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Understanding Aqueous Reactions and Solution Stoichiometry

Explore the fundamentals of aqueous solutions, including acid-base reactions, precipitation, and oxidation-reduction reactions. Learn about the solute and solvent components in solutions, the characteristics of strong and weak electrolytes, and the methods for calculating concentration and molarity. Understand the principles of solution stoichiometry, including neutralization and displacement reactions. Discover the importance of titration techniques for determining the concentration of unknown solutions and the role of indicators in these reactions.

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Understanding Aqueous Reactions and Solution Stoichiometry

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  1. Aqueous reactions and solution stoichiometry • Aqueous Solutions • Acid and Bases • Precipitation Reactions • Acid-Base Reactions • Oxidation-Reduction Reactions • Concentration • Solution Stoichiometry

  2. Solutions • Solution : A homogeneous mixture of two or more components, consists of two component types • Solvent: major component • Solute: component in the lesser extent • Aqueous Solutions : • Ionic compounds • Molecular compounds • Electrolyte : • Strong electrolytes: strong acid/base, soluble ionic compounds • Weak electrolytes: weak acid/base • Nonelectrolytes

  3. H2O Acid and Base • Acid - a compound that increases [H+] in water ex. HNO3 H+(aq) + NO3-(aq) • Strong acid: HCl, HBr, HI, HNO3, H2SO4, HClO4, HClO3 • Weak acid • Base - a compound that increases [OH-] in water, proton acceptor • Strong base: hydroxide of IA, IIA, LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 • Weak base

  4. Precipitation Reactions • Precipitate • Insoluble product that is formed from a reaction is solution • Solubility: solubility rule, Table 4.1, p. 118 • Exchange reaction (metathesis) AX+BY --> AY + BX • * Exchange reaction will occur when one of the products is insoluble solids, gas, weak or nonelectrolyte • Ionic Equation • Molecular equation • Ionic equation Complete ionic equation, net ionic equation

  5. Acid-Base Reactions • Neutralization reaction Acid + Base --> Salt + H2O Ex. HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O (l) • Acid-base reaction with gas formation Ex HCl (aq) + NaHCO3 (aq) --> NaCl (aq) +H2O (l) + CO2 (g)

  6. Oxidation-Reduction Reactions • Redox reactions: electrons are transferred between reactants • Oxidation: lose electron • Reduction: gain electron • Oxidation state/oxidation number • Assigning oxidation number • Element • Monatomic ion • Nonmetal in compounds • All other • Displacement reaction A + BX --> AX + B • Activity Series: Table 4.5, P.131

  7. Concentration no of moles of solute total volume solution in L Molarity, M = • Concentration: measures how much solute is in a solution • Molarity, M: unit in mol/L • Dilution Mconcx Vconc = Mdil x Vdil

  8. Solution Stoichiometry • Procedure: Fig 4.18, P. 139 • Start with balancing equation • Work with moles • Convert to concentration or volume

  9. Titration • Titration : A method to determine the amount of a substance in solution • Standard solution (titrant): a solution of known concentration • Equivalence point : when just enough titrant is added to the solution • Indicator : a substance changes color at the end point • End point : when indicator changes color • Acid-base titration: to determine the concentration of unknown solution

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