Unit 2: Solutions

Solutions Unit Overview Thursday 10/5: Introduction to Solutions Video. Start “Saturated and Unsaturated Solutions” Friday 10/6: “Saturated & Unsaturated Solutions”. Work on Independent Practice #1 with extra time Monday 10/9: “Solubility” & Solubility Curves Tuesday 10/10: Solubility Curves. Independent Practice #1 is Due Wednesday 10/11: Quiz #1. Introduction to the Mole Thursday 10/12: Molar Mass Problems Monday: Molar Mass Problems / “Molarity” Tuesday/Wednesday: “Molarity” and Independent Practice #2 Due (end of class) Thursday 10/19: Review Independent Practice #2 & Quiz #2 Friday 10/20: Review Monday: Unit 2 Exam

Wednesday Learning Objectives: Components of a Solution Classify mixtures as heterogeneous or homogeneous Classify heterogeneous mixtures as suspensions or colloids Define solute, solvent, and solution Describe a solution as saturated or unsaturated

Solutions Video While you are watching, take notes about: The different types of mixtures What makes them unique

https://www.youtube.com/watch?v=Vt7lN4QPU0k

Post video check in! 1. What is not a characteristic of a mixture? Two or more components are combined with one another A chemical change occurs within a mixture Elements in a mixture are combined without creating a chemical reaction All of the above

Post video check in! 2. What are the three main types of mixtures? Girded, lattice, suspension Solid, liquid, gas Solution, colloid, suspension None of the above

Post video check in! 3. What is a characteristic of a solution? The particles are visible and identifiable with the naked eye The particles are too small to be visible with the naked eye They contain emulsifiers that help two substances that do not blend All of the above

Matter Pure Substances Elements Compounds Mixtures Homogeneous Heterogeneous Anything that: Has mass Takes up space (has volume) A collection of identical particles A collection of two or more different particles A collection of single atoms of the same kind Two or more different types of atoms chemically combined  A mixture which has uniform composition and properties throughout  A mixture where the parts remain separate after they are mixed

Saturated & Unsaturated Solutions Start working on the Saturated & Unsaturated Solutions POGIL as a team!

Thursday Describe a solution as saturated or unsaturated Learning Objectives: Components of a Solution Classify mixtures as heterogeneous or homogeneous Classify heterogeneous mixtures as suspensions or colloids Define solute, solvent, and solution Describe a solution as saturated or unsaturated

Saturated & Unsaturated Solutions Work as a team to complete the saturated and unsaturated activity When you are done, take the check in quiz. (write the answers on your own paper – the quiz is too tiny for writing ) Take a look at the key - If you got a 100% on the check in quiz, move on to solubility If you get less than 100% on the check in quiz, review the activity and go over your independent practice questions before you move on to solubility

Friday Learning Objectives: Read and interpret Solubility Curves Use solubility curves to determine solubility of a substance when given a temperature

Monday 10/9/17 Learning Objectives: Read and interpret Solubility Curves Use solubility curves to determine solubility of a substance when given a temperature We’ll start by talking about last week – including the exam  Looks like some people still need to finish! Have your binder out and your work from last week.

NEW PLAN Today (Monday) Tuesday Wednesday Thursday Finish Exam (as needed) Quick Notes Check in on Saturated vs. Unsaturated Solubility Check in on Solubility Tuesday Solubility Curves Finish Independent Practice #1 Wednesday Quiz 1 (pick up Independent Practice #2 Thursday What is a MOLE? Mass to Mole Conversions

Matter Pure Substances Elements Compounds Mixtures Homogeneous Heterogeneous Anything that: Has mass Takes up space (has volume) A collection of identical particles A collection of two or more different particles A collection of single atoms of the same kind Two or more different types of atoms chemically combined  A mixture which has uniform composition and properties throughout  A mixture where the parts remain separate after they are mixed

Recap from last week Solution: A type of homogenous mixture which has uniform composition and properties throughout. Particles are too small to be visible with your eyes Solute: the stuff you are adding to the solvent Solvent: what you are adding the solute to Example: Salt water- solution Salt – solute Water - Solvent

Saturated / Unsaturated / Supersaturated Saturated: The maximum amount of solute has been dissolved in the solvent for that volume and temperature Unsaturated: more solute can be dissolved in the solvent at that volume and temperature Supersaturated: more solute has been dissolved in the solvent than would be in a saturated solution. Usually done by manipulating the temperature or by evaporating some of the solvent

Solubility Work as a team to complete the solubility activity When you are done, take the check in quiz. Write the answers on your own paper – the quiz is too tiny for writing ) Take a look at the key - If you got a 100% on the check in quiz, move on to the solubility curves worksheet as a group. If you get less than 100% on the check in quiz, review the activity and go over your independent practice questions before you move on to the solubility curve activity

Solubility Check in! (check the key when you’re done)

Solubility Curves Work with your team to complete the solubility curves practice. One per group – when you’re done, write your own question using the solubility curve given on the large paper. Write the answer on the back. When you are done work on Independent Practice #1 because we will be checking answers at the end of class

Wednesday 10/11/2017 WARM UP Clear your table of everything except something to write with and a calculator. When you are done with the quiz, pick up the molar mass notes and independent practice #2

Thursday 10/12/2017 Learning Target Moles & Molar Mass WARM UP Identify number of atoms of each element when given a chemical formula. Define the chemical mole as 6.022x1023 particles of any substance Explain why chemists use the chemical mole as a counting number WARM UP Have your notes out and pick up a periodic table

What is a mole? 6.022 x 1023 of ANYTHING Just like a dozen is 12 of anything, a mole is 6.022 x 1023 of anything. A mole of cats would be 6.022 x 1023 of cats A mole of eggs would be 6.022 x 1023 eggs A mole of carbon atoms would be 6.022 x 1023

How did chemists determine the mole?

