May 09, Ksp.notebook. Ksp = [Li + ] [F + ] Find the Ksp for the above reaction.
|
|
- Samson Harvey
- 5 years ago
- Views:
Transcription
1 example: Constant Product K sp Solubility Product Constant Some compounds dissolve in water Some compounds dissolve better than others The more that a compound can dissolve, the more soluble the compound is Solubility can be quantified using K sp Equilibrium equation: M NM (s) M + (aq) + NM (aq) solubility NaCl MgSO 4 = > < example: [Li + ] [F + ] If you calculate the molarity of saturated LiF(aq) as 0.50 M, what is the molarity of Li +? F? Find the Ksp for the above reaction. 3. Write the equilibrium equation for the dissolution of sodium chloride. 4. Based upon your molarity calculation, what is the concentration of sodium ions? What is concentration of chlorine ions? 5. Calculate the Ksp. Calculations: 1. Calculate the number of moles of NaCl present in the 10.0 ml of saturated solution. 2. Calculate the molarity of the saturated sodium chloride solution. Calculations: 1. Calculate the number of moles of NaCl present in the 10.0 ml of saturated solution. 2. Calculate the molarity of the saturated sodium chloride solution. 1
2 Calculations: 1. Calculate the number of moles of NaCl present in the 10.0 ml of saturated solution. 2. Calculate the molarity of the saturated sodium chloride solution. Write the equilibrium equation for lithium fluoride: Write the equilibrium equation for lithium fluoride: 1) Determine formula for solid Write the equilibrium equation for magnesium oxide: Write the equilibrium equation for beryllium chloride: Write the equilibrium equation for potassium sulfide: 2) Determine the products and write as a reversible reaction 1) Write the equilibrium equation for iron(iii) carbonate. 1) Write the equilibrium equation for lithium chloride. 2) Calculate the Ksp, given that 3.05g dissolve in 500mL of water. 2) Write the equilibrium equation for lithium chloride. 3) Calculate the Ksp for lithium chloride, given that 3.05g dissolve in 500.mL of water. 2
3 10. REACHING EQUILIBRIUM. Initially, the dissolving (forward) reaction is faster. As more sodium chloride dissolves, what happens to the number of ions in solution? How does this affect the rate of crystallization (the ions coming together to form the solid)? Draw a graph to show the change in rates over time. 11. SATURATED SOLUTION AND EQUILIBRIUM. Describe the equilibrium state of the saturated solution you initially prepared. Include rates and conditions. What happens to the concentration of sodium chloride dissolved in solution, once it is saturated? Are ions still moving into and out of solution? Write the equation to show equilibrium. 12. DISSOLVING AND ENERGY. When one mole of sodium chloride is dissolved in a large volume of water, 3.88 kj of energy are absorbed. Will the temperature of the surroundings and the solution increase or decrease? Explain why. Is this reaction endothermic or exothermic? Describe the reaction in terms of energy and bonds. Draw and explain a labeled energy graph to summarize this reaction. Is the reaction is favored or not based upon enthalpy? Write the equilibrium equation for magnesium oxide: 4. Based upon your molarity calculation, what is the concentration of sodium ions? What is concentration of chlorine ions? 5. Calculate the Ksp. Write the equilibrium equation for beryllium chloride: Write the equilibrium equation for potassium sulfide: 3
4 Equilibrium Expression Potassium bromide dissolving in water KBr(s) K + (aq) + Br (aq) 7. WATER. Describe the water. Describe the polar covalent bond and the electrons in that bond that holds together the water molecule. Explain the polarity of the water molecule. Describe the dipole dipole attraction (hydrogen bonds) between water molecules. 8. SODIUM CHLORIDE. Describe the formation of the ions. How does a sodium atom become an ion? How does a chlorine atom become a chlorine ion? Describe the solid sodium chloride and the ionic bond between the ions that holds together the solid salt. 9. DISSOLVING. Describe the dissolving of sodium chloride in water initially before it reaches saturation. What happens to the ionic bond? Where are the ions? What new attractions form? How are water molecules involved? Include collisions. Write an equation for dissolving. 10. REACHING EQUILIBRIUM. Initially, the dissolving (forward) reaction is faster. As more sodium chloride dissolves, what happens to the number of ions in solution? How does this affect the rate of crystallization (the ions coming together to form the solid)? Draw a graph to show the change in rates over time. 11. SATURATED SOLUTION AND EQUILIBRIUM. Describe the equilibrium state of the saturated solution you initially prepared. Include rates and conditions. What happens to the concentration of sodium chloride dissolved in solution, once it is saturated? Are ions still moving into and out of solution? Write the equation to show equilibrium. 