15. A demonstration Pb(NO 3 ) 2 (aq) + KI(aq) There are four different ions in the mix. Visualize the collisions.
16. Which collisions will result in a weak ionic bond easily broken by another collision? Which collisions will not even occur due to repulsions between the ions? Which collisions will form strong ionic bonds and clumps of ions visible as a cloudy precipitate? Pb(NO 3 ) 2 (aq) + 2 KI(aq) 2 KNO 3 (aq) + PbI 2 (s)
17. Visualizing the Double Replacement Reaction Ionic equations show the ions in solution AgNO 3 (aq) + NaCl(aq) NaNO 3 (aq) + AgCl(s) Ions in solution are actually dissociated or separated. In the solid the ions are together Ag + (aq) + NO 3 - (aq) + Na + (aq) + Cl - (aq) Na + (aq) + NO 3 - (aq) + AgCl(s) Notice Na + and NO 3 - ions have not changed. They are spectator ions. Net ionic equation leaves out the spectator ions. Ag + (aq) + Cl - (aq) AgCl(s)
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19. Write the balanced equation for this double replacement reaction. Which collisions will result in a weak ionic bond easily broken by another collision? Which collisions will not even occur due to repulsions between the ions? Which collisions will form strong ionic bonds and clumps of ions visible as a cloudy precipitate? Write the net ionic equation for the reaction.
20. Write the balanced equation for this double replacement reaction. Which collisions will result in a weak ionic bond easily broken by another collision? Which collisions will not even occur due to repulsions between the ions? Which collisions will form strong ionic bonds and clumps of ions visible as a cloudy precipitate?
21. Write the balanced equation for this double replacement reaction. Which collisions will result in a weak ionic bond easily broken by another collision? Which collisions will not even occur due to repulsions between the ions? Which collisions will form strong ionic bonds and clumps of ions visible as a cloudy precipitate? How is this solution at equilibrium and saturated?
24. Gravimetric Analysis- A quantitative analysis of a double replacement reaction The solid produced in the reaction is isolated by filtering and rinsing. After the filter and solid are dried, the mass of the barium sulfate is measured.
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29. Write equations (molecular, total and net ionic) for the reaction shown above. Explain the formation of the precipitate and the ions remaining in solutions by describing the collisions and attractions.
30. Ions in solution are dissociated attracted to the water by ion-dipole attractions. While ions in the precipitate held in fixed positions by ionic bonds between the ions H 2 O
31. Precipitation Reactions Precipitate – insoluble solid that separates from solution net ionic equation Na + and NO 3 - are spectator ions “ If you’re not a part of the solution, then you’re a part of the precipitate!” Pb 2+ + 2NO 3 - + 2Na + + 2I - PbI 2 ( s ) + 2Na + + 2NO 3 - Pb(NO 3 ) 2 ( aq ) + 2NaI ( aq ) PbI 2 ( s ) + 2NaNO 3 ( aq ) precipitate Pb 2+ + 2I - PbI 2 ( s )
32. Chemistry In Action: An Undesirable Precipitation Reaction CO 2 ( aq ) CO 2 ( g ) Ca 2+ ( aq ) + 2HCO 3 ( aq ) CaCO 3 ( s ) + CO 2 ( aq ) + H 2 O ( l ) -
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34. Total Ionic Equations Molecular Equation: K 2 CrO 4 + Pb(NO 3 ) 2 PbCrO 4 + 2 KNO 3 Soluble Soluble Insoluble Soluble Total Ionic Equation: 2 K + + CrO 4 -2 + Pb +2 + 2 NO 3 - PbCrO 4 (s) + 2 K + + 2 NO 3 -
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