Solubility Rules and Precipitation Reactions

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Presentation transcript:

Solubility Rules and Precipitation Reactions

Factors Affecting Solubility

Surface Area More solute/solvent contact means faster dissolving Crush substance into fine powder Use mortar and pestle

Stirring or Agitation: More solute/solvent contact (solids/liquids) However, stirring disturbs dissolved gases and they come out of solution.

Temperature of Solvent Higher temperatures will allow more solid solutes to dissolve

Gases dissolve better when solvent temperature is colder. Ex: CO2 gas in hot soda (flat) vs. cold soda (fizzy)

Pressure Effects gas solubility only Why? Increasing pressure on a gas above a liquid causes more gas molecules to be “pushed” into solution. Ex: CO2(aq) in soda

Nature of Solute and Solvent Polar solutes dissolve in polar solvents Nonpolar solutes dissolve in nonpolar solvents Most ionics (but not all) dissolve in polar solvents (molecule-ion attractions)

Not all ionic compounds dissolve! Instead of doing experiments all the time to see which ones will dissolve, we use The solubility rules.

Solubility Rules All nitrates (NO3-) are soluble. All ammonium (NH4+) or alkali (Li+, Na+, K+, Rb+, Cs+, Fr+) compounds are soluble. All carbonates (CO32-), phosphates (PO4 3 -) and hydroxides (OH-) are insoluble except with the cations in Rule #2. 4. All chlorides (Cl-), bromides (Br-), and iodides (I-), are soluble except with Ag+, Pb2+, or Hg+. 5. All sulfates (SO42-) are soluble except with Ca2+, Sr2+, Ba2+, Ra2+, Pb2+,

Which of the following are soluble in water? SrSO4 b. NaNO3 c. PbCl2 Not soluble soluble Not soluble

Precipitation Reactions When a solid doesn’t dissolve it is called insoluble. A solid that forms when two solutions are mixed is called a precipitate.

Precipitates Precipitates are insoluble ionic compounds formed in double replacement reactions. Determine which product is the insoluble precipitate by using your rules.

When a precipitate forms, you create a heterogeneous mixture. You can separate a precipitate by filtration. The solid will stay on the paper.

Predict the products of the following reaction: (if no solid precipitate is formed, there is no reaction) Pb(NO3)2(aq) + KI (aq) → Pb(NO3)2(aq) + 2KI (aq) → PbI2(s) + 2KNO3 (aq) We know it is a solid precipitate because it is insoluble according to the solubility rules.

Net Ionic Equation Write the balanced chemical and net ionic equation for: Na2CO3(aq) + CaCl2(aq) → Step 1: Write the balanced chemical equation Na2CO3(aq) + CaCl2(aq) → CaCO3(s) + 2NaCl (aq) Step 2: Remove the spectator ions (those that are soluble). Ca2+(aq) + CO32-(aq) → CaCO3(s) Insoluble precipitate