1 / 9

Solubility Rules

Solubility Rules. #2 Rule. #1 Rule. [Exceptions]. Metathesis (Double Displacement). A X + B Y AY + BX. Acid-Base neutralization A =H + X=anion of the acid B Y =Base H Cl + Na OH H 2 O + NaCl.

mmercado
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 #2 Rule #1 Rule [Exceptions]

  2. Metathesis (Double Displacement) AX + BYAY + BX Acid-Base neutralization A=H+ X=anion of the acid BY=Base HCl + NaOHH2O + NaCl note: In the case of ammonia: AX + YAY + X HCl+NH3NH4+ +Cl-

  3. Precipitation Reactions (metathesis) AX + BYAY(s) + BX AX=Soluble Salt BY=Soluble Salt AY=Insoluble Solid (precipitate,ppt) BX=Soluble Salt AgNO3 + NaClAgCl(s) + NaNO3 Formula unit Ag++NO3- + Na+ + Cl-AgCl(s) + Na+ + NO3- Total Ionic Ag++ Cl-AgCl(s) Net Ionic Spectator Ions = nitrate ions and sodium ions

  4. Fe(NO3)3 + 3NaOH Fe(OH)3(s) + 3NaNO3 Fe3+ + 3NO3- + 3Na+ + 3OH- Fe(OH)3(s) + 3NO3- + 3Na+ Fe3+ + 3OH- Fe(OH)3(s)

  5. Will a precipitate form if we add solid Calcium Nitrate and solid Potassium Carbonate to water? Ca(NO3)2 Ca2+ + 2NO3- K2CO3 2K+ + CO32- Ca2+ NO3- K+ CO32- Ca(NO3)2 + K2CO3 CaCO3(s) + 2KNO3 Formula Unit Ca2+ + 2NO3- + 2K+ + CO32- CaCO3(s) + 2NO3- + 2K+ Total Ionic Ca2+ + CO32- CaCO3(s) Net Ionic Spectator ions: nitrate ions and potassium ions

  6. Oxidation State (Oxidation Number) 2Na(s) 2Na+(aq) + 2e- oxidation 1/2 reaction 2H2O + 2e- 2OH-(aq) + H2(g) reduction 1/2 reaction 2Na(s)+2H2O2NaOH(aq)+H2(g) redox reaction oxidation-loss of electrons reduction-gain of electrons reducing agent-compound that is oxidized (Na(s)) oxidizing agent-compound that is reduced (H2O) We need an accounting system-oxidation state

  7. Oxidation State Rules • The oxidation state of any atom in a free uncombined element is zero (Cl2, H2, O2, P4, Na(s) ... ) • The oxidation state of any monatomic ion is equal to the charge (Na+ ox. state = +1 ; Cl- ox. state = -1 ; Fe2+ ox. state = +2) • The sum of oxidation numbers of all atoms in a compound is zero • The sum of oxidation numbers of all atoms in an ion is equal to the charge of the ion (SO42- sum of ox. numbers = -2)

  8. 1 2 3 4 5 6 7 8

  9. -2 +1 0 -2 2Na(s) + 2H2O2NaOH(aq) + H2(g) +1 +1 0 H2O 2*(+1) + X = 0 X= -2 for O in H2O NaOH (+1) + (+1) + X = 0 X=-2 for O in NaOH OH-- (+1) + X = -1 X=-2 for O in OH- Oxidation-increase in the oxidation state (number) Na(s) 0 +1 Reduction-decrease in the oxidation state (number) H +1 0

More Related