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Acids and Bases.

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Presentation on theme: "Acids and Bases."— Presentation transcript:

1 Acids and Bases

2 Acids Taste sour Turn litmus paper red React vigorously with metals
Conduct electricity Corrosive Make H3O+ Proton donors (BrØnsted-Lowry)

3 Bases Turn litmus blue Taste bitter Feel slippery Conduct electricity
Corrosive Make OH- ions Proton acceptor (BrØnsted-Lowry)

4 Dissociation Ionic compound breaks apart into its ions
Write the dissociation equation for the following: NaOH Ca(OH)2 HCl H2CO3

5 Strong vs. Weak (electrolytes/acids/bases)
Strong completely dissociate Weak partially dissociate A strong (acid/base) completely ionizes in a solvent. A weak (acid/base) partially ionizes in a solvent. In equilibrium Few H+/OH- are released in aqueous solution.

6 Arrhenius Acids Any substance that, when added to water, increases the hydronium (H3O+) concentration. Number of ionizable H determines how many H3O+ are made. Ionizable H are at the beginning of the cmpd HCl H2SO4

7 Arrhenius Base Any substance that, when added to water, increases the hydroxide (OH-) Number of OH- in formula is how many OH- are made NaOH Ca(OH)2

8 Problems w/Arrhenius Limited to aqueous solutions
Cannot classify substances that can act as either acids or bases.

9 Brønsted-Lowry Classification
Brønsted-Lowry acid - donates a proton look at the reaction: (1) HCl  H+ + Cl− (2) H+ + H2O  H3O+ HCl is an Arrhenius acid- makes a H3O+. HCl is a Brønsted-Lowry acid because it donates a proton (H+).

10 Brønsted and Lowry Base
A proton acceptor. Ammonia (NH3)-proton acceptor NH3- makes OH- in water so Arrhenius base

11 Classification Arrhenius acids/bases are also Brønsted-Lowry acids/bases Brønsted-Lowry acids/bases are not always Arrhenius acids/bases

12 Conjugate Acids and Bases
When an acid looses a proton, it becomes a conjugate base When a base gains a proton, it becomes a conjugate acid Write the conjugate base for the following: HF H2CO3 Write the conjugate acid for the following: NO3- HCO3-

13 Every acid has a conjugate base
Every base has a conjugate acid We can look at an acid/base equations and determine acid/base pairs.

14 When the reaction is reversed, we can identify another acid and another base.
But it is the same acid/base pairs as before

15 HCl + H2O → H3O+ + Cl-

16 Amphoteric Substances that can be either both an acid or a base
can both donate and accept protons. Example: Water Has properties of both acid and base Can donate or accept H+ Hydrogen carbonate HCO3- + H2O → H2CO3 + OH- (base; H+ acceptor) HCO3- + H2O → CO3-2 + H3O+ (acid; H+ donor)


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