Chapter 2 Water 2019

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Across
  1. 3. The number of electron pairs around an oxygen atom in water
  2. 4. pH is the negative logarithm of the ______ ion concentration.
  3. 5. This type of noncovalent interaction involves electrostatic interactions between permanently charged species.
  4. 7. Maintenance of intracellular ____ is vital to all cells.
  5. 8. This type of noncovalent interaction stabilizes biological macromolecules such as base stacking in DNA. (use as one word)
  6. 9. The _____ effect is one of the main factors behind protein folding.
  7. 14. Weak ______ dissociate only partially in water
  8. 15. True or False: The buffering capacity of acid/anion system is lowest when pH=pKa.
  9. 16. This amino acid can be used as in vivo buffer system
  10. 18. Entropy _____ as ordered crystal lattice is dissolved.
  11. 19. ______ pressure is the force necessary to resist the movement of water from a high water concentration to areas of low water concentration.
  12. 20. Which is more dense, water or ice?
  13. 22. Log(1) = _____
Down
  1. 1. These solutions resist changes in pH.
  2. 2. Water is a good solvent for ______ and polar substances.
  3. 4. This equation can be used to determine the pH of solution from known concentrations of acid and conjugate base solution; The _________-Hasselbalch equation.
  4. 6. This property of water depends on the chemical nature of the solute such as viscosity and surface tension.
  5. 7. The negative logarithm of the acid dissociation constant (Ka).
  6. 10. This property of water does not depend on the nature of the solute such as boiling point and melting point.
  7. 11. This type of noncovalent interaction inovolves electrostatic interactions between uncharged but polar molecules.
  8. 12. This structure results with a high concentration of amphipathic molecules that result from aggregation.
  9. 13. When water dissociates the products are a proton and a ______ ion.
  10. 17. Water is a poor solvent for ______ substances.
  11. 21. True or False: Osmotic pressure is influenced by the concentration of each solute in solution.