
The document discusses molarity, which is a measurement of concentration that expresses the number of moles of solute per liter of solution. It provides examples of calculating molarity when given the mass of a solute and volume of solution. It also covers diluting solutions, where the moles of solute stay the same but the concentration decreases as volume increases. Molarity can be used to determine the moles, mass, or volume of a solution component when any two pieces of information are known.
Solutions, Molarity, Molality
This document provides information on various concepts related to solutions including vocabulary terms, molarity, molality, and percent composition. For molarity, it defines the term, provides examples of how to calculate molarity given different variables, and discusses dilution problems. For molality, it notes some of the challenges in calculating molality for hydrated solutes. It also defines percent composition and provides sample problems calculating density, molality and molarity for different solutions.
Concentration of solution
A saturated solution contains as much solute as can dissolve at a given temperature, an unsaturated solution contains less, and a super-saturated solution contains more. The maximum amount of solute that can dissolve in a specified amount of solvent at a set temperature is known as the solute's solubility in that solvent at that temperature. Solubility is expressed as the amount of solute that dissolves in 100 grams of solvent. The concentration of a solution refers to the amount of solute present in a given quantity of the solution and can be expressed as a percentage by mass or volume.
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The document discusses concentration of solutions in terms of molarity. It defines molarity as moles of solute per liter of solution. It provides the key formula for calculating molarity given moles of solute and volume of solution. Examples are shown for calculating molarity, moles of solute, and volume of solution given different variables. Dilution of solutions is also discussed, where the number of moles of solute remains constant but volume changes upon addition of solvent.
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containing definition and equations of molarity &normality and so on .and how to prepare solution .
Preparation of the LAB reagents
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How to prepare:
For the Qualitative analysis (identification) of anions and cations from inorganic salt solutions.
1. For sulphate (SO42¯) identification
a. Dilute (6M) Hydrochloric acid (HCl)
b. 0.1M Barium chloride (BaCl2) or Barium nitrate {Ba(NO3)2¬} solution
2. For halide ions identification
a. Dilute nitric acid (2M)
b. 5% Silver nitrate (AgNO3) solution
c. Dilute ammonium hydroxide solution (2M)
d. Concentrated ammonium hydroxide solution (~9M)
3. For nitrate ion identification
a. Concentrated Hydrochloric acid (37%) {÷Conc. Sulphuric acid }
b. 5% Ferrous sulphate (FeSO4) solution
4. For Acetate ion identification
a. Dilute Hydrochloric acid
b. 0.2M Ferric chloride (FeCl3) solution
A. For group I cations
a. Dilute hydrochloric acid (6M)
b. Ammonia solution (9M)
c. Potassium chromate (1M)
B. For group II cations
a. Nitric acid (6M)
b. Stannous chloride (0.1M)
c. Concentrated Ammonia solution (9M)
d. Dilute Ammonia solution (2M)
e. Dilute Sodium hydroxide solution (2M)
C. For group III cations
a. Ammonia solution (9M)
b. Ammonia solution (2M)
c. Potassium ferricyanide (K3[Fe(CN)6]) [250 mg in 10 mL]
d. Potassium thiocyanate [250 mg in 10 mL]
e. Sodium hydroxide (2M)
f. Sodium hydroxide (10M)
MOLARITY
Molarity is a measurement that expresses the concentration of a solute in a solution as moles of solute per liter of solution. It is calculated by taking the moles of solute and dividing by the total liters of solution. Several examples are provided to demonstrate how to calculate molarity from mass, moles, or volume information and how to determine moles or mass of a solute given the molarity and volume of a solution.
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2) Titrating samples of vinegar with the standardized NaOH solution and calculating the molarity and percentage by mass of acetic acid in the vinegar.
3) The titrations used phenolphthalein indicator and were conducted using common lab equipment like a burette, pipette, and Erlenmeyer flasks. Calculations applied the principles of titration stoichiometry and acid-base reactions.
