COMPOSITION AND FORMULA OF A HYDRATED SALT

Slides:

Advertisements

Similar presentations

Lab # 2 The Formula Of Hydrates. Hydrates Hydrates are ionic compounds that have a specific number of water molecules attached to them. Examples: Calcium.

Advertisements

Stoichiometry © 2009, Prentice-Hall, Inc. Unit 10: Stoichiometry 1 Calculations with Chemical Formulas.

Vocabulary Hydrate - chemically, a salt with water molecule(s) attached MN. xH2O e.g. CaSO4 . ½ H2O Anhydrous - without water MN. xH2O.

Copyright Sautter 2003 HOW ARE THE CHEMICAL FORMULAS FOR COMPOUNDS DETERMINED? THEY CONTAIN WATER !! WE ARE GOING TO CARRY OUT AN EXPERIMENT TO FIND.

Simplest Formula for a Compound Experiment 9

Section 10-1 Counting Particles Chemists need a convenient method for accurately counting the number of atoms, molecules, or formula units of a substance.

CHEMISTRY Matter and Change

Oxford Area High School Science Department

(How many empiricals “fit into” the molecular?)

Chapter 10 review.

Empirical formula of magnesium oxide Background The empirical formula of a compound is the simplest value of the ratio of atoms of each element in the.

Using the MOLE. Percentage composition Percentage composition is the mass of individual elements in a compound expressed as a percentage of the mass of.

Aim: How to determine Empirical and Molecular Formula DO NOW: Here is data from an experiment: 1.Mass of empty crucible + cover = g 2.Mass of crucible.

Molecular Formula Represents the actual number of atoms of each element in compound – Not necessary for ionic compounds – Necessary for covalent compounds.

WHAT IS A MOLE?. Moles: Measuring Matter A UNIT OF MEASURE!!! 1 mole = 6.02 x representative particles – atoms, molecules, formula units, ions –

Percent Composition and Molecular Formulas.  Determining the percent composition of each element in a compound  H 2 O 1. Find the molar mass of the.

 The percent composition of fuel is 81.7% carbon and 18.3% hydrogen. What is the empirical formula of the fuel?  Start by assuming 100 g of the compound.

Determining the Percent of Water in a Hydrated Salt Questions and Calculations Help.

Objective/Warm-Up SWBAT review topics for the final. If you have 30 g of NaCl or 100 g of NaCl, which would have the greater % of Cl? Why? Calculate the.

 substances that include water into their formula  water is not actually part of the chemical substance and this is reflected in the way the formula.

Lab # 4. Key Terms Atomic Radius Ionization Energy Electronegativity Transition element Octet Rule Percent Composition.

Composition Stoichiometry Chapter 7. Percent Composition by Mass What is a percent? A percent is part of a whole quantity. When using percents, we assume.

Empirical and Molecular Formulas. Chemistry Joke Q: What happens to rock that has been heated to 6.02 X degrees? A: It becomes molten!

CHEMICAL QUANTITIES Composition Stoichiometry Calculating Molar Mass Avogadro’s Number and the Mole Percentage Composition and Empirical Formulas Molecular.

Aim: How to determine Empirical and Molecular Formula DO NOW: Copy the question. Here is data from an experiment: 1.Mass of empty crucible + cover =

Empirical Formula and Molecular Formula. Empirical Formula  Empirical formula is the simplest whole number ratio of atoms in a formula  Empirical information.

Hydrates Percent Composition Empirical Formula Naming Chapter 8.

PACKET #6 Moles/Stoichiometry Textbook: Chapters 6 & 9 Reference Table: T & PT

PACKET #6 Moles/Stoichiometry Reference Table: T & PT

Chapter 11 The Mole. I. Measuring Matter A. Counting Particles Chemists needed a convenient method for counting the number of atoms in a sample of a substance.

Chapter Menu The Mole Section 10.1Section 10.1Measuring Matter Section 10.2Section 10.2 Mass and the Mole Section 10.3Section 10.3 Moles of Compounds.

