1 / 9

Double Replacement Reactions

Double Replacement Reactions. How do we know if these happen?. Double Replacement Reaction. 2 KI (aq) + Pb(NO 3 ) 2(aq)  2 KNO 3(aq) + PbI 2(s). Double Replacement Reactions. Two types of Double Replacement Reactions: Formation of an insoluble precipitate

emile
Download Presentation

Double Replacement Reactions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Double Replacement Reactions How do we know if these happen?

  2. Double Replacement Reaction 2 KI(aq) + Pb(NO3)2(aq) 2 KNO3(aq) + PbI2(s)

  3. Double Replacement Reactions • Two types of Double Replacement Reactions: • Formation of an insoluble precipitate • NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s) • Formation of a gas • Acid + salt → gas + another salt • H2SO4(aq) + Na2S(aq) → H2S(g) + Na2SO4(aq)

  4. Solubility Rules • All sodium, potassium, and ammonium salts are soluble • All acetate, nitrate, and chlorate salts are soluble • All halide salts (F, Cl, Br, I) are soluble • Except lead (II), silver, and mercury (I) • All sulfates are soluble • Except calcium, barium, lead (II), and silver • All carbonates, phosphates, and sulfides are INSOLUBLE • Except sodium, potassium, ammonium

  5. Ionic Equations • Since ionic compounds (salts) exist as ions in solution, a precipitation reaction can be shown as ions: • NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s) • Na+(aq) + Cl-(aq) + Ag+(aq) + NO3-(aq) → Na+(aq) + NO3-(aq) +AgCl(s) • This is the ionic equation for the reaction • Be careful with coefficients and subscripts from balanced formula equations

  6. Net Ionic Equations • Na+(aq) + Cl-(aq) + Ag+(aq) + NO3-(aq) → Na+(aq) + NO3-(aq) +AgCl(s) • Na+ and NO3- ions are on both side, so they can be cancelled: • Cl-(aq) + Ag+(aq) → AgCl(s) • Na+ and NO3- are spectator ions • They are soluble on both sides of the ionic equation • The net ionic equation shows the reaction without the spectator ions • The net ionic equation shows which ions react and how the reaction occurs

  7. For the following sets of reactants… • Predict if a reaction will occur, based on solubility rules • Write a balanced formula equation, if the reaction occurs • Write a balanced ionic equation, if the reaction occurs • Write a balanced net ionic equation, if the reaction occurs

  8. Double Replacement Reactions • Potassium chromate + silver nitrate • Sodium hydroxide + iron (III) chloride • Sodium nitrate + calcium chloride • Lead (II) acetate + potassium sulfate • Silver nitrate + magnesium sulfate • Potassium hydroxide + nitric acid • Sodium acetate + potassium carbonate

More Related