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This document discusses the titration of hydrated oxalic acid with a sodium hydroxide solution of unknown concentration. The titration reaction is used to determine the molarity of the sodium hydroxide solution. Phenolphthalein indicator is added, which causes the solution to change from colorless to light pink at the endpoint of the reaction. By performing the titration and calculating the moles of sodium hydroxide reacted, the experimenter determined the molarity of the sodium hydroxide solution to be 0.21M. Issues that affected the precision of the results are also discussed, such as using too much acid volume past the endpoint. Recommendations for improving technique include avoiding bubbles in the
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Subscribe to my youtube channel for such great contents
www.youtube.com/c/AwesomeBiochemistry
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This document discusses different methods of expressing concentrations in solutions. It defines key terms like solution, standard solution, concentration, percent concentration, parts per million, parts per billion, molarity, normality, molality and formality. It provides formulas and examples to calculate the concentration values using these different methods for solutions like sodium hydroxide and hydrochloric acid. The key methods covered are percent concentration, parts per million, parts per billion, molarity, normality, molality and formality.
13.2 molarity
Molarity describes the concentration of a solution in terms of moles of solute per liter of solution. To calculate molarity, you need the moles of solute and the total volume of solution. The moles of solute can be determined by converting any given mass of solute to moles using the molar mass. The total volume must include both the solute and solvent volumes, as adding solute increases the total volume of the solution. Proper unit conversion and labeling of final answers is important when calculating molarity.
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solutionsclassxii.pdf
1. The document discusses various terms used to express the concentration of solutions such as percentage, molarity, molality, normality, and mole fraction. It provides examples and formulas to calculate these quantities.
2. Several numerical problems are given related to calculating concentration based on the mass or volume of components in a solution. This includes problems determining the percentage or mole fraction composition of mixed solutions.
3. Additional "HOTS" or higher-order thinking skills problems are presented involving multiple steps to determine volumes, densities, or concentrations required to achieve a desired solution composition.
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The document discusses molarity, which is a measurement of concentration that expresses the number of moles of solute per liter of solution. It provides examples of calculating molarity when given the mass of a solute and volume of solution. It also covers diluting solutions, where the moles of solute stay the same but the concentration decreases as volume increases. Molarity can be used to determine the moles, mass, or volume of a solution component when any two pieces of information are known.
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This document provides information on various concepts related to solutions including vocabulary terms, molarity, molality, and percent composition. For molarity, it defines the term, provides examples of how to calculate molarity given different variables, and discusses dilution problems. For molality, it notes some of the challenges in calculating molality for hydrated solutes. It also defines percent composition and provides sample problems calculating density, molality and molarity for different solutions.
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A saturated solution contains as much solute as can dissolve at a given temperature, an unsaturated solution contains less, and a super-saturated solution contains more. The maximum amount of solute that can dissolve in a specified amount of solvent at a set temperature is known as the solute's solubility in that solvent at that temperature. Solubility is expressed as the amount of solute that dissolves in 100 grams of solvent. The concentration of a solution refers to the amount of solute present in a given quantity of the solution and can be expressed as a percentage by mass or volume.
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This document discusses concentration of solutions in chemistry. It defines molarity as moles of solute per liter of solution. It provides an example problem calculating the molarity of a solution made by dissolving 5 grams of nickel chloride hexahydrate in 250 mL of water. It also discusses molality, defined as moles of solute per kilogram of solvent, and provides an example problem calculating the molality of a sodium chloride solution. Finally, it discusses the process of diluting solutions through calculations that conserve the number of moles while changing the volume.
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This document discusses different methods of preparing solutions of varying concentrations, including percentage solutions, molarity, molality, normality, and parts per million. It provides examples and problems for calculating amounts of solutes needed to make solutions of specific concentrations and volumes. Buffer solutions are also introduced as solutions that can tolerate small pH changes during reactions. They are typically composed of a weak acid and its salt.
Quantitative Expressions of the Concentration of Solutions
The document discusses different methods to calculate the concentration of solutions, including percent by mass, percent by volume, molarity, molality, and mole fraction. It provides examples of calculating concentration using each method. Percent by mass is the mass of solute divided by the total mass of the solution. Percent by volume is the volume of solute divided by the total volume of solution. Molarity is moles of solute per liter of solution. Molality is moles of solute per kilogram of solvent. Mole fraction is the moles of one component divided by the total moles of all components.
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The document discusses concentration of solutions in terms of molarity. It defines molarity as moles of solute per liter of solution. It provides the key formula for calculating molarity given moles of solute and volume of solution. Examples are shown for calculating molarity, moles of solute, and volume of solution given different variables. Dilution of solutions is also discussed, where the number of moles of solute remains constant but volume changes upon addition of solvent.
