University:
Massachusetts Institute of Technology
Course:
1.76 | Aquatic Chemistry
Academic year:

2021
Views:

342

Pages:

2
Author:

Trevon Carney

Answers to 1.76 Practice Problems 1 1) 5.0 2) 4.0 3) 3.0 4) 9.0 5) 10.0 6) 11.0 7) 7.0 8) 6.8 9) 6.5 10) 5.0 11) 4.2 12) 3.5 13) 9.0 14) 9.8 15) 10.4 16) Name Chem Formula Species formed in aqueous sol’n Acid/ Base/ Ampi/ Salt potassium chloride KCl potassium ion, K+ chloride, Cl- salt (very soluble, >10g/100mL, KCl (aq) formation unlikely) nitric acid HNO3 calcium sulfate CaSO4 hydrogen ion, H+ nitrate, NO3calcium ion, Ca2+ sulfate, *SO42CaSO4 (aq); (slightly soluble, log Ksp = -4.2) acid salt (*can act as a base, however, no HSO4- formation,HSO4- << SO42- in neutral waters, pKa= 2.0) calcium hydroxide CaOH2 hydroxide, OHcalcium ion, Ca2+ basic calcium carbonate CaCO3 basic ammonium acetate ammonium nitrate CH3COONH4 calcium ion, Ca2+ carbonate, CO32carbonate + H+ ↔ bicarbonate: CO32-+ H+ ↔ HCO3- (pKa=10.33) acetate + H+ ↔ acetic acid: CH3COO- + H+ ↔ CH3COOH ammonium ↔ ammonia + H+: NH4+ ↔ NH3 + H+ nitrate, NO3ammonium, *NH4+ (*can act as an acid, however, pKa= 9.2, so will hydrogen sulfide sodium nitrite H2S NH4NO3 amphiprotic, a buffer, stabilizes the pH over a given capacity salt NOT dissociate significantly in neutral waters) hydrogen sulfide↔ bisulfide + H+, H2S↔ HS- + H+ (sulfide, S NaNO2 2- - 2- acid + not formed significantly, HS ↔ S + H , pKa=12.9) sodium ion, Na+ nitrite, NO2- (no HNO2 formation; HNO2 << NO2- in neutral waters, pKa= 3.3) Refs: Umland & Bellama, General Chemistry, 3rd Edition, Brooks/Cole Publishing, 1999 Morel & Hering, Principles and Applications of Aquatic Chemistry, Wiley & Sons, 1993 salt

Answers to 1.76 Practice Problems 1

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