May 09, Ksp.notebook. Ksp = [Li + ] [F + ] Find the Ksp for the above reaction.

Size: px

Start display at page:

Download "May 09, Ksp.notebook. Ksp = [Li + ] [F + ] Find the Ksp for the above reaction."

Samson Harvey
5 years ago
Views:

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

10. REACHING EQUILIBRIUM. Initially, the dissolving (forward) reaction is faster. As more sodium chloride dissolves, what happens to the number of ions in solution?

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

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