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This document discusses important concepts for preparing solutions in biotechnology. It defines key terms like solute, solvent, concentration, and solution. It explains different units for expressing concentration, such as weight/volume percent, molarity, and normality. Examples are provided for calculating amounts of solute needed to make solutions of a given concentration and volume. Equations are presented for diluting stock solutions to prepare solutions of lower concentration. Serial dilutions are also introduced as a method to make a series of progressively more dilute solutions from a concentrated stock.
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containing definition and equations of molarity &normality and so on .and how to prepare solution .
Preparation of the LAB reagents
Preparation of the LAB reagents
How to prepare:
For the Qualitative analysis (identification) of anions and cations from inorganic salt solutions.
1. For sulphate (SO42¯) identification
a. Dilute (6M) Hydrochloric acid (HCl)
b. 0.1M Barium chloride (BaCl2) or Barium nitrate {Ba(NO3)2¬} solution
2. For halide ions identification
a. Dilute nitric acid (2M)
b. 5% Silver nitrate (AgNO3) solution
c. Dilute ammonium hydroxide solution (2M)
d. Concentrated ammonium hydroxide solution (~9M)
3. For nitrate ion identification
a. Concentrated Hydrochloric acid (37%) {÷Conc. Sulphuric acid }
b. 5% Ferrous sulphate (FeSO4) solution
4. For Acetate ion identification
a. Dilute Hydrochloric acid
b. 0.2M Ferric chloride (FeCl3) solution
A. For group I cations
a. Dilute hydrochloric acid (6M)
b. Ammonia solution (9M)
c. Potassium chromate (1M)
B. For group II cations
a. Nitric acid (6M)
b. Stannous chloride (0.1M)
c. Concentrated Ammonia solution (9M)
d. Dilute Ammonia solution (2M)
e. Dilute Sodium hydroxide solution (2M)
C. For group III cations
a. Ammonia solution (9M)
b. Ammonia solution (2M)
c. Potassium ferricyanide (K3[Fe(CN)6]) [250 mg in 10 mL]
d. Potassium thiocyanate [250 mg in 10 mL]
e. Sodium hydroxide (2M)
f. Sodium hydroxide (10M)
MOLARITY
Molarity is a measurement that expresses the concentration of a solute in a solution as moles of solute per liter of solution. It is calculated by taking the moles of solute and dividing by the total liters of solution. Several examples are provided to demonstrate how to calculate molarity from mass, moles, or volume information and how to determine moles or mass of a solute given the molarity and volume of a solution.
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The document describes a titration experiment involving:
1) Standardizing a sodium hydroxide solution by titrating it against samples of potassium hydrogen phthalate and calculating the molarity of the NaOH.
2) Titrating samples of vinegar with the standardized NaOH solution and calculating the molarity and percentage by mass of acetic acid in the vinegar.
3) The titrations used phenolphthalein indicator and were conducted using common lab equipment like a burette, pipette, and Erlenmeyer flasks. Calculations applied the principles of titration stoichiometry and acid-base reactions.
Discussion exp 1
This document discusses the titration of hydrated oxalic acid with a sodium hydroxide solution of unknown concentration. The titration reaction is used to determine the molarity of the sodium hydroxide solution. Phenolphthalein indicator is added, which causes the solution to change from colorless to light pink at the endpoint of the reaction. By performing the titration and calculating the moles of sodium hydroxide reacted, the experimenter determined the molarity of the sodium hydroxide solution to be 0.21M. Issues that affected the precision of the results are also discussed, such as using too much acid volume past the endpoint. Recommendations for improving technique include avoiding bubbles in the
Preparation of standard, normal and molar solutions
Preparation of standard, Normal and molar solutions
Subscribe to my youtube channel for such great contents
www.youtube.com/c/AwesomeBiochemistry
Methods of expressing concentration
This document discusses different methods of expressing concentrations in solutions. It defines key terms like solution, standard solution, concentration, percent concentration, parts per million, parts per billion, molarity, normality, molality and formality. It provides formulas and examples to calculate the concentration values using these different methods for solutions like sodium hydroxide and hydrochloric acid. The key methods covered are percent concentration, parts per million, parts per billion, molarity, normality, molality and formality.
13.2 molarity
Molarity describes the concentration of a solution in terms of moles of solute per liter of solution. To calculate molarity, you need the moles of solute and the total volume of solution. The moles of solute can be determined by converting any given mass of solute to moles using the molar mass. The total volume must include both the solute and solvent volumes, as adding solute increases the total volume of the solution. Proper unit conversion and labeling of final answers is important when calculating molarity.
