Need help. Acids and Bases Reactions.

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  

An acid–base reaction is a type of chemical reaction that involves the exchange of one or more hydrogen ions, H+, between species that may be neutral (molecules, such as water, H2O) or electrically charged (ions, such as ammonium, NH4+; hydroxide, OH−; or carbonate, CO32−).

Explanation:Look at the following examples:

Nitric acid reacts with sodium carbonate to form sodium nitrate, carbon dioxide and water. ...

Sulfuric acid reacts with calcium carbonate to form calcium sulfate, carbon dioxide and water. ...

Hydrochloric acid reacts with calcium carbonate to form calcium chloride, carbon dioxide and water.

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