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ACID / BASE CHEMISTRY

ACID / BASE CHEMISTRY. Swedish Chemist Savante Arrhenius 1880’s Theory of Ionization. HNO3 ( aq )  H+ ( aq ) + (NO3)- ( aq ). KOH (s) + H20  K+ ( aq ) + (OH)- ( aq ). NH3 ( aq ) + H2O (l)   (NH4) + ( aq ) + (OH)- ( aq ).

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ACID / BASE CHEMISTRY

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  1. ACID / BASE CHEMISTRY

  2. Swedish Chemist Savante Arrhenius 1880’s Theory of Ionization

  3. HNO3 (aq)  H+ (aq) + (NO3)- (aq)

  4. KOH (s) + H20  K+ (aq) + (OH)- (aq)

  5. NH3 (aq) + H2O (l)   (NH4) + (aq) + (OH)- (aq)

  6. 1920’s Johannes Bronsted & Thomas Lowry • Bronsted-Lowry acid/base concept

  7. Bronsted-Lowry acid is a hydrogen ion donor • Bronsted-Lowry base is a hydrogen ion acceptor

  8. CH3COOH (aq) + H20   (CH3 COO)- (aq) + (H30)+ (aq)

  9. STRONG ACIDS • HCLO3 • HBR • HCL • HI • HNO3 • HCLO4 • HMn04 • H2SO4 • HBF4

  10. WEAK ACIDS • CH3COOH • H3B03 • HCN • HFl • H2S • HCLO • HNO2 • H2C204 • H3P04 • H2S03

  11. STRONG BASES • Ba(OH)2 • Ca(OH)2 • KOH • NaOH • NA3P04

  12. WEAK BASES • NH3 • C6H5NH2 • K2C03 • Na2CO3 • (CH3)3N

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