Chem 1210 Exam 2

33 flashcards · Biology · by Elsa Schutfort

1. Solution

   a homogeneous mixture of 2 or more substances

2. Solvent

   the substance in the solution present in greatest quantity

3. Solutes

   other substances that are dissolved in the solvent

4. Solution concentration

   the amount of solute dissolved in a given quantity of solvent or solution

5. An aqueous solution is a

   solution where water is the solvent

6. common aqueous solutions of sugar

   glucose, fructose, sucrose, and lactose

7. common aqueous solutions of alcohols

   methanol and ethanol

8. common aqueous solutions of salts

   sodium chloride, potassium chloride, ammonium sulfate, etc

9. common aqueous solutions include

   bases and acids

10. The solution process

    free up individual molecules (solute)n(solute)_n(solute)n​ --> n solute water to water disrupt (water)n(water)_n(water)n​ --> m water Form new solute-water intermolecular forces n solute + m H2OH_2OH2​O --> (solute)n(water)m(solute)_n(water)_m(solute)n​(water)m​

11. Electrolytes

    compounds that dissolve in water to produce IONS Na^+ + Cl^-"> NaCl−−>Na++Cl−NaCl --> Na^+ + Cl^-NaCl−−>Na++Cl−

12. Non-electrolytes

    compounds that dissolve in water BUT do not form ions in solution

13. Strong base (def and ex)

    ionize completely in solution (ex Na^+ + OH^-"> NaOH(s)−>Na++OH−NaOH_(s) -> Na^+ + OH^-NaOH(​s)−>Na++OH− )

14. Weak bases (def and ex)

    ionize only partially in solution (ex NH_{4}^+ -> OH^-"> NH3+H2O−>NH4+−>OH−NH_3 + H_{2}O -> NH_{4}^+ -> OH^-NH3​+H2​O−>NH4+​−>OH− )

15. Salts

    compounds that dissociate in water but ARE NOT ACIDS OR BASES

16. Strong electrolytes

    salts, acids, and bases that dissolve completely or nearly completely in water to form ions (ex H^+ + Cl^-"> HCl−>H++Cl−HCl -> H^+ + Cl^-HCl−>H++Cl− )

17. Weak electrolytes

    compounds that dissolve in water, but produce only a small concentration of ions when dissolved (partial dissociation; partial ionization) (ex CH_{3}OOC^- + H"> CH3COOH−>CH3OOC−+HCH_{3}COOH -> CH_{3}OOC^- + HCH3​COOH−>CH3​OOC−+H )

18. soluble in water

    means a significant amount can dissolve (ex. glucose, NaCl, NaOH, acetic acid, MgSO4MgSO_4MgSO4​ )

19. insoluble in water

    a very little amount dissolves (ex CaCO3,AgCl,C6H12,I2CaCO_3 , AgCl, C_6H_12 , I_2CaCO3​,AgCl,C6​H1​2,I2​ )

20. miscible with water

    soluble at all portions (ex ethanol, glycerol, and formaldehyde)

21. Precipitation Reactions

    Formation of an insoluble salt from the mixing of aqueous solutions of soluble salts

22. Molecular equation

    shows complete chemical formula (ex. AgNO3(aq)+NaCl(aq)AgNO_{3(aq)} + NaCl_{(aq)}AgNO3(aq)​+NaCl(aq)​ )

23. Complete ionic equation

    all soluble salts are shown as ions (ex. AgCl_{s} + Na_{aq}^+ + NO_{3(aq)}^-"> Agaq++NOaq−+Naaq++Claq−−>AgCls+Naaq++NO3(aq)−Ag_{aq}^+ + NO_{aq}^- + Na_{aq}^+ + Cl_{aq}^- -> AgCl_{s} + Na_{aq}^+ + NO_{3(aq)}^-Agaq+​+NOaq−​+Naaq+​+Claq−​−>AgCls​+Naaq+​+NO3(aq)−​ )

24. Net ionic equation

    only ions and molecules directly involved in the chemical reaction (ex. AgCl_{s}"> Agaq++Claq−−>AgClsAg_{aq}^+ + Cl_{aq}^- -> AgCl_{s}Agaq+​+Claq−​−>AgCls​ )

25. Spectator ions

    ions in solution that are not involved in a chemical reaction (ex. Na+Na^+ Na+ and NO3−NO_3^-NO3−​ )

26. Neutralization reactions

    Chemical reactions where acids and baes react with one another

27. potentially part of neutralization reactions

    water and a salt or weak electrolyte is formed A reactant may be solute or insoluble to begin with Sometimes a product is a gas Reactions can be represented by molecular, complete ionic, or net ionic equations

28. Oxidation/reduction reactions

    chemical reactions where electrons are transferred from one reactant to another

29. Molarity

    M = moles solute / Volume of solution (liters) or M = # of particles / defined volume

30. Potential energy

    Energy possessed by resting objects that results from interactive forces with other objects at rest.

31. Electrostatic Potential energy

    Energy of interaction between charged particles held at fixed positions

32. Law of conservation of energy

    Energy is not created or destroyed during any process. It is converted from one from to another.

33. State function

    A function or property whose value depends only on the present state of the system, not the path used to arrive at that condition (ie age, weight, location)