Solution types of stoichiometry problems are no harder than any other stoichiometry problem. You must use the concentration given (molarity) to convert.

Slides:

Advertisements

Similar presentations

Solutions stoichiometry.

Advertisements

Electrolytes Some solutes can dissociate into ions. Electric charge can be carried.

Stoichiometry Chapter 12.

Highland Science Department Limiting Reactants in Solution.

Unit 3: Chemical Equations and Stoichiometry

Information given by chemical equations

1. Write a sentence that describes

Metal + Acid Displacement. Activity Series of Metals.

Chemistry Chapter 10, 11, and 12 Jeopardy

In any chemical reaction, it is easy to run out of one or another reactant – which has an impact on the amount of products that can result from a reaction.

0.277 mol ammonium acetate Convert to grams: mol NH 4 C 2 H 3 O 2 Step 1: Write the formula  NH 4 C 2 H 3 O 2 Step 2: Write the given information.

STANDARD GRADE CHEMISTRY CALCULATIONS Calculations involving the mole. 1 mole of a solid substance is the formula mass of the substance in grams. This.

MOLARITY A measurement of the concentration of a solution Molarity (M) is equal to the moles of solute (n) per liter of solution M = n / V = mol / L 2.

Stoichiometry with Solutions Combining what you’ve just learned with what you are already good at.

The Nature of Aqueous Solutions and Molarity and Solution Stoichiometry Chemistry 142 B James B. Callis, Instructor Autumn Quarter, 2004 Lecture #10.

Section 8.3 pg In any chemical reaction, it is easy to run out of one or another reactant – which has an impact on the amount of products that.

Mind Soccer (Yeaaahhh)

Quantitative Relationships (Stoichiometry). Lets take a moment… sit back… relax… and review some previously learned concepts… Lets take a moment… sit.

What quantities are conserved in chemical reactions? grams and atoms.

Final Information Open-ended: 6/11 (review 6/10) Last day to ask questions for MC 6/14 Topics: –Bonding –Reactions Chemical Equations (balancing, types)

Stoichiometry “Stoichiometry” refers to the relative quantities of moles. It also refers to calculations that make use of mole ratios.

Notes #3 Grams to grams stoichiometry 4- step bridge.

Irrelevant Information to Take Your Mind Off of Stoichiometry The first person to use the word “stoichiometry” was Nicephorus I, the ecumenical Patriarch.

Aqueous Reactions Aqueous Reactions and Solution Stoichiometry CDO High School.

Identify reaction type Agenda  review balancing  Check equations I  Write explaining how to balance.  Class notes: ID reaction types  Demos  Homework:

1 Chapter 8 Quantities in Chemical Reactions Tro, 2 nd ed.

Solutions: Molarity. A. Concentration – measure of the amount of solute that is dissolved in a given amount of solvent I. Concentration of Solutions Solutions:

 Most reactions occur in aqueous solutions because water is cheap, easily accessible and dissolves many substances  Chemicals mix more completely when.

Start-Up What is the molar mass for Calcium hydroxide? A g/mol B g/mol C g/mol D. 27 g/mol.

In the reaction: CH 4 + 2O 2  CO 2 + 2H 2 O How many moles of CH 4 react with 6 moles of O 2 ? A.2 moles B.4 moles C.3 moles D.1 mole.

Chemical Calculations Stoichiometry OBJECTIVES: – Calculate stoichiometric quantities from balanced chemical equations using units of moles and mass.

Stoichiometry ©2011 University of Illinois Board of Trustees

REVIEW: Converting to MOLES WHAT DOES A MOLE REPRESENT? 6.02 x MASS # MOLES Molecular Weight # particles # MOLES 6.02 X Volume of a gasMoles.

Recall: A limiting reagent is the reactant whose entities are completely consumed in a reaction. It is the one that runs out first, and as a result, stops.

Question: Write the chemical reaction when lithium hydroxide is mixed with carbonic acid. Step 1: write out the reactants LiOH (aq) + H 2 CO 3 (aq)

Chemical Calculations Stoichiometry u OBJECTIVES: Calculate stoichiometric quantities from balanced chemical equations using units of moles, mass, representative.