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1. The document discusses various terms used to express the concentration of solutions such as percentage, molarity, molality, normality, and mole fraction. It provides examples and formulas to calculate these quantities.
2. Several numerical problems are given related to calculating concentration based on the mass or volume of components in a solution. This includes problems determining the percentage or mole fraction composition of mixed solutions.
3. Additional "HOTS" or higher-order thinking skills problems are presented involving multiple steps to determine volumes, densities, or concentrations required to achieve a desired solution composition.
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2. Several numerical problems are given related to calculating concentration based on the mass or volume of components in a solution. This includes problems determining the percentage or mole fraction composition of mixed solutions.
3. Additional "HOTS" or higher-order thinking skills problems are presented involving multiple steps to determine volumes or densities based on given molarities, molalities, or percentages of solutions.
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1. This document discusses various methods of measuring concentration in chemistry, including molarity, percent concentration, parts per million, and grams per liter.
2. It explains that concentration is calculated by taking the amount of solute divided by the total amount of solution. The amount of solute and solvent must both be specified.
3. Examples are provided for how to calculate concentration using various units for different types of solutions, including calculating moles of solute in a given volume of a molar solution and determining the mass percent of a NaCl solution.
Concentration of Solutions.pptx
The document provides information on different ways of expressing the concentration of solutions, including percent by mass, mole fraction, molarity, molality, percent by volume, and parts per million (ppm). It discusses an activity where students are asked to mix a substance with water and observe whether the mixture is uniform or non-uniform. Finally, it defines key terms related to solution concentration such as solution, solute, solvent, concentration, solubility, miscible, and immiscible.
PPT Preparation of Solutions and Bench Reagents.pdf
This document provides definitions and examples for preparing common types of solutions and interpreting concentration expressions. It begins by defining key terms like solute, solvent, saturated and supersaturated solutions. It then discusses different concentration expressions including percentage by weight/volume, parts, weight/volume, and molarity. Specific examples are provided for calculating amounts of solutes needed to achieve given concentrations and volumes of solutions. The document aims to explain the various methods used for quantifying solutions.
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The document discusses the concept of molarity, which is defined as the number of moles of solute per liter of solution. It provides examples of how to calculate the mass of solute needed to make a solution of a given molarity and volume. The document also discusses how to dilute a more concentrated solution to a desired molarity and volume. Additional topics covered include percent solutions and how to convert between mass and volume percent. The remainder of the document provides recipes for making common laboratory solutions with given molarities.
Chapter 5 stoichiometric calculations summer2014
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This document discusses different methods of expressing the concentration of solutions, including percentage by weight/weight (% w/w), percentage by weight/volume (% w/v), percentage by volume/volume (% v/v), parts per million (ppm), and molarity (M). It provides examples and practice problems for each method. It also covers how dilution affects concentration, standard solutions, primary standards including sodium chloride and potassium dichromate, and common substances that are not primary standards like sulfuric acid and sodium hydroxide.
1573871775612 pc 540 chapter 8_solutions (1)
This document discusses guidelines for preparing laboratory solutions, drug solutions, and reagents. It covers interpreting recipes and expressing concentration in various ways such as weight/volume, molarity, percent, parts per million. Methods are described for preparing dilute solutions from concentrated stocks, biological buffers, and solutions with multiple solutes. Quality assurance measures are outlined including documentation, calibration, and using reference standards.
UNIT- 8 DRUG SOLUTIONS PREPARATIONS
STORAGE
CONCENTRATION EXPRESSION
COMMON SOLVENTS
STABILIZING AGENTS
STORAGE CONDITIONS
REFERENCE STANDARDS
METHODS OF PROCUREMENT OF REFERENCE STANDARDS
FALSE POSITIVE & FALSE NEGATIVE
LESSON-2.-CONCENTRATION-OF-SOLUTIONS.pdf
This document provides an overview of solutions and mixtures. It defines key terms like homogeneous and heterogeneous mixtures, solutes and solvents, concentration, and solubility. It also discusses different units used to measure concentration, including molarity, molality, and percent composition. Methods for separating mixtures like distillation, filtering, and chromatography are also outlined. The document provides examples of calculating concentration using various units and solving stoichiometric problems involving solutions.
calculations.pptx
This document discusses various methods of expressing concentration in pharmaceutical analysis, including:
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- Parts per million (ppm), which expresses the number of grams of solute per 1,000,000 grams of solution.