12. DISSOLVING AND ENERGY. When one mole of sodium chloride is dissolved in a large volume of water, 3.88 kj of energy are absorbed. Will the temperature of the surroundings and the solution increase or decrease? Explain why. Is this reaction endothermic or exothermic? Describe the reaction in terms of energy and bonds. Draw and explain a labeled energy graph to summarize this reaction. Is the reaction is favored or not based upon enthalpy? 13. COMPARING SOLUBILITY. Compare the molarity of the saturated solution of calcium sulfate and magnesium sulfate. Which compound is more soluble? Explain what this means. How does the Ksp indicate this? What does their solubility suggest about the strength of the ionic bond between these ions? 15 d. If silver nitrate solution is added to a solution of sodium chloride, what do you expect to happen? What will happen to the ions in solution? Write an equation for this reaction. e. Describe the reaction and formation of the precipitate. Compare the appearance of a solution with a soluble compound to the appearance with an insoluble precipitate. f. Write an equation for the reaction of silver nitrate and sodium chloride. Use a collision to explain the formation of the precipitate. 14. ELECTRICAL FORCE AND THE IONIC BOND. a. The magnitude of electrical force acting between two charges depends directly upon the and inversely upon the. Copy and complete the sentence. 1. Calculate the number of moles of NaCl present in the 10.0 ml of saturated solution. 2. Calculate the molarity of the saturated sodium chloride solution. 3. Write the equilibrium equation for the dissolution of sodium chloride. 4. Based upon your molarity calculation, what is the concentration of sodium ions? What is concentration of chlorine ions? 5. Calculate the Ksp. 6. Repeat 1 5 for magnesium sulfate and calcium sulfate 4
5 Text Referencesmolarity calculations p. 473 electrolytes p solublity p. 492 Ksp p Ksp.notebook 1. Write the solubility equilibrium equation for calcium sulfate, CaSO4. 2. Write the solubility equilibrium equation for magnesium hydroxide. 3. Write the equilibrium equation for strontium carbonate. 4. Write the solubility equilibrium equation for copper II phosphate. 1) Equilibrium Equation 12/3/13 Then, write the Ksp expressions for each :) 1) K sp= 2) 3) 4) 2) K sp= 3) K sp= 4) K sp= 5
6 1. Write the solubility equilibrium equation for calcium sulfate, CaSO4. 2. Write the solubility equilibrium equation for magnesium hydroxide. 3. Write the equilibrium equation for strontium carbonate. 4. Write the solubility equilibrium equation for copper II phosphate. Then, write the Ksp expressions for each :) Ksp for any salt: A x B y (s) Example: Ksp for Calcium fluoride: K sp = [A y+ ] x [B x ] y xa y+ (aq) + yb x (aq) K sp = [Ca 2+ ][F ] 2 Ag 2 SO 4 (s) 2 Ag + (aq) + SO 4 2 (aq) K sp = [Ag + ] 2 [SO 4 2 ] K sp = [A y+ ] x [B x ] y A x B y (s) xa y+ (aq) + yb x (aq) Example: K sp = [Ca 2+ ][F ] 2 Ksp for Calcium fluoride: Ksp for any salt: Ag 2 SO 4 (s) 2 Ag + (aq) + SO 4 2 (aq) K sp = [Ag + ] 2 [SO 4 2 ] Calculating K sp from solubility Most parts of the ocean are nearly saturated with CaF2. In a region where evaporation raises the concentration of dissolved materials, the mineral fluorite, CaF2, may precipitate. A saturated solution of CaF2 of 25 o C is 3.4x10 4 M. Calculate the solubility product constant for CaF2. K sp = [Ca 2+ ] [F ] 2 K sp = [Ca 2+ ] [F ] 2 Lab 3 Conclusion p.532# Calculate Ksp for sodium sulfate if the concentration is 2.05g/1000. ml. 1. Write the solubility equilibrium equation for sodium sulfate. 2. Write the equilibrium equation for potassium carbonate. 3. Write the Ksp expression for both. 12/4/13 4. Calculate Ksp for sodium sulfate if the concentration is 2.05g/1000ml. sodium sulfate potassium carbonate 6
