Day 1 Acid-Base.

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Presentation transcript:

Day 1 Acid-Base

Review of naming acids

Determine Name: H2SO3 H2SO4 H2S HClO3 HCl HClO2

Determine Name: H2SO3 H2SO4 H2S HClO3 HCl HClO2

Determine Formula Hydrofluoric acid Carbonic acid Nitrous acid Hydroselenic acid

Determine Formula Hydrofluoric acid Carbonic acid Nitrous acid Hydroselenic acid

Characteristics of Acids & Bases

Acids are Characterized by: Sour taste  color of indicator Release of H2 gas Reacts with bases  salt ( ionic compound) & H2O

Bases are Characterized by: Bitter taste Feels slippery  color of indicator Reacts with acid  salt( ionic compound) & H2O Conducts electric current ( its an ionic compound)

Adding or removing electrons (e-) Making a cation or anion Ionization Adding or removing electrons (e-) Making a cation or anion

Ionizes completely = breaks up completely Conducts electric current Strong Acids Ionizes completely = breaks up completely Conducts electric current (remember electrolyte demo aka light bulb)

Hydrochloric Acid (HCl) Strong Acids Examples: Hydrochloric Acid (HCl) Sulfuric Acid (H2SO4) Nitric Acid (HNO3)

Strong Base Ionizes completely = breaks up completely Examples: group 1 hydroxides – sodium hydroxide, potassium hydroxide, etc.

Neutralization Reaction HCl + NaOH  NaCl + HOH Strong + Strong  Salt + Water Acid Base HNO3 + KOH  KNO3 + HOH

Neutralization Reaction Is a double replacement rxn b/w … Strong + Strong  Salt (ionic compound) + H2O Acid Base

Homework

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