Why do we use it? The mole is so extremely useful because atoms are so very small! If we try to take the mass of individual atoms we get mass readings in AMU (atomic mass units) which aren’t super helpful. Instead, chemists created the mole – a way of taking the mass of 6.022 x 1023 atoms or particles or molecules so we can get our mass readings in grams.

Relative Mass and the Periodic Table 55.847 Fe 26  Relative Atomic Mass  Atomic Number

How many atoms are present in a compound? A chemical formula for a compound represents two things: The elements contained in the compound The number of atoms of each element in the compound, written as subscripts   A few hints: Each capital letter starts a new element If parentheses are present, the subscripts inside the parentheses multiply by those on the outside to calculate a total number of atoms

(NH₄)₂CO₃

Learning Target: Moles and Molar Mass Warm-up: How many atoms of each element are in the compound (NH₄)₂CO₃ N: H: C: O: Learning Target: Moles and Molar Mass Plan for today: Review Unit 1 Exam Review Unit 2 Quiz 1 Moles & Molar Mass

Molar Mass The mass of one mole of that substance (typically in grams) EXAMPLE: (NH₄)₂CO₃ Find the Molar Mass of the above compound

Conversions 1 mole of a substance = the molar mass of that substance Can use this to convert between moles of a substance and grams of a substance EXAMPLE: How many grams are in 1.7 moles of (NH₄)₂CO₃? How many moles are in 654 g of (NH₄)₂CO₃?

Plan for Today Finish Notes Complete Molar Mass & Gram-Mole Conversion practice Complete first page of Independent Practice #2

Molarity Work as a team to complete the molarity activity When you are done, take the check in quiz. If you get a 100% on the check in quiz, start studying for the quiz and exam If you get less than 100% on the check in quiz, review the activity and go over your independent practice questions before you start studying for the quiz

CuCl2 (Copper Chloride) Block Day Warm-Up (on your paper- be ready to share out) Calculate the Molar Mass of the following compounds: CuCl2 (Copper Chloride) C12H22O12 (Glucose) Learning Target: Molarity Define Molarity Use molarity equation to calculate for molarity, moles, or volume Explain the concept of molarity as it relates to concentration Plan for today: Molarity Notes Trashketball

What is Molarity and why do we care about it?

“2 M” is read as “two molar” Molarity M= molarity “2 M” is read as “two molar”

Check in Write a mathematic equation to show how the molarity of a solution is calculated (hint: it should have three variables)

Use your formula to calculate the molarity of the following solution: 210 grams of Copper Chloride mixed in 400 mL of solution

Use your formula to calculate the molarity of the following solution: 2 moles of Glucose mixed in 4 L of solution

Use your formula to calculate the VOLUME of the following solution: A 5.3M solution with 350 g of Copper Chloride

Calculate the molarity of a solution containing 1.5 moles of NaCl in 0.50 L of solution.

Calculate the molarity of a solution containing 0 Calculate the molarity of a solution containing 0.40 moles of acetic acid in 0.250 liters of solution

74.55 g KCl (potassium chloride) in 2000 mL of solution What is the molarity?

Calculate molarity 2.5 grams of Copper Chloride in 1 L of solution.

37.3 grams of KCl in 500 mL of solution.

Calculate the molarity of a solution containing 2 Calculate the molarity of a solution containing 2.6 moles of NaCl dissolved in 2L of water.

Calculate the number of moles of NaCl necessary to make. 5L of a 4 Calculate the number of moles of NaCl necessary to make .5L of a 4.0M solution.

Calculate the number of grams necessary to make. 5L of a 4 Calculate the number of grams necessary to make .5L of a 4.0M solution of NaCl.

Calculate the molarity of a solution where 5 Calculate the molarity of a solution where 5.6g of C2H6O2 are dissolved in 0.3L of water.

When sugar is dissolved in water, what term best describes the sugar?

How many grams of solute are contained in 64. 3mL of a 1 How many grams of solute are contained in 64.3mL of a 1.40M H2SO4 solution

Grams = Molarity x molar mass of the substance (g) x Liters

What mass of sodium sulfate Na2SO4 is present in 250 mL of a 2 What mass of sodium sulfate Na2SO4 is present in 250 mL of a 2.6 M solution?

How many grams of NaCl are contained in 0. 350 L of a 0 How many grams of NaCl are contained in 0.350 L of a 0.28 M solution of sodium chloride?

Calculate the number of moles in 78g of carbon monoxide (CO)

Molarity Work as a team to complete the molarity envelope activity. When you are done, take the check in quiz. If you get a 100% on the check in quiz, start studying for the quiz and exam If you get less than 100% on the check in quiz, review the activity and go over your independent practice questions before you start studying for the quiz

Equations for Molarity M = moles / liters Or Grams = Molarity x molar mass of the substance (g) x Liters