7 4. Calculate Ksp for sodium sulfate if the concentration is 2.05g/1000. ml. p. 532 # 1 3 Homework #2 Lab 3 Conclusion p.532#1-3 The Ksp value for silver carbonate is 8.4 x at 298K. The concentration of carbonate ions in a saturated solution is 1.28 x 10 4 M. What is the concentration of silver ions? Homework #2 The Ksp value for silver carbonate is 8.4 x at 298K. The concentration of carbonate ions in a saturated solution is 1.28 x 10 4 M. What is the concentration of silver ions? 3) Copper(I) bromide is dissolved in water to saturation at 25 oc. The concentration of copper ions in solution is 7.9 x 10 5 mol/l. Calculate the Ksp for copper (I) bromide at this temperature. 14. ELECTRICAL FORCE AND THE IONIC BOND. a. The magnitude of electrical force acting between two charges depends directly upon the and inversely upon the. Copy and complete the sentence. b. Use electrical force to predict which ion will be more attracted to an anion with a charge of 1: a +1 cation or a +2 cation. Explain your reasoning. c. Larger ions cannot get as close to each other as smaller ions. Use electrical force to predict which ion will be more attracted to an anion with a charge of 1: a smaller +1 cation or a larger +1 cation. Explain your reasoning. 7
8 15. SILVER CHLORIDE AND SILVER NITRATE. The concentration of a saturated solution of silver chloride is 1.34 x 10 5 M. a. What does this indicate about the solubility of silver chloride. Explain. Compare the solubility of sodium chloride and silver chloride. Compare the saturated solutions. b. What does this suggest about the attraction between silver and chloride ions compared to their attractions to water molecules? Explain. c. Silver nitrate is fairly soluble. How would the Ksp of silver nitrate compare to the Ksp of silver chloride. Compare the number of ions in a saturated solution of silver nitrate to the ions in solution of silver chloride. Which has more ions in solution? d. If silver nitrate solution is added to a solution of sodium chloride, what do you expect to happen? What will happen to the ions in solution? Write an equation for this reaction. e. Describe the reaction and formation of the precipitate. Compare the appearance of a solution with a soluble compound to the appearance with an insoluble precipitate. f. Write an equation for the reaction of silver nitrate and sodium chloride. Use a collision to explain the formation of the precipitate. Homework #2 The Ksp value for silver carbonate is 8.4 x at 298K. The concentration of carbonate ions in a saturated solution is 1.28 x 10 4 M. What is the concentration of silver ions? Calculating K sp from solubility Lab 3 Conclusion p.532#1-3 Most parts of the ocean are nearly saturated with CaF2. In a region where evaporation raises the concentration of dissolved materials, the mineral fluorite, CaF2, may precipitate. A saturated solution of CaF2 of 25 o C is 3.4x10 4 M. Calculate the solubility product constant for CaF2. 2. Write K sp expression Calculating concentrations using K sp At a temperature of 298K, the concentration of Ca 2+ in a given saturated solution of CaF2 is 2.2x10 4 M and the Ksp for CaF2 is 1.6x Calculate the concentration of F in the solution. Calculating concentrations using K sp At a temperature of 298K, the concentration of Ca 2+ in a given saturated solution of CaF2 is 2.2x10 4 M and the Ksp for CaF2 is 1.6x Calculate the concentration of F in the solution. 1.6x10 10 = [2.2x10 4 ][F ] 2 1.6x10 10 = [F ] 2 2.2x x10 10 = [F ] 2 = 8.5 x 10 4 M = [F ] 2.2x x10 10 = [2.2x10 4 ][F ] 2 1.6x10 10 = [F ] 2 2.2x x10 10 = [F ] 2 = 8.5 x 10 4 M = [F ] 2.2x10 4 8
9 1. Write the solubility equilibrium equation for sodium sulfate. 2. Write the equilibrium equation for potassium carbonate. 3. Write the Ksp expression for both. 4. Calculate Ksp for sodium sulfate if the concentration is 2.05g/1000ml. sodium sulfate potassium carbonate 9
Solubility Equilibria. Dissolving a salt... Chem 30S Review Solubility Rules. Solubility Equilibrium: Dissociation = Crystalization
Chem 30S Review Solubility Rules Solubility Equilibria Salts are generally more soluble in HOT water(gases are more soluble in COLD water) Alkali Metal salts are very soluble in water. NaCl, KOH, Li 3
More informationSolubility Equilibrium
2016 Ksp note.notebook Solubility Equilibrium Learning Goals: to understand what happens when a compound dissolves in water to calculate the extent of dissolution...the molar solubility to calculate the
More informationExplain freezing-point depression and boiling-point elevation at the molecular level.
Solutions 1 UNIT4: SOLUTIONS All important vocabulary is in Italics and bold. Describe and give examples of various types of solutions. Include: suspension, emulsion, colloid, alloy, solute, solvent, soluble,
More informationModified Dr. Cheng-Yu Lai
Ch16 Aqueous Ionic Equilibrium Solubility and Complex Ion Equilibria Lead (II) iodide precipitates when potassium iodide is mixed with lead (II) nitrate Modified Dr. Cheng-Yu Lai Solubility-product constant
More informationChemistry 12 Solubility Equilibrium I. Name: Date: Block: 1. Solutions Vocab & Calculations 2. Predicting Solubility 3.
