catalyst
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Catalyst. End. Which tastes the strongest?. Justify – TPS. Why did the cup you picked taste the strongest? What was different about it from the other cups?. Lecture 3.4 – Solution Chemistry. Today ’ s Learning Targets. LT 3.5 – I can identify the solute and solvent in a given solution. - PowerPoint PPT PresentationTRANSCRIPT
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Catalyst
End
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Which tastes the strongest?
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Justify – TPS
• Why did the cup you picked taste the strongest? What was different about it from the other cups?
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Lecture 3.4 – Solution Chemistry
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Today’s Learning Targets• LT 3.5 – I can identify the solute and solvent in a
given solution. • LT 3.6 – I can calculate the molarity and percent
composition of a solution and discuss what the final concentration indicates.
• LT 3.10 – I can analyze a substances molarity and determine the number of grams of a compound that are contained within a solution.
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How do we describe solutions?
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I. Solute and Solvent
• The solvent is the substance in which the solute is dissolved and is primary ingredient in a solution.
• The solute is the substance that is dissolved in the solvent.
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II. Solute and Solvent• Water is the universal solvent. • If ever there is a solution that is water and
another compound, then the solvent is always water.
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How do we calculate molarity?
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I. Concentration
• The concentration of a solution is the amount of a particular substance in a given quantity of solution.
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II. Molarity• Molarity is a concentration unit of a solution
expressed as moles of solute dissolved per liter of solution.
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Class Example
• I have 72 g of HCl that I dissolved in 4 L of solution. What is the molarity of this final solution?
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Table Talk• In order to torture this gummy bear you need
you make a solution of KClO3 you dissolve 1,220 g of KClO3 in 1 L of water. What is the molarity of your final solution?
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SUMMARIZE
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White Board Races
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Question 1
• You have a solution that is sugar dissolved in water. What is the solute in this solution?
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Question 2
• You have a solution of naphthalene dissolved in methanol. What is the solvent?
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Question 3
• You have 82 g of NaOH and you dissolve it in 4 L. What is the molarity of the solution?
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Question 4
• You have 52 g of H2SO4 dissolved in 0.5 L. What is the molarity of the solution?
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Question 5
• You have 52 g of CaCl2 dissolved in 0.1 L. What is the molarity of the solution?
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How do we determine grams from molarity?
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I. Hold Up! We Can Work in Reverse
• We can work backwards if we have a molarity and volume of solution.
• From this we can determine both the moles and mass of our solute Molarity of
the solution
Molar Mass of solute
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Class Example
• If you have a 3 L of a 0.6 M solution of AgNO3, then what mass of AgNO3 is contained in this solution?
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Table Talk
• If all the water in 430 mL of a 0.45 M NaCl solution evaporates, what mass of NaCl remains?
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How do we calculate percent composition?
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I. Percent Composition
• Percent composition conveys the concentration in terms of percent of solute in a solution.
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Class Example
• A 4 g sugar cube (Sucrose: C12H22O11) is dissolved in a 350 g of water. What is the percent composition by mass of the sugar solution that is created?
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Table Talk
• You have 5 moles of NaCl and you dissolve this in 500 g of water, what is the concentration of this solution in terms of percent composition?
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SUMMARIZE
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Connect 4
• With a partner you will be using the connect 4 sheet to practice problems.
• Silently read through the directions on the sheet in front of you
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Closing TimeClosing Time• Homework 3.6 due Tuesday/Wednesday