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ACIDS and BASES

 

 Acids

Link-->ACID NAMING RULES

Properties- 

Produce H(H3O+) in water as the only positive ion.

Acids are electrolytes. They ionize and conduct electricity in water. ex. HCl(aq) 

Dilute quantities taste sour. ex. Citric Acid

Corrodes metals to produce hydrogen gas (H2)

Concentrated Acids are CAUSTIC, they cause chemical burns to skin.

Turn Blue Litmus Red

Phenolphthalein turn colorless

Neutralizes Bases

pH less than 7

--->Strong Acids vs. Weak Acid Tutorial<---

Determining Strong Acids-Strong acids almost completely ionize in water. Looking at TABLE L the IONS lie to the right in the equilibrium equation. Therefore a LARGE value for K will indicate the equilibrium exist to the RIGHT and the acid is STRONG.

EXAMPLES- HI, HBr, HCl, HNO3, H2SO4

Determining Weak Acids- Weak acids exist as molecules rather then ions in water. Looking at TABLE L, the since IONS lie to the right in the equilibrium equation and the molecules lie to the LEFT. A small value for K will indicate the equilibrium exist to the LEFT and the acid is WEAK.

Conjugate Acid Base Pairs-

Given the reaction:CH3COOH(aq) + H2O(l) <---> CH3COO-(aq) + H3O+        

CH3COOH is an acid in the forward reaction
True
False

Bases

Properties

Produce OH- in water

Taste bitter, chalky

Electrolytes

Feel slippery, like soap

React with acid to form salt and water

pH greater than 7

Turns red litmus blue

Strong Bases-Bases that have a large Kb will ionize more completely and are thus stronger bases. A strong base has a lower H+ concentration because they are fully protonated and less hydrogen ions remain in the solution. A lower H+ concentration also means a higher OH- concentration and therefore, a larger Kb

Ex. Group 1 Hydroxides. NaOH, LiOH, RbOH, KOH

Weak Bases-In chemistry, a weak base is a chemical base that does not ionize fully in an aqueous solution.

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