Chemistry 12 Solubility Equilibrium I Name: Date: Block: 1. Solutions Vocab & Calculations 2. Predicting Solubility 3. Writing Equations Solutions Vocab & Calculations What is a solution? A homogenous
More informationName period AP Unit 8: equilibrium
Name period AP Unit 8: equilibrium 1. What is equilibrium? Rate of the forward reaction equals the rate of the reverse reaction 2. How can you tell when equilibrium has been reached? The concentrations
More informationName: Thermochemistry. Practice Test C. General Chemistry Honors Chemistry
Name: Thermochemistry C Practice Test C General Chemistry Honors Chemistry 1 Objective 1: Use the relationship between mass, specific heat, and temperature change to calculate the heat flow during a chemical
More informationinsoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water
Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of
More informationPlease hand your completed booklet to your Chemistry tutor when you begin A Level Chemistry in September
#THIS I S TH E P L AC E A-LEVEL CHEMSITRY NAME: You should complete this work ready for starting Year 1 A Level Chemistry. If there are any questions that you cannot do, even after using your GCSE notes
More informationGive 6 different types of solutions, with an example of each.
Warm up (Jan 5) Give 6 different types of solutions, with an example of each. 1 Warm Up (Jan 6) 1. Write the reaction showing the dissolving of the following solids (be sure to note whether they are covalent
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More information1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions)
Chemistry 12 Solubility Equilibrium II Name: Date: Block: 1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions) Forming a Precipitate Example: A solution may contain the ions Ca
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationName HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions
Name HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are
More informationHonors Chemistry Unit 4 Exam Study Guide Solutions, Equilibrium & Reaction Rates
Honors Chemistry Unit 4 Exam Study Guide Solutions, Equilibrium & Reaction Rates Define the following vocabulary terms. Solute Solvent Solution Molarity Molality Colligative property Electrolyte Non-electrolyte
More informationStudent Name: Teacher: Date: District: NCGaston. Assessment: 9_12 Science Chemistry Exam 3. Description: Chemistry Mock Final Exam
Student Name: Teacher: Date: District: NCGaston Assessment: 9_12 Science Chemistry Exam 3 Description: Chemistry Mock Final Exam 2014-15 Form: 301 1. Shown below is a model of the structure of atom X.
More informationWe CAN have molecular solutions (ex. sugar in water) but we will be only working with ionic solutions for this unit.
Solubility Equilibrium The Basics (should be mostly review) Solubility is defined as the maximum amount of a substance which can be dissolved in a given solute at a given temperature. The solubility of
More informationLAB # 5: Metals and Single Replacement Reactions
LAB # 5: Metals and Single Replacement Reactions Purpose: Compare different metals and their reactions with hydrochloric acid. Construct a model of oxidation and reduction in single replacement reactions.
More informationProperties of Compounds
Chapter 6. Properties of Compounds Comparing properties of elements and compounds Compounds are formed when elements combine together in fixed proportions. The compound formed will often have properties
More informationName CHEMISTRY / / Oxide Reactions & Net Ionic Reactions
Name CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are two
More information5. Pb(IO 3) BaCO 3 8. (NH 4) 2SO 3
Chemistry 11 Solution Chemistry II Name: Date: Block: 1. Ions in Solutions 2. Solubility Table 3. Separating Ions Ions in Solutions Ionization Equation - Represents the salt breaking apart into ions. Practice:
More informationAP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section
Slide 1 / 91 Slide 2 / 91 AP Chemistry Aqueous Equilibria II: Ksp & Solubility Products Table of Contents: K sp & Solubility Products Slide 3 / 91 Click on the topic to go to that section Introduction
More informationThermodynamics. Standard enthalpy change, H
Standard enthalpy change, H Thermodynamics Enthalpy change, H, is defined as the heat energy change measured under conditions of constant pressure. The value of the enthalpy change for a particular reaction
More information1. Dimensional Analysis: convert the following values a. 47,340 cm to m Unit 1: Chemistry Matters b. 40.64 km to m c. 58,700 ml to L 2. Calculate the number of significant figures a. 0.0210 b. 3.6056 c.
More informationChapter 19. Solubility and Simultaneous Equilibria p
Chapter 19 Solubility and Simultaneous Equilibria p. 832 857 Solubility Product ) The product of molar concentrations of the constituent ions, each raised ot the power of its stoichiometric coefficients
More informationWhat are the rules for writing and naming stable ionic formulas?
1 1. Define electronegativity. a measure of the ability of an atom in a chemical compound to attract electrons. 2. On the periodic table, where are the LEAST/MOST electronegative elements found? Least-Bottom
More informationMacro Tab: Part A. Shake some salt into the water. 1. Identify the solute and the solvent: The solute is and the solvent is.
PhET Simulation: Sugar and Salt Solutions Name Period 1 2 3 4 Useful Information Evaporation: You can evaporate all the water and see the solute crystallize above its saturation point. Formula Molar mass
More information(03) WMP/Jun10/CHEM4
Thermodynamics 3 Section A Answer all questions in the spaces provided. 1 A reaction mechanism is a series of steps by which an overall reaction may proceed. The reactions occurring in these steps may
More informationSolubility Rules and Net Ionic Equations
Solubility Rules and Net Ionic Equations Why? Solubility of a salt depends upon the type of ions in the salt. Some salts are soluble in water and others are not. When two soluble salts are mixed together
More informationIONIC CHARGES. Chemistry 51 Review
IONIC CHARGES The ionic charge of an ion is dependent on the number of electrons lost or gained to attain a noble gas configuration. For most main group elements, the ionic charges can be determined from
More informationTry this one Calculate the ph of a solution containing M nitrous acid (Ka = 4.5 E -4) and 0.10 M potassium nitrite.
