Aquatic Chemistry

1. “always add _______ to water, never the reverse” (lab safety rule)
2. the graduated cylindrical glassware that will be used to dispense the acid into water for the lab
3. the ion product constant of water
4. N2 -> NH4+ (nitrogen fixation) is an example of a ___________ redox reaction
6. this legislation significantly helped improve air quality and reduce acid rainfall in the northeast USA
10. loss of electrons; often oxygen-rich
12. lowest energy yield on a REDOX ladder producing “biogas”
15. the name of the Adirondack Lake we will compare our pH and alkalinity water values with today
16. determining concentration by slowly adding a solution until a reaction endpoint is reached
18. the strong acid you will titrate with today
19. microscopic living organisms that drive nutrient cycling

1. the ability of water to neutralize or buffer acid
2. carbon system (multiple carbon forms) that buffers pH in water
5. a basic substance has a high concentration of this
7. rain precipitation usually made by sulfur and nitrogen pollution in the atmosphere
8. a change in pH can alter the solubility of __________ in water
9. negatively charged ion made of one carbon and three oxygen atoms; important in buffering water
11. involves the transfer of electrons, releases energy, and can lead to oxygen depletion in lakes and wetlands
13. in lab, you must add an acid until the pH is below _______ to create your titration curve
14. shock – a sudden drop in a lake’s pH, often occurring in spring snow melt season, when accumulated acidic compounds from snow are rapidly released
17. concentration of hydrogen ions in an aqueous solution