- Molarity and normality, which express the number of moles or equivalents of solute per liter of solution.
- Examples are provided for converting between different units of concentration like w/v, mg/ml, μg/ml. Dilution techniques and examples for preparing calibration curves from stock solutions are also outlined.
Colligative properties, sifat koligatif
This document discusses colligative properties of solutions, specifically molality and mole fraction. Molality is defined as the number of moles of solute per kg of solvent. Mole fraction is the ratio of moles of solute or solvent to the total moles of solution. Several examples are provided to demonstrate how to calculate molality and mole fraction for different solutions. Practice problems are also included at the end to help reinforce understanding of these concepts.
Calculations Based on Balanced Equations.
A chemical reaction describes what occurs in a chemical change. It shows not only the kind but also the relative amounts of the substances involved in a change. The coefficients written before the formulas in a balanced equation represent the number of moles of each substance involved in a reaction. Since the number of moles is related to the mass of any substance and to the volume of any gaseous substance, the mole relationship can be easily changed to mass/volume relationship. The concepts on how to calculate molarity, molality and normality are important in identifying the relative amounts of the substances involved in a chemical reaction.
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7 concentration part d
- 2. Solution Concentration Concentration = quantity of solute quantity of solution (not solvent) There are 3 basic ways to express concentration: 1) percentages, 2) ppm and ppb (used for very low concentrations) 3) molar concentrations
- 3. 1. Percent concentration % concentration can be in 1a) % V/V 1b) % W/W 1c) % W/V
- 4. %V/V = volume of solute (mL or L) X 100% Volume of solution (mL or L) 1. 140 mL of acetic acid is present in a 500 mL bottle of solution? What is the percentage by volume concentration of acetic acid? 28% V/V 2. Gasohol fuel is a solution of ethanol and gasoline. A typical gasohol mixture available across Canada contains 4.1 L of ethanol in a 55-L tank of fuel. What is the percentage by volume concentration of ethanol? 7.5 3. What is approximate % V/V if 30 mL of pure ethanol is added to 250 mL of water? 11% V/V 1a) Percent volume by volume concentration
- 5. • %m/m = mass of solute (g or kg) X100% mass of solution (g or kg) 1. What is the % W/W if 8.0 g copper is added to enough zinc to produce 100 g of an alloy? 8% W/W. 2. Brass is a copper-zinc alloy. If the concentration of zinc is relatively low, the brass has a golden color and is often used for inexpensive jewellery. If a 35.0 g pendant contains 1.7 g of zinc, what is the percentage weight by weight of zinc in brass? 4.9% W/W 3. What is the % m/mof copper in an alloy when 10 kg of Cu is mixed with 250 kg of Zn? 3.8 % W/W 1b) Percent mass by mass concentration
- 6. • % W/V = mass of solute (g) X 100% volume of solution (mL) • Can use g/ml or kg/L 1. Solder flux, available at hardware stores, contains 16 g of zinc chloride in 50 mL of solution. The solvent is HCl (aq). What is the percentage weight by volume of zinc chloride in the solution? 16 g / 50 mL = 32% W/V 2. If 250 g of sodium chloride is present in 3 L of solution, what is the percentage weight by volume of sodium chloride? 250g/3000ml = 8.5% W/V 1c) Percent mass by volume concentration
- 7. 2. Very low concentrations • Expressed in parts per million (ppm) or parts per billion (ppb) • A type of m/m or m/V concentration • E.g. chlorine concentration in a swimming pool may be expressed as ppm • 1 mg/L 1 ppm 1 mg/1000L 1 ppb 1 mg/kg 1 mg/1000kg • 1 g/L 1 ppt 1 g/kg
- 8. Calculation: ppt • 45 g/kg of a solid • We know that 1 ppt = 1 g/1000 g • Set up proportion • ‘x’ g = 45 g 1000 g 1000g • x = 45 ppt
- 9. Calculation: ppm • 4.5 g/250L of a water solution • We know that 1 ppm = 1 mg/1L • Set up proportion • ‘x’ mg = 45000 g 1 L 250 L • x = 180 ppm
- 10. Calculation: from ppm • 5 ppb Lead in water as V/V% • We know 1 ppb = 1 mg/1 kg • Set up proportion • ‘x’ mg = 5 mg = 5 mg x 100% • 1 kg 1000 g 1000,000 mg • 0.0005% V/V