Chapter 17 Applying equilibrium 17.1 The Common Ion Effect When the salt with the anion of a is added to that acid, it reverses the dissociation of the acid. Lowers the of the acid. The same principle
More informationGas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T
Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided
More informationSolubility Equilibrium When a substance dissolves an equilibrium results between the precipitate and the dissolved ions. The solution becomes
Solubility Equilibrium When a substance dissolves an equilibrium results between the precipitate and the dissolved ions. The solution becomes saturated. The particles dissolving equals the particles precipitating.
More informationLect. 2: Chemical Water Quality
The Islamic University of Gaza Faculty of Engineering Civil Engineering Department M.Sc. Water Resources Water Quality Management (ENGC 6304) Lect. 2: Chemical Water Quality ١ Chemical water quality parameters
More informationChapter 16: Applications of Aqueous Equilibrium Part 3. Solubilities of Ionic Compounds and K sp
Chapter 16: Applications of Aqueous Equilibrium Part 3 Solubilities of Ionic Compounds and K sp You ve already learned that not all ionic compounds are water soluble. You memorized the solubility rules
More information22. What is the maximum concentration of carbonate ions that will precipitate BaCO 3 but not MgCO 3 from a solution that is 2.
PX312-1718 1. What is the solubility product expression for Th(IO 3 ) 4? A) K sp = [Th 4+ ][4IO 3 ] 4 B) K sp = [Th 4+ ][IO 3 ] C) K sp = [Th][IO 3 ] 4 D) K sp = [Th 4+ ][IO 3 ] 4 E) K sp = [Th 4+ ][IO
More informationmohd faisol mansor/chemistry form 4/chapter 5 CHAPTER 5 CHEMICAL BONDS
CHAPTER 5 CHEMICAL BONDS Almost all chemical substances exist as compounds in nature except inert gases and other stable element (such as gold and silver). Atom of other element that have less than eight
More informationQuick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent
Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,
More informationUnit 6 ~ Learning Guide Name:
Unit 6 ~ Learning Guide Name: Instructions: Using a pencil, complete the following notes as you work through the related lessons. Show ALL work as is explained in the lessons. You are required to have
More informationSOLUBILITY REVIEW QUESTIONS
Solubility Problem Set 1 SOLUBILITY REVIEW QUESTIONS 1. What is the solubility of calcium sulphate in M, g/l, and g/100 ml? 2. What is the solubility of silver chromate? In a saturated solution of silver
More informationCovalent (sharing of electron pairs) Ionic ( electrostatic attraction between oppositely charged ions)
Covalent (sharing of electron pairs) Ionic ( electrostatic attraction between oppositely charged ions) Metallic (electrostatic attraction between + metal ions and delocalised electrons) Group 1 ions 1+
More informationNet Ionic Reactions. The reaction between strong acids and strong bases is one example:
Net Ionic Reactions Model 1 Net Ionic Reactions. Net ionic reactions are frequently used when strong electrolytes react in solution to form nonelectrolytes or weak electrolytes. These equations let you
More informationSolubility and Complex-ion Equilibria
Solubility and Complex-ion Equilibria Solubility Equilibria Many natural processes depend on the precipitation or dissolving of a slightly soluble salt. In the next section, we look at the equilibria of
More informationQ = Enthalpy change for the formation of calcium chloride (P). D Twice the enthalpy change of atomization of chlorine (S).
1 What is the equation for the first electron affinity of sulfur? S(s) + e S (g) S(g) + e S (g) S(s) S + (g) + e S(g) S + (g) + e 2 The diagram shows a orn-haber cycle for calcium chloride. It is not drawn
More information2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product?
PRE-AP CHEMISTRY SPRING FINAL EXAM REVIEW Name _ Period Exam Date 100% COMPLETION OF THIS REVIEW BY THE DAY OF YOUR FINAL EXAM WILL COUNT AS A 5 POINT BONUS ADDED TO YOUR FINAL EXAM SCORE. THERE WILL BE
More information1. (i) Give an equation for the dissociation of propanoic acid and hence an expression for its dissociation constant, K a. ...
