1 / 6

Solubility Rules

Solubility Rules. Steps for Net Ionic Equations. Write the chemical formula equation. Decide which are strong electrolytes and put a line between the anion and the cation. Also, show the charge of the ion.

sonora
Télécharger la présentation

Solubility Rules

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. Solubility Rules Mullis

  2. Steps for Net Ionic Equations • Write the chemical formula equation. • Decide which are strong electrolytes and put a line between the anion and the cation. Also, show the charge of the ion. • If the species is not a strong electrolyte, draw a box around it so you will remember to leave it as a compound. • Cancel the spectator ions. Mullis

  3. Net ionic equations (quick way) • Includes only those compounds and ions that undergo chemical change in a reaction in an aqueous solution. • Ions that do not take part in the reaction and are found in solution both before and after are spectator ions. Ex: Pb(NO3)2 + 2KCl PbCl2+ 2KNO3 All are soluble except lead(II)chloride, so: Pb2+/ NO3- + K+/Cl- PbCl2 + K+/NO3- Net ionic equation (cross out spectators on both sides): Pb2+ + 2Cl- PbCl2 Mullis

  4. Net ionic equations (textbook way) • Includes only those compounds and ions that undergo chemical change in a reaction in an aqueous solution. • Ions that do not take part in the reaction and are found in solution both before and after are spectator ions. Ex: Zinc nitrate and ammonium sulfide make a solid precipitate, ZnS. Zn(NO3)2 (aq) + (NH4)S (aq) ZnS(s) + 2NH4NO3 (aq) Overall ionic equation: Zn2+ + 2NO3- + 2NH4 + + S2- ZnS + 2NH4+ + 2NO3- Net ionic equation (cross out spectators on both sides): Zn2+ + S2- ZnS Mullis

  5. Net ionic equations--Examples Potassium sulfate and barium nitrate make a solid precipitate, BaSO4. K2SO4 (aq) + Ba(NO3)2(aq) BaSO4(s) + 2KNO3 (aq) Overall ionic equation: 2K++ SO42- +Ba2+ + 2NO3- BaSO4 + 2K+ + 2NO3- Net ionic equation (cross out spectators on both sides): SO42- +Ba2+ BaSO4 Mullis

  6. HNO3 and NaOH are mixed in chemically equivalent quantities. What is the correct formula equation, overall ionic equation and net ionic equation? HNO3(aq) + NaOH(aq) NaNO3(aq) + H2O (l) Overall ionic equation: H3O+ + NO3- +Na+ + OH- Na+ + NO3- + 2H2O (l) Net ionic equation (cross out spectators on both sides): H3O+ + OH- 2H2O (l) Mullis

More Related