1. Arrhenius 's bases contains OH and produces OH⁻. The opposite to acids.
Acids from Bronsted Lowry → protons donators.
2. LiOH (aq) → Li⁺(aq) + OH⁻(aq)
3. CsOH (aq) → Cs⁺(aq) + OH⁻(aq)
4. Sr(OH)₂ (aq) → Sr²⁺(aq) + 2OH ⁻(aq)
5. Al(OH)₃ (aq) → Al³⁺(aq) + 3OH⁻(aq)
6. NaCl (aq) → Na⁺(aq) + Cl⁻(aq)
7. BaCl₂ (aq) → Ba²⁺ + 2Cl⁻
8. HCl (aq) → H⁺(aq) + Cl⁻(aq)
9.HClO₃(aq) → H⁺(aq) + ClO₃⁻(aq)
10. H₂O → OH⁻
11. HI → I⁻
12. H₂S → S⁻²
13. HCO₃⁻ → CO₃⁻²
14. H₂O → H₃O⁺
15. OH⁻ → H₂O
16. PH₃ → PH₄⁺
Explanation:
For the chart
1. Arrhenius theory states that bases, contains OH and produces OH⁻. The opposite to acids.
Acids from Bronsted Lowry are the ones that are protons donators.
To dissociate the compounds, you must split the molecules.
2. LiOH (aq) → Li⁺(aq) + OH⁻(aq)
3. CsOH (aq) → Cs⁺(aq) + OH⁻(aq)
4. Sr(OH)₂ (aq) → Sr²⁺(aq) + 2OH ⁻(aq)
5. Al(OH)₃ (aq) → Al³⁺(aq) + 3OH⁻(aq)
6. NaCl (aq) → Na⁺(aq) + Cl⁻(aq)
7. BaCl₂ (aq) → Ba²⁺ + 2Cl⁻
8. HCl (aq) → H⁺(aq) + Cl⁻(aq)
When hydrochloric acid react to water it can release a proton and form chlorides
9.HClO₃(aq) → H⁺(aq) + ClO₃⁻(aq)
When the chloric acid react to water, it releases a proton and form chlorate anion
The conjugate base, are the ions that can accept a proton to produce the acid again.
10. H₂O → OH⁻
Water release a proton, so we got hydroxides
11. HI → I⁻
Hydroiodic acid release a proton, so we got iodide
12. H₂S → S⁻²
Sulfide will be the conjugate base because it will acept the 2 protons
13. HCO₃⁻ → CO₃⁻²
Bicarbonate donates a proton, so we got carbonate anion, as the conjugate base
When the compounds acts like a base, the conjugate acids will be the one that can release the proton
14. H₂O → H₃O⁺
Hydronium release the proton
15. OH⁻ → H₂O
Water will relase the proton to the hydroxide
16. PH₃ → PH₄⁺
Phosphine is similar to ammonia.
When the ammonium is formed is acts like the conjugate base, because it can release the proton make ammonia
NH₃ + H₂O ⇄ NH₄⁺ + OH⁻
Base Acid Conj. acid Conj. base