1. (i) Give an equation for the dissociation of propanoic acid and hence an expression for its dissociation constant, K a.... At 5 C K a for propanoic acid is 1.30 10 5 mol dm 3. Find the ph of a solution
More informationSOLUTIONS. Homogeneous mixture uniformly mixed on the molecular level. Solvent & Solute. we will focus on aqueous solutions
SOLUTIONS Homogeneous mixture uniformly mixed on the molecular level Solvent & Solute we will focus on aqueous solutions SOLUTE-SOLVENT SOLVENT INTERACTIONS Why do solutions form? Processes occur spontaneously
More informationHonors Chemistry Semester 2 Final Exam MC Practice
Honors Chemistry Semester 2 Final Exam MC Practice Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1. What do the alkali metals all have in common?
More informationIB Chemistry Solutions Gasses and Energy
Solutions A solution is a homogeneous mixture it looks like one substance. An aqueous solution will be a clear mixture with only one visible phase. Be careful with the definitions of clear and colourless.
More informationChemistry 20 Final Review Solutions Checklist Knowledge Key Terms Solutions
Chemistry 20 Final Review Solutions Checklist Have you mastered the concepts, applications, and skills associated with the following items? Check them off when you are confident in your understanding.
More informationPart 01 - Notes: Reactions & Classification
Objectives: Identify, define, and explain: combination reaction, synthesis reaction, decomposition reaction, single replacement reaction, double replacement reaction, combustion reaction, rapid oxidation,
More informationChemical Equilibrium
Chemical Equilibrium THE NATURE OF CHEMICAL EQUILIBRIUM Reversible Reactions In theory, every reaction can continue in two directions, forward and reverse Reversible reaction! chemical reaction in which
More informationUNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12)
I. Multiple Choice UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) 1) Which one of the following would form an ionic solution when dissolved in water? A. I 2 C. Ca(NO 3 ) 2 B. CH 3 OH D.
More informationExample 1: m = 100mL = 100g T i = 25 o C T f = 38 o C ΔT = 13 o C c = 4.18 J / (g o C) Q =??? Molar Heat of Dissolutions
Molar Heat of Dissolutions It is observed that when 8.0g of Lithium chloride (LiCl) at 25 o C is dissolved in 100mL of water inside a calorimeter the final temperature of the water is 38 o C. Questions:
More informationQ1. As the world population increases there is a greater demand for fertilisers.
Q1. As the world population increases there is a greater demand for fertilisers. (a) Explain what fertilisers are used for............. (b) The amount of nitrogen in a fertiliser is important. How many
More informationIonic or Covalent: Track Those Electrons
Electrons Goal Use rings and diagrams to model the formation of ionic compounds and covalent compounds. What to Do Use a blank piece of paper and rings to model electron transfers and electron sharing,
More informationPreliminary Chemistry
Name: Preliminary Chemistry Lesson 6 Water In Theory. This booklet is your best friend. Success is Contagious. Synergy Chemistry. 0466 342 939 garyzhanghsc@gmaiil.com www.hscsynergyeducation.weebly.com
More information- Some MOLECULES can gain or lose electrons to form CATIONS or ANIONS. These are called POLYATOMIC IONS
63 POLYATOMIC IONS - Some MOLECULES can gain or lose electrons to form CATIONS or ANIONS. These are called POLYATOMIC IONS - Polyatomic ions form ionic compounds in the same way that single-element ions
More informationPractice I: Chemistry IGCSE
Practice I: Chemistry IGCSE cristian.obiol@gmail.com 1) Explain the following processes related to changes of states of matter. -Melting:... -Vaporization:... -Freezing:... -Condensation:... -Sublimation:...
More informationSilver nitrate solution is added to sodium dichromate solution
Chem. 110 50 Points Final Exam Part 1 Practice Write the chemical names or formulas for the following a H 2 SO 4 b NiNO 2 c Aluminum thiosulfate d Plumbic acetate e Ag 2 C 2 O 4 f P 2 O 5 g Cyanic acid
More informationChemistry 20 Unit 3A Solutions FITB Notes. Topic A Classification of Solutions
Chemistry 20 Unit 3A Solutions FITB Notes General Outcome: Topic A Classification of Solutions Matter is a substance with and A substance is a type of matter with one definite formula (elements, compounds)
More informationCommon Ion Effect on Solubility
Common Ion Effect on Solubility How is the solubility of a solid affected by other ion species in solution? Why? The solubility product (K sp ) for a salt allows chemists to predict the concentration of
More informationSolubility Products. Solubility Products. Solubility Products. Solubility Products. Slide 2 / 57. Slide 1 / 57. Slide 3 / 57.
Slide 1 / 57 Slide 2 / 57 Products queous equilibria II Products onsider the equilibrium that exists in a saturated solution of aso 4 in water: aso 4 (s) a 2+ (aq) + SO 4 2- (aq) Slide 3 / 57 Products
More informationReactions in Aqueous Solutions
Copyright 2004 by houghton Mifflin Company. Reactions in Aqueous Solutions Chapter 7 All rights reserved. 1 7.1 Predicting if a Rxn Will Occur When chemicals are mixed and one of these driving forces can
More informationCHEMISTRY 202 Hour Exam I. Dr. D. DeCoste T.A.