The Math of Chemical Reactions

Stoichiometry A chemical equation shows the reactants (left side) and products (right side) in a chemical reaction. A balanced equation shows, in terms.

Stoichiometry It’s Finally Here!. What in the world is Stoichiometry? Stoichiometry is how we figure out how the amounts of substances we need for a.

UNIT VII Stoichiome-tree Unit 7: Lesson 1. S TOICHIOMETRY Stoichiometry : The relationship between the amount of reactants used in a chemical reaction.

Conversion Stoich. Moles to Quantity Moles of 1 substance are given and you are asked to find the mass, concentration or volume of another.

1 Pb(NO 3 ) 2 (aq) + KI (aq)  PbI 2 (s) + KNO 3 (aq) __ 212 Molarity and Stoichiometry M M V V P P mol M L M = mol L mol = M L What volume of 4.0 M KI.

$200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 $200 $300 $400 $500 $100 Back to the Basics Solution.

Unit 8 Review Stoichiometry. 1. Describe how a chemist uses stoichiometry? To determine the amount of reactants needed or products formed based on the.

Stoich Review. Particles in 10.5 mols of Ammonium Nitrate.

Mole to Mole Assignment. 1. Given the following equation: 2 C 4 H O 2 ---> 8 CO H 2 O Show what the following molar ratios should be. a.

Stoichiometry Introduction to Chemistry. Stoichiometry Example: 2H 2 + O 2 → 2H 2 O Equivalencies: 2 mol H 2 for every 1 mol O 2 2 mol H 2 for every 2.

Here is a helping hand with some of the new material on Molarity:

Solutions Stoichiometry.

9.5 Solutions stoichiometry.

Stoichiometric Review

Solutions stoichiometry.

Stoichiometry with Solutions

Solutions stoichiometry.

Solution stoichiometry.

Unit 13: More Chemical Reactions

Unit 13: Stoichiometry -How can we quantitatively analyze reactions?

The Stoichiometry Game!

Solution Stoichiometry

Stoichiometric Calculations

Unit 4: Chemical Equations and Stoichiometry

Unit 4: Chemical Equations and Stoichiometry

Presentation transcript:

Solution types of stoichiometry problems are no harder than any other stoichiometry problem. You must use the concentration given (molarity) to convert to moles, then use the molar ratio to convert to moles of the final product, then use concentration of the final product to convert to the final answer. Moles/L

Stoichiometry overview Recall that in stoichiometry the mole ratio provides a necessary conversion factor: grams (x)  moles (x)  moles (y)  grams (y) molar mass of xmolar mass of y mole ratio from balanced equation We can do something similar with solutions: volume (x)  moles (x)  moles (y)  volume (y) mol/L of xmol/L of y mole ratio from balanced equation

Calculate the volume of a 2.00 mol/L silver nitrate solution that is needed for 12.0 g of copper metal to react according to the following equation? 2 mol AgNO 3 1 mol Cu x # mol AgNO 3 = 12.0 g Cu 0.38 mol AgNO 3 = 1 mol Cu 63.5 g Cu x Cu(s) + 2AgNO 3 (aq)  Cu(NO 3 ) 2 + 2Ag(s) Calculate the moles of AgNO 3, then volume of AgNO 3 L = 0.38 mol AgNO 3 / 2.00 mol / L = 0.19L = 190mL

Ammonium sulfate is manufactured by reacting sulfuric acid with ammonia. What concentration of sulfuric acid is needed to react with 24.4 mL of a 2.20 mol/L ammonia solution if 50.0 mL of sulfuric acid is used? 1 mol H 2 SO 4 2 mol NH 3 x # mol H 2 SO 4 = L NH mol H 2 SO 4 = 2.20 mol NH 3 L NH 3 x H 2 SO 4 (aq) + 2NH 3 (aq)  (NH 4 ) 2 SO 4 (aq) Calculate mol H 2 SO 4, then mol/L = mol/ L mol/L = mol H 2 SO 4 / L = mol/L

