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chapter 4; reactions in aqueous solutions

Chapter 4; Reactions in Aqueous Solutions. MolarityAcid-Base TitrationsDilution of Solutions. 4.1. A solution is a homogenous mixture of 2 or more substances. The solute is(are) the substance(s) present in the smaller amount(s). The solvent is the substance present in the larger amount. In aqueous solutions (aq)*solvent is water*solute can be ionic compounds, aqueous acids, bases, or molecular compounds.

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chapter 4; reactions in aqueous solutions

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    1. Chapter 4; Reactions in Aqueous Solutions Electrolytes vs. NonElectrolytes Precipitation Reaction Solubility Rules Reactions of Acids Neutralization Acid and Carbonate Acid and Metal Metal and Water

    5. 4 Types of Inorganic Compounds Molecular; Made of 2 or more Nonmetals Ionic; Made of + and – ion. Generally + ion is from metal and – ion from nonmetal. Bases; + ion; - ion is hydroxide (OH)- Aqueous Acid; H+ and – ion dissolved in water. Generally – ion is nonmetal

    6. Inorganic Compounds Dissolved in WaterALL BUT MOLECULAR PRODUCE IONS

    8. Electrolytic Solutions Contain Mobile Cations (+) and Anions(-) Ionic Compounds, Aqueous Acids, and Base Dissociate Into the Ions They are Made of When Dissolved in Water. NaCl (s) ? Na+ (aq) + Cl-(aq) More Ions in Solutions; Stronger Electrolyte

    10. Precipitation Reactions Mix two aqueous solutions made by dissolving ionic compounds in water. If a reaction happens, a precipitate (solid) is formed.

    12. Predicting Products of Precipitation Reactions Ionic Compounds are Strong Electrolytes –Determine charge on all ions of reactants Using Ion Charges; Predict formula of products. ( + ion of one reactant forms compound with – ion of other reactant) Balance Equation Determine is product is solid or aqueous solution

    14. Predicting Products of Precipitation Reactions (Cont) Determine spectator ions (Ions that are still dissolved in water in the product) Write net ionic equation (Only shows ions involved in forming solid)

    18. Acids Produce H+ (proton) or (H3O)+ when dissolved in water Proton donor

    20. Bases

    21. Neutralization Reaction Acid + Base -> Salt + H2O

    22. Acid + Carbonate -> Salt + CO2(g) + H2O (l) Carbonate; Contains (CO3)-2 or (HCO3)- Chalk; Ca(CO3)

    23. Displacement Reactions – Metal Displaces H from acid or water Metal + Acid -> Salt + H2 (g) Metal + Water -> Base + H2(g) Use Activity Series to Know if a Reaction Will Happen

    24. Activity Series

    27. Acid/Base Titrations Experimental technique that determines the concentration (in Molarity) of an acid (or base) This is based upon an acid/base neutralization reaction. ACID +BASE -> SALT + H2O Base (or acid) is added until there is the same amount (same # moles) of base and acid.

    31. At the endpoint of an acid/base titration…. Moles acid = Moles base (MV)acid = (MV)base Note If solid; moles = mass/ MM If aqueous solution; moles = MV

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