Acids & Bases Flashcard
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| HCl |
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| (Strong Acid) Hydrochloric Acid H+(aq) + Cl-(aq) |
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| HBr |
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| (Strong Acid) Hydrobromic acid H+(aq) + Br-(aq) |
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| HI |
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| Strong Acid (Hydroiodic acid) H+(aq) + I-(aq) |
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| H2SO4 |
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| Strong Acid (Sulfuric acid) H+(aq) + HSO4-(aq) (HSO4- is a weak acid that contributes additional protons) |
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| HNO3 |
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| (Strong Acid) Nitric acid H+(aq) + NO3-(aq) |
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| HClO3 |
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| (Strong Acid) Chloric acid H+(aq) + ClO3-(aq) |
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| HClO4 |
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| (Strong Acid) Perchloric acid H+(aq) + ClO4-(aq) |
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| NaOH |
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| Strong Base (Sodium hydroxide) Na+(aq) + OH-(aq) |
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| KOH |
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| Strong Base (Potassium hydroxide) K+(aq) + OH-(aq) |
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| LiOH |
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| (Strong Base )Lithium hydroxide Li+(aq) + OH-(aq) |
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| RbOH |
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| (Strong Base) Rubidium hydroxide Rb+(aq) + OH-(aq) |
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| CsOH |
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| Strong Base (Caesium hydroxide) Cs+(aq) + OH-(aq) |
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| Ca(OH)2 |
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| Strong Base Calcium hydroxide Ca2+(aq) + 2OH-(aq) (but not very soluble) |
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| Ba(OH)2 |
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| Strong Base (Barium hydroxide) Ba2+(aq) + 2OH-(aq) (but not very soluble) |
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| Sr(OH)2 |
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| Strong Base Strontium_hydroxide Sr2+(aq) + 2OH-(aq) (but not very soluble) |
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| NaCl |
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| Salt Sodium Chloride HCl + NaOH > H2O + NaCl |
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| NaHSO4 |
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| Salt Sodium Bisulfate NaOH + H2SO4 > NaHSO4 + H2O OR!! NaCl + H2SO4 > NaHSO4 + HCl |
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| K2Cr2O7 |
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| Salt Potassium Dichromate K2Cr2O7 > 2 K+ + Cr2O72- OR!! Cr2O72- + H2O ? 2 CrO42- + 2 H+ |
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| CaCl2 |
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| Salt Calcium Chloride (Solvay process) 2 NaCl + CaCO3 > Na2CO3 + CaCl2 |
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| HCOOH |
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| Weak Acid Formic Acid HCOOH + H20 <--> H30+ + COOH- |
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| CH3COOH |
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| Weak Acid Acetic Acid CH3COOH + H2O --> CH3C00- + H3O+ |
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| CCl3COOH |
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| Weak Acid Trichloroacetic Acid CCl3COOH +H20 -> CCl3COO– + H+ (aq) |
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| HF |
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| Weak Acid Hydrofluoric Acid HF + H2O ---------> H3O+ + F- |
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| HCN |
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| Weak Acid Hydrocyanic Acid HCN + H20 -> H30+ + CN- |
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| H2S |
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| Weak Acid Hydrogen sulfide H2S + H2O --> H3O+ + HS- |
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| H2O |
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| Weak Acid/Base Water H2O -> H+ + OH-. |
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| NH4+ |
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| Weak Acid: Conjugate acids of weak bases |
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| NH3 |
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| Weak Base Ammonia NH3 + HOH <==> NH4+ + OH- A few interactions between ammonia and water will result in this case, were ammonia acts as a Bronsted-Lowry base and water acts as an acid. NH3 + H2O <==> NH2- + H3O+ But a fraction of the interactions between ammonia and water will produce this reaction since both ammonia and water are amphoteric. But in fact, the majority of NH3 molecules in aqueous solution stay NH3 molecules and don't react at all. |
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| N(CH3)3 |
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| Weak Base trimethyl ammonia |
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| C5H5N |
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| Weak Base pyridine |
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| NH4OH |
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| Weak Base ammonium hydroxide |
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| HS- |
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| Weak Base HS- ion |
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| HCOO- |
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| Weak Base: Conjugate bases of weak acids |