Calculate the volume of mol/L calcium hydroxide solution that can be completely reacted with 25.0 mL of mol/L aluminum sulfate solution. 3 mol Ca(OH) 2 1 mol Al 2 (SO 4 ) 3 x # L Ca(OH) 2 = L Al 2 (SO 4 ) 3 = L Ca(OH) mol Al 2 (SO 4 ) 3 L Al 2 (SO 4 ) 3 x Al 2 (SO 4 ) 3 (aq) + 3Ca(OH) 2 (aq)  2Al(OH) 3 (s) + 3CaSO 4 (s) L Ca(OH) mol Ca(OH) 2 x

A chemistry teacher wants 75.0 mL of mol/L iron(Ill) chloride solution to react completely with a mol/L sodium carbonate solution. What volume of sodium carbonate solution is needed? 3 mol Na 2 CO 3 2 mol FeCl 3 x # L Na 2 CO 3 = L FeCl 3 = L Na 2 CO 3 = 90.0 mL Na 2 CO mol FeCl 3 L FeCl 3 x 2FeCl 3 (aq) + 3Na 2 CO 3 (aq)  Fe 2 (CO 3 ) 3 (s) + 6NaCl(aq) L Na 2 CO mol Na 2 CO 3 x

1.H 2 SO 4 reacts with NaOH, producing water and sodium sulfate. What volume of 2.0 M H 2 SO 4 will be required to react completely with 75 mL of 0.50 mol/L NaOH? 2.How many moles of Fe(OH) 3 are produced when 85.0 L of iron(III) sulfate at a concentration of mol/L reacts with excess NaOH? 3.What mass of precipitate will be produced from the reaction of 50.0 mL of 2.50 mol/L sodium hydroxide with an excess of zinc chloride solution. Assignment

4.a) What volume of 0.20 mol/L AgNO 3 will be needed to react completely with 25.0 mL of 0.50 mol/L potassium phosphate? b) What mass of silver phosphate is produced from the above reaction? Assignment

Answers 2 mol Fe(OH) 3 1 mol Fe 2 (SO 4 ) 3 x # mol Fe(OH) 3 = 85 L Fe 2 (SO 4 ) mol Fe 2 (SO 4 ) 3 L Fe 2 (SO 4 ) 3 x 1. H 2 SO 4 (aq) + 2NaOH(aq)  2H 2 O + Na 2 SO 4 (aq) = 102 mol 1 mol H 2 SO 4 2 mol NaOH x # L H 2 SO 4 = L NaOH = L = 9.4 mL 0.50 mol NaOH L NaOH x 2. Fe 2 (SO 4 ) 3 (aq) + 6NaOH(aq)  2Fe(OH) 3 (s) + 3Na 2 SO 4 (aq) L H 2 SO mol H 2 SO 4 x

3. 2NaOH (aq) + ZnCl 2 (aq)  Zn(OH) 2 (s) + 2NaCl (aq) 1 mol Zn(OH) 2 2 mol NaOH x # g Zn(OH) 2 = L NaOH = 6.21 g 2.50 mol NaOH L NaOH x 4a. 3AgNO 3 (aq) + K 3 PO 4 (aq)  Ag 3 PO 4 (s) + 3KNO 3 (aq) g Zn(OH) 2 1 mol Zn(OH) 2 x 3 mol AgNO 3 1 mol K 3 PO 4 x # L AgNO 3 = L K 3 PO 4 = L = 0.19 L 0.50 mol K 3 PO 4 L K 3 PO 4 x L AgNO mol AgNO 3 x 1 mol Ag 3 PO 4 1 mol K 3 PO 4 x # g Ag 3 PO 4 = L K 3 PO 4 = 5.2 g 0.50 mol K 3 PO 4 L K 3 PO 4 x g Ag 3 PO 4 1 mol Ag 3 PO 4 x 4b. 3AgNO 3 (aq) + K 3 PO 4 (aq)  Ag 3 PO 4 (s) + 3KNO 3 (aq)