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1. How much 12 M HCl would you need to prepare 500 mL of 1 M HCl? 2. How would you actually prepare such a dilution? I would add Day 2 1-7 Slide 2 Slide 3 If you dissolve 117 grams of NaCl in 4000 mL, what is the resulting molarity of your solution? Day 3 1-8 period 1 Slide 4 If you dissolve 234 grams of NaCl in 500 mL, what is the resulting molarity of your solution? Day 5 1-13 both periods Slide 5 A.Molecular equation Substances are written in their compound or molecular form. AgNO 3 (aq) + KCl (aq) AgCl (s) + KNO 3 (aq) AgCl (s) + KNO 3 (aq) 5 Notes page 3 Slide 6 B.Complete ionic equation All strong electrolytes (strong acids, strong bases, and soluble ionic salts) are dissociated into their ions. This more accurately reflects the species that are found in the reaction mixture. 6 Slide 7 B.Complete ionic equation Ag + (aq) + NO 3 - (aq) + K + (aq) + Cl - (aq) AgCl (s) + K + (aq) + NO 3 - (aq) AgCl (s) + K + (aq) + NO 3 - (aq) 7 Slide 8 C.Net ionic equation Only active ions and molecules are included. Ag + (aq) + Cl - (aq) AgCl (s) 8 Slide 9 Ag + (aq) + NO 3 - (aq) + K + (aq) + Cl - (aq) AgCl (s) + K + (aq) + NO 3 - (aq) Net Ionic Equation To form the net ionic equation, cross out anything that does not change from the left side of the equation to the right. The only things left in the equation are those things that change (i.e., react) during the course of the reaction. Those things that didnt change (and were deleted from the net ionic equation) are called spectator ions. 9 Slide 10 D.Spectator ions Non-reactive ions that didnt change (and were deleted from the net ionic equation) NO 3 - (aq) + K + (aq) 10 Slide 11 E.Questions and considerations when writing ionic equations 1. Is the substance __________ ? (_____________ or ____) 2. Is the substance a strong or weak ____________? insoluble precipitategas electrolyte 11 Slide 12 3. These types of substances are written as ions: 4. These types of substances are written as molecules: strong acids, strong bases, soluble ionic compounds weak acids, weak bases, insoluble ionic compounds, nonelectrolytes 12 Slide 13 1. How much 9 M H 2 SO 4 would you need to prepare 450 mL of 3 M H 2 SO 4 ? 2. How would you actually prepare such a dilution? I would add Day 6 1-14 Slide 14 F. Ex: Write the molecular, complete ionic, and net ionic equations for the reaction of solutions of aluminum sulfate and calcium nitrate. Al 2 (SO 4 ) 3(aq) + 3Ca(NO 3 ) 2(aq) 2Al(NO 3 ) 3(aq) + 3CaSO 4(s) 2Al +3 (aq) + 3SO 4 -2 (aq) + 3Ca +2 (aq) + 6NO 3 - (aq) 2Al +3 (aq) + 6NO 3 - (aq) + 3CaSO 4(s) 3SO 4 -2 (aq) + 3Ca +2 (aq) 3CaSO 4(s) 14 Slide 15 #s 19, 20, 22-24 on page 531 Slide 16 How many grams do you need for 50 mL of a 0.1M solution Slide 17 Write a molecular, complete ionic, and net ionic equation for the precipitation reaction between lead II nitrate and potassium iodide (the precipitate is lead II iodide. Day 5 2-19 Pb(NO 3 ) 2(aq) + 2KI (aq) 2KNO 3(aq) + PbI 2(s) Pb (aq) +2 + 2NO 3(aq) - + 2K (aq) + + 2I (aq) - 2K (aq) + + 2NO 3(aq) - + PbI 2(s) Pb (aq) +2 + 2I (aq) - PbI 2(s) Slide 18 1. Molarity, M or M a. Most widely-used unit of __________________ b. Formula concentration M = # mols of solute # L of solution Slide 19 D. Dilution is adding more ________ to a solution to reduce the ________________. 1. Used to prepare solutions from _______________ solutions. 2.Formula solvent concentration stock or conc. V c M c = V d M d (Volume of Conc.)(M Conc.) = (Volume of Dilute)(M of Dilute soln) 19 Slide 20 A.A solute that forms ions in solution and conducts ____________ is known as an _____________, while a solute that neither forms ions nor conducts ____________ is known as a ________________. electricity electrolyte electricity nonelectrolyte 20 Slide 21 21 Slide 22 22 Slide 23 B.Ionic compounds and some molecular compounds ____________ in water. 1.Strong electrolytes produce a _______ number of ions. 2. Weak electrolytes produce a _________ number of ions. dissociate larger smaller 23 Slide 24 24 Slide 25 C.Most molecular compounds _________ in water and are called _______________. D.Solubility does not determine if a solute is a strong or weak electrolyte. 1. Acetic acid: _____ solubility + ______ electrolyte disperse nonelectrolytes Only 1% is H + + C 2 H 3 O 2 - in soln, rest is HC 2 H 3 O 2 highweak Equilibrium: HC 2 H 3 O 2(aq) H + (aq) + C 2 H 3 O 2 - (aq) 25 Slide 26 2. Barium hydroxide: ____ solubility + ________ electrolyte E. Solvation is the surrounding of _______ particles by particles of the ________. Known as ___________ when water is the solvent. lowstrong Not very soluble but everything that dissolves dissociates solute solvent hydration 26 Slide 27 A. Acids 1. Able to ionize and form ___ in aqueous solutions 2. Often referred to as ________ donors 3. Decrease the concentration of _____ in aqueous solutions H+H+ proton 27 OH - Slide 28 4. Monoprotic acids release ____ ___ per molecule of acid. Ex: 5. Diprotic acids release _____ ___ per molecule of acid. Ex: oneH+H+ HCl, HNO 3, HC 2 H 3 O 2 28 twoH+H+ H 2 SO 4 H 2 SO 4(aq) HSO 4(aq) + H + (aq) HSO 4(aq) SO -2 4(aq) + H + (aq) Only some of 2 nd H + come off 1 st H + always comes off Slide 29 6. Strong acids 7. Weak acids - completely ionize in H 2 O chloric, hydrobromic, hydrochloric, hydroiodic, nitric, perchloric, sulfuric - partly ionized in H 2 O, most acids are weak acetic, hydrofluoric, carbonic 29