THE MOLE. STANDARDS Use the mole concept to determine the number of particles and mass in a chemical compound. (includes gram to mole to atom conversions)

Chapter Menu The Mole Section 10.1Section 10.1Measuring Matter Section 10.2Section 10.2 Mass and the Mole Section 10.3Section 10.3 Moles of Compounds.

Analysis of Alum Objectives

What do you notice about these formulae? C 2 H 4 C 3 H 6 C 4 H 8.

THE MOLE CHAPTER 10 Chemistry Class Mrs. Gonsalves.

Hydrates (11.5) Hydrate- compound with a specific amount of water molecules bound to it.

Exp 3A: The Empirical Formula of an Oxide

Empirical Formula of Magnesium Oxide

Exploring the reaction of Mg with O2

Section 9.3—Analysis of a Chemical Formula

Click a hyperlink or folder tab to view the corresponding slides.

Composition Stoichiometry

Empirical and Molecular Formulas

Exp 3B - Hydrates and Thermal Decomposition

PACKET #6 Moles/Stoichiometry Reference Table: T & PT.

Do Now: If one stick of Juicy Fruit gum weighs 3.0g, what percent of the total mass of the gum is sugar?

AP Chemistry Unit 2 Review: Choose your destiny

Percent Composition, Empirical Formulas, and Molecular Formulas

Section 3.2 Stoichiometry and Compound Formulas

The Mole -just as a _____ is always ____, a _______ is always _______,

Percent Composition Empirical Formula Molecular Formula

Unit 6 Mole Calculations

II. Percent composition

Chapter 10: The Mole.

Analysis of Alum Objectives

6.9 – NOTES Formula of a Hydrate

II. Percent composition

Chemical Composition Mole (mol) – The number equal to the number of carbon atoms in grams of carbon. Avogadro’s number – The number of atoms in exactly.

Using Chemical Formulas

Some compounds exist in a “hydrated” state.

Empirical formulas of compounds – experiment part a

Introduction to the Mole and Math Concepts

Chemical Quantities For example – let’s say you want to buy some Bazooka Gum You could buy it by the piece from the deli You could buy it by the box from.

Empirical and Molecular Formulas

Do Now: If one stick of Juicy Fruit gum weighs 3.0g, what percent of the total mass of the gum is sugar?

Using Chemical Formulas

(How many empiricals “fit into” the molecular?)

Molecular Formula.

Chemical Formulas Tell type & number atoms in compound

Presentation transcript:

COMPOSITION AND FORMULA OF A HYDRATED SALT By : aisha al-anssari 200800271 haya al-dossari 201100907 ghadah al-ghamdi 201102713

Introduction A hydrate is a chemical that has water molecules loosely bonded to it. The water molecules are not actually part of the formula, so the formula is written slightly differently. The water can easily be removed from a hydrate just by heating strongly. You will be weighing a hydrate and heating it to remove the water (now called "anhydrous salt") and weigh it again. You can now find the percent of the anhydrous salt and the water. By finding a mol ratio, you can find out how many moles of water there are per mol of anhydrous salt. This number goes just before the H2O in the formula.

Objective Determination of the water of hydration in a hydrated barium chloride salt and using this value to determine the percent composition of a mixture of hydrated barium chloride and sand.

Material required Barium chloride dehydrate Crucible and cover Tongs Clay triangle Electronic balance Tripod stand Burner

Procedure Clean and dry a crucible and find its mass on an accurate balance.

Objective Obtain a scoop of the hydrate from your teacher and find the mass again.

Procedure Heat the crucible under moderate heat for 3-5 minutes. Let the crucible cool and find its mass again.

Procedure Heat the crucible again under moderate heat for another 2 minutes. Place an inverted beaker over it while cooling. Find its mass again. Repeat this heating and weighing until the mass doesn't change any more (stays within .05 grams).

Conclusion As the conclusion, by doing the empirical method we can determined the number of moles in the given substance of the element. Moreover this method also help us to find the real molecular formula.