stoichiometry

• precipitation reaction creates a solid
• acid-base reaction has an acid and base can neutralize
• redox reaction single replacement
• preciptation

  • double replacement
  • net ionic equation
  • solubility
  • 2 ionic compounds / aqueous solutions -> an aqueous solution and precipitate
• the soluble product ions are called spectator ion
• molecular equation (balanced equation) -> total ionic equation (write the charges and cancel anything same on both sides) -> net ionic equations ( for solid only)
• same stoichiometry expect you have to write the balanced net ionic equation IF and ion is mentioned
• Acid = H+ donor (H+)

  Base = H+ acceptor (usually OH-)

  Neutralization reaction:

  Acid + base -> Salt + water
• find limited reactant and USE the moles of the limiting reactant for ALL calculations
• • Titrant-solution of known concentration used in titration
• • Analyte- substance being analyzed
• • Equivalence point- enough titrant added to react exactly with the analyte (moles of acid=moles of base)
• • Neutralization means @ equivalence point
• • End point- indicator change color so you can tell the equivalence point has been reach
• acid base titiration:

  1. titrate put into burette
  2. put analyte into beaker/flask
  3. add acid-base indicator into beaker
  4. titrate in burette will slowly drip into beaker
  5. stop when change color = equivalence point = when pH changes
  6. titration can happen at any point so pick the pH where you want it to titrate
• titration calculations

  • Net ionic equation for moles
  • M of analyte = (Mtitrate x Vtitrate) / Vanalyte
• redox reaction = reduction and oxidation reaction are happening simultaneously
• OIL RIG:

  reduction = a gain or e-

  oxidation = a loss of e-
• How do you balance redox reactions in acidic solutions?


  Use half-reaction method
• What are the steps to balance redox reactions in basic solutions?


  1. Balance as in acidic
  2. Add OH equal to H (both sides)
  3. Form water by combining H and OH
  4. Check elements and charges for balance
• oxidation number

  • element = zero
  • ions (ionic compound) = charge of ion
• oxidation number IN A COMPOUND

  • group 1 = +1
  • group 2 = +2
  • oxygen = -2 EXCEPT in H202(peroxide) -> -1
  • hydrogen = +1 EXCEPT with group 1 or 2 -> -1
  • halogens = -1 EXCEPT with element with higher electronegativity
  • ex: clo3 = 5 = x + (-2x3) = -1
• Balancing Redox solution

  1. half equation
  2. balance the element other than O or H
  3. balance O by adding H2O
  4. balance h by adding H+
  5. balance the charges by adding elections
  6. put them together and balance the electrons
• solubitlty rule:

  • Group 1
  • ammonium, Nitrates, acetates
  • Halogens are soluble except with Ag⁺, Pb²⁺, and Hg₂²⁺
  • strong acid and base
  • Sulfates are soluble except with Ba²⁺, Sr²⁺, Pb²⁺, or Ca²⁺
• more solubility rules

  1.Nitrate and acetate (C2H5O2-) salts are soluble

  2. Alkali (group1) salts and NH4+ are soluble

  3. Halide salts are soluble (NOT Ag+, Pb+2, Hg22+)

  4. Sulfates salts are soluble (NOT BaSO4, PbSO4, HgSO4,

  CaSO4, SrSO4)

  5. OH- salts are insoluble (strong bases are soluble)

  6. Most S-2, CO32-, CrO42-, PO43- salts are insoluble

  7. Strong acids are soluble