CHEMISTRY 0 Hour Exam I September, 016 Dr. D. DeCoste Name Signature T.A. This exam contains 3 questions on 11 numbered pages. Check now to make sure you have a complete exam. You have two hours to complete
More informationSemester 1 Review Chemistry
Name Period Date Semester 1 Review Chemistry Units & Unit Conversions Ch. 3 (p. 73-94) PART A SI UNITS What type of measurement is indicated by each of the following units? Choices are in the last column.
More informationChemistry Final Review Worksheet
Chemistry Final Review Worksheet 1. Balance this equation and then write it in words. Al + F 2 ---> AlF 3 N P 2. What does it mean for a molecule to be polar? What are polar molecules able to do? Use the
More informationSOLUBILITY EQUILIBRIA (THE SOLUBILITY PRODUCT)
SOLUBILITY EQUILIBRIA (THE SOLUBILITY PRODUCT) Saturated solutions of salts are another type of chemical equilibria. Slightly soluble salts establish a dynamic equilibrium with the hydrated cations and
More informationChem 42 Final Review Sheet Mr. J. Fassler Spring 2018
Chem 42 Final Review Sheet Mr. J. Fassler Spring 2018 These problems are given to help you review concepts you may have forgotten. Old tests, quizzes and review sheets are also important in studying. Chapter
More informationSaturated vs. Unsaturated
Solubility Equilibria in Aqueous Systems K sp (Equilibria of Slightly Soluble Salts, Ionic Compounds) Factors that Affect Solubility (Common Ion Effect, AcidBase Chemistry) Applications of Ionic Equilibria
More informationScience 1206 Unit 3: Chemical Reactions Page 1 of 15
Science 1206 Unit 3: Chemical Reactions Page 1 of 15 Introduction to Chemical Reactions Notes Part II TEXT p. 218-219 (word equations) There are many chemical reactions too many to count in fact! Like
More informationName of Anion. (aq) NaCl NaNO 3 NaOH Na 2 SO 4 Na2CO3. MgSO4. AgNO 3. Ba(NO 3 ) 2. Pb(NO 3 ) 2. CuSO (1) AgNO 3 ( ) + NaCl( )
Name of Compound Prelab #1 Formula Cation (Metal) Name of Cation silver nitrate Ag Ag + silver magnesium sulfate barium nitrate lead nitrate copper sulfate Cation = (+)positive ion Anion = ()negative ion
More informationChapter 4: Types of Chemical Reactions and Solution Stoichiometry
Chapter 4: Types of Chemical Reactions and Solution Stoichiometry 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition of Solutions (MOLARITY!)
More informationStoichiometry: Chemical Calculations. Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change.
Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change. In order to do this, we need to be able to talk about numbers of atoms. The key concept is
More informationChapter 15 Additional Aspects of
Chemistry, The Central Science Chapter 15 Additional Aspects of Buffers: Solution that resists change in ph when a small amount of acid or base is added or when the solution is diluted. A buffer solution
More informationCHM Electrolytes and the Ionic Theory (r14) Charles Taylor 1/5
CHM 110 - Electrolytes and the Ionic Theory (r14) - 2014 Charles Taylor 1/5 Introduction In 1884, Arrhenius proposed that some substances broke up when dissolved in water to form freely moving ions. We've
More informationSection 6.2A Intermolecular Attractions
Section 6.2A Intermolecular Attractions As we know, molecules are held together by covalent bonds, but there are also attractive forces BETWEEN individual molecules (rather than within). These are called
More informationSolubility Equilibria
Solubility Equilibria Heretofore, we have investigated gas pressure, solution, acidbase equilibriums. Another important equilibrium that is used in the chemistry lab is that of solubility equilibrium.
More informationChemistry. Student Number. Mark / 64. Final Examination Preliminary Course General Instructions. Total Marks 64
Student Number Mark / 64 Chemistry Final Examination Preliminary Course 2003 General Instructions Reading time 5 minutes Working time 120 minutes Write using black or blue pen Draw diagrams using pencil
More informationPart A Answer all questions in this part.
Part A Directions (1-24): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.
More informationUnit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6.
Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6. Formula, Complete, Net Ionic Equations 7. Qualitative Analysis
More informationREVIEW OF BASIC CHEMISTRY ANSWER KEY
REVIEW OF BASIC CHEMISTRY ANSWER KEY 1. Name the following elements. Spelling counts: 2. Write the symbols for the following elements. H hydrogen sodium Na S sulphur phosphorus P Cl chlorine fluorine F
More informationQ1. The electrolysis of sodium chloride solution produces useful substances. (a) (i) Choose a word from the box to complete the sentence.
