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Chemistry Review: Solutions, Acids/Bases, Kinetics, and Equilibrium

This review covers topics such as solutions, acids and bases, kinetics, and equilibrium in chemistry. It includes concepts like activation energy, colligative properties, dissociation, electrolytes, pH, salt solubility, and more.

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Chemistry Review: Solutions, Acids/Bases, Kinetics, and Equilibrium

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  1. Chemistry Review 5 Solutions Acids/Bases Kinetics and Equilibrium

  2. Arrhenius acid Arrhenius Base Activation energy catalyst Colligative Properties Dissociation Electrolyte equilibrium Heat of Reaction Hydrogen ion Hydronium ion Hydroxide Indicator Neutralization pH Potential Energy Diagram Salt Solubility Solute Solvent Today’s vocab

  3. An ionic compound containing positive ions other than hydrogen and negative ions other than hydroxide

  4. Salt

  5. The graph displaying the changes of energy during a chemical reaction, indicating energy levels of reactants and products, and energy of activation for both exothermic and endothermic reactions.

  6. Potential Energy Diagram

  7. The minimum energy required to initiate a reaction

  8. Activation energy

  9. The minimum energy required to initiate a reaction

  10. Activation energy

  11. Properties of matter that depend more upon the number of particles than upon their characteristics

  12. Colligative Properties

  13. A dynamic chemical state in a reversible reaction in which the forward and reverse reaction rates are equal and the concentrations remain the same

  14. Equilibrium

  15. A substance that changes the activation energy required and thus affects the rate of a chemical reaction

  16. Catalyst

  17. substance that yields hydrogen (H+) ions as the only positive ions in aqueous (aq) solution

  18. Arrhenius Acid

  19. measures concentration in moles of solute per liter of solution

  20. Molarity

  21. reaction in which the products contain less energy than the reactants; energy change ∆H is negative

  22. exothermic

  23. substance that yields hydroxide ions (OH-) as the only negative ions in aqueous solution.

  24. Arrhenius Base

  25. have a pH less than 7. • will react with certain metals to liberate hydrogen gas. • cause color changes in acid-base indicators. • react with hydroxides to form water and a salt. • Dilute aqueous solutions have a sour taste. • Aqueous solutions of these conduct electricity.

  26. Acids

  27. The formation of ions; the separation of the ions in an ionic compound

  28. Dissociation

  29. reaction in which the products contain more energy than the reactants; energy change ∆H is positive

  30. Endothermic reaction

  31. A water molecule with a positive charge due to the presence of an additional hydrogen ion: H3O+

  32. Hydronium ion

  33. Acids Give H+ in sol’n pH < 7 Taste sour React with active metals to give H2 Bases Give OH- in sol’n pH > 7 Taste bitter Slippery

  34. Salts: ionic substance with neither H+ nor OH- ions Not always neutral Are electrolytes

  35. Neutalization • Acid + Base  salt + water • Titration: add known to unknown such that # H+s = # OH-s • Ma X Va = Mb X Vb

  36. Solutions

  37. Metals lose e’s  become smaller ions • Nonmetals gain e’s  become bigger ions

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