1. Solutions and Solubility

2. Solutions formed when substances ____________ in other _____________ _______________ mixtures _______________ phase remain _______________; particles do not _______________ out cannot be separated by _______________ dissolve substances homogeneous single mixed settle filtration

3. Parts of a Solution – solvent: present in _______________ amount ____________ the ____________ to make the solution – solute: present in _______________ amount _______________ in the ______________ larger dissolvessolute lesser dissolvedsolvent

4. LIQUID SOLUTIONS liquid solvent in which a gas, solid, or liquid is dissolved gas dissolved in liquid: –ex. carbonated beverage liquid in liquid: –ex. antifreeze in water miscible: the two liquids mix immiscible: the two liquids don’t mix solid dissolved in a liquid: –ex. salt water Aqueous: water is the solvent Tincture: alcohol is the solvent

5. SOLID SOLUTIONS: alloys: solid mixtures of metals (brass is a mixture of copper and zinc)

6. GAS SOLUTIONS: gases dissolved in each other (air is most common example)

7. Suspension a heterogeneous mixture Particles in the suspension are thousands of times larger than molecules and atoms (ions) Particles will settle out upon standing can be separated by filtration exhibit the Tyndall Effect --the scattering of light in all directions

8. Tyndall Effect Glass on left has colloidial silver, while the glass on the right does not

9. Colloid particles are medium in size between those of suspensions and true solutions particles do not settle out upon standing can not be separated by filtration exhibit the Tyndall Effect

10. Emulsion colloidial dispersion of liquids in liquids emulsifying agent is necessary for maintaining stability (soap is an example)

11. Electrolyte: dissolves in water to form a solution that conducts electricity Nonelectrolyte: dissolves in water to form a solution that does NOT conduct electricity

13. Factors Affecting the Rate of Solution 1) Surface Area : –increasing the surface area of the solute by crushing speeds up dissolving by increasing the number of collisions between the solvent and the solute surface. 2) Agitation: –stirring or shaking helps to disperse solute particles, increasing the number of collisions between the solvent and the solute surface. 3) Heating: –increases the average kinetic energy of the solvent molecules so that collisions between the solvent molecules and the solute are more frequent

14. Solute/Solvent Amounts Saturated: solution containing all the dissolved solute possible at given conditions of temperature and pressure. Unsaturated: solution containing less dissolved solute than the maximum amount that can be dissolved at given conditions of temperature and pressure. Supersaturated: unusual solution containing more dissolved solute than is normally possible at given conditions of temperature and pressure.

15. Solubility A measure of how much solute can dissolve in a given amount of solvent at a specific temperature. –Dilute Solution: The amount of solute dissolved is small in relation to the amount of solvent present. –Concentrated Solution: The amount of solute dissolved is large in relation to the amount of solvent – present.

16. Solubility Rules 1. Salts containing Group I elements are soluble (Li+, Na+, K+, Cs+, Rb+). Exceptions to this rule are rare. Salts containing the ammonium ion (NH 4 + ) are also soluble. 2. Salts containing nitrate ion (NO 3 - ) are generally soluble. 3. Salts containing Cl -, Br -, I - are generally soluble. Important exceptions to this rule are halide salts of Ag +, Pb 2+, and (Hg 2 ) 2+. Thus, AgCl, PbBr 2, and Hg 2 Cl 2 are all insoluble. 4. Most silver salts are insoluble. AgNO 3 and Ag(C 2 H 3 O 2 ) are common soluble salts of silver; virtually anything else is insoluble. 5. Most sulfate salts are soluble. Important exceptions to this rule include BaSO 4, PbSO 4, Ag 2 SO 4 and SrSO 4. 6. Most hydroxide salts are only slightly soluble. Hydroxide salts of Group I elements are soluble. Hydroxide salts of Group II elements (Ca, Sr, and Ba) are slightly soluble. Hydroxide salts of transition metals and Al 3+ are insoluble. Thus, Fe(OH) 3, Al(OH) 3, Co(OH) 2 are not soluble. 7. Most sulfides of transition metals are highly insoluble. Thus, CdS, FeS, ZnS, Ag 2 S are all insoluble. Arsenic, antimony, bismuth, and lead sulfides are also insoluble. 8. Carbonates are frequently insoluble. Group II carbonates (Ca, Sr, and Ba) are insoluble. Some other insoluble carbonates include FeCO 3 and PbCO 3. 9. Chromates are frequently insoluble. Examples: PbCrO 4, BaCrO 4 10. Phosphates are frequently insoluble. Examples: Ca 3 (PO 4 ) 2, Ag 2 PO 4 11. Fluorides are frequently insoluble. Examples: BaF 2, MgF 2 PbF 2.