Q1. The electrolysis of sodium chloride solution produces useful substances. (a) (i) Choose a word from the box to complete the sentence. covalent ionic non-metallic Electrolysis takes place when electricity
More informationMolecules Compounds chemical bonds
Chemical Bonds Molecules are made up of more than one atom. Compounds are made up of more than one element. When atoms combine to make molecules, they form chemical bonds. Types of Bonds: Ionic Bonds Covalent
More informationYear 10 Science Chemistry Examination November 2011 Part A Multiple Choice
Year 10 Science Chemistry Examination November 2011 Part A Multiple Choice Answer these questions on the multiple choice answer sheet provided 2 Isotopes have been found as variations of atoms. Which of
More informationIB Topics 5 & 15 Multiple Choice Practice
IB Topics 5 & 15 Multiple Choice Practice 1. Which statement is correct for this reaction? Fe 2O 3 (s) + 3CO (g) 2Fe (s) + 3CO 2 (g) ΔH = 26.6 kj 13.3 kj are released for every mole of Fe produced. 26.6
More informationChapter 6: Chemical Bonding
Chapter 6: Chemical Bonding Learning Objectives Describe the formation of ions by electron loss/gain to obtain the electronic configuration of a noble gas. Describe the formation of ionic bonds between
More informationChapter Practice Test
Name: Class: Date: Chapter 17-18 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Examining a chemical system before and after a reaction
More informationSpring Semester Final Exam Study Guide
Honors Chemistry Name Period AlCl3 Cu2S NaCN HI PCl3 CrBr3 Naming and Formula Writing 1. Write the name or formula for each of the following: HClO2 (NH4)2SO4 I4O10 H3N NiN H3PO4 Mercury (II) bromide Phosphorous
More informationThe Water Molecule. Draw the Lewis structure. H O H. Covalent bonding. Bent shape
Water & Solutions 1 The Water Molecule Draw the Lewis structure. H O H Covalent bonding. Bent shape 2 Water What determines whether a molecule is polar? Is water a polar molecule? d- d+ d+ 1. Oxygen is
More informationThe electrolysis of sodium chloride solution produces useful substances. covalent ionic non-metallic
1 The electrolysis of sodium chloride solution produces useful substances. (a) (i) Choose a word from the box to complete the sentence. covalent ionic non-metallic Electrolysis takes place when electricity
More informationOperational Skills. Operational Skills. The Common Ion Effect. A Problem To Consider. A Problem To Consider APPLICATIONS OF AQUEOUS EQUILIBRIA
APPLICATIONS OF AQUEOUS EQUILIBRIA Operational Skills Calculating the common-ion effect on acid ionization Calculating the ph of a buffer from given volumes of solution Calculating the ph of a solution
More informationChemistry 40S Chemical Equilibrium (This unit has been adapted from
Chemistry 40S Chemical Equilibrium (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 2 Lesson 1: Defining Equilibrium Goals: Describe physical and chemical equilibrium. Describe the
More informationDraw one line from each solution to the ph value of the solution. Solution ph value of the solution
1 The ph scale is a measure of the acidity or alkalinity of a solution. (a) Draw one line from each solution to the ph value of the solution. Solution ph value of the solution 5 Acid 7 9 Neutral 11 13
More informationSolubility and Complex-ion Equilibria
Solubility and Complex-ion Equilibria Contents and Concepts Solubility Equilibria 1. The Solubility Product Constant 2. Solubility and the Common-Ion Effect 3. Precipitation Calculations 4. Effect of ph
More informationAcid-Base Equilibria and Solubility Equilibria
Acid-Base Equilibria and Solubility Equilibria Acid-Base Equilibria and Solubility Equilibria Homogeneous versus Heterogeneous Solution Equilibria (17.1) Buffer Solutions (17.2) A Closer Look at Acid-Base
More informationIGCSE TEST_ (Ch. 2,3,4,5,6) Name... Date...
IGCSE TEST_ (Ch. 2,3,4,5,6) Name... Date... 1 Winston Churchill, a British Prime Minister, had his false teeth electroplated with gold. The teeth were coated with a thin layer of carbon and were then placed
More informationCHEMICAL REACTIONS. The process by which one or more substances are changed into one or more different substances
CHEMICAL REACTIONS The process by which one or more substances are changed into one or more different substances Equations Reactions are represented by a chemical equation Reactants Products Must have
More informationChapter 4 Compounds and Their Bonds. Octet Rule. Metals Form Positive Ions. Ionic and Covalent Bonds. Formation of a Sodium Ion, Na +
Chapter 4 Compounds and Their Bonds Octet Rule 4.1 Octet Rule and Ions An octet Is 8 valence electrons. Is associated with the stability of the noble gases. Helium (He) is stable with 2 valence electrons
More informationAP Chapter 14: Chemical Equilibrium & Ksp
AP Chapter 14: Chemical Equilibrium & Ksp Warm-Ups (Show your work for credit) Name Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 14: Chemical Equilibrium & Ksp 2 Warm-Ups
More information