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Introduction to Acids and Bases
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What are Acids and Bases?
There are two models: Arrhenius (He came first and most often this is what is used as a definition for an acid or a base) Bronsted-Lowry (they expanded they definitions to include substances that didn’t necessarrily meet the requirements of Arrehenius’ definition)
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Acid: Increases H+ concentration in water.
Arrhenius Acid: Increases H+ concentration in water. The individual ions will separate! Examples: HCl H+ + Cl- HNO H+ + NO3- H2SO H+ + SO4 2- H2O
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Base: Increases OH- concentration in water.
Arrhenius Base: Increases OH- concentration in water. The individual ions will separate! Examples: NaOH Na+ + OH- LiOH Li+ + OH- Ca(OH) Ca2+ + 2OH- H2O Note: Contain OH- as anion in formula!
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In a formula: Acids will start with an H Bases will end in an OH
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Bronsted-Lowry Acid: A substance that can DONATE a proton (H+) to another substance. Base: A substance that ACCEPTS a proton (H+) from another substance. Examples: NH HCl NH4 + Cl- CO HBr HCO Br-
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Bronsted-Lowry Acids further grouped by # of H+ they can donate: Monoprotic: HF, HCl, HNO3 , HClO3 Diprotic: H2SO3 , H2SO4 , H2CO3 Triprotic: H3PO4
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Comparison Arrhenius Acid HCl HBr H2SO4 H3PO4 etc. Bronsted-Lowry Acid
Same as above
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Comparison Arrhenius Base NaOH LiOH Ca(OH)2 Bronsted-Lowry Base
NH3 , OH - , HCO3 -
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These are called conjugate acids and bases.
A better way to identify acids and bases is by LOOKING FOR PROTON ACCEPTORS AND DONATORS NH3 + H2S NH SH- These are called conjugate acids and bases.
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Conjugate Acids and Bases
(Note: Conjugates are on the product side, the right side, of the chem. eqn.) Conjugate Acid: -the substance formed when a base gains a hydrogen ion. NH3 + H2S NH SH- conj. acid
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Conjugate Acids and Bases
Conjugate Base: -the substance formed when an acid loses a hydrogen ion. NH3 + H2S NH SH- conj. base
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Conjugate Acids and Bases
Conjugate Acid-Base Pair: consists of two substances related by the loss or gain of a single hydrogen ion NH3 + H2S NH SH- Base Acid Conj Conj Acid Base
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Conjugate Acids and Bases
Try These: Label acid, base, conjugate acid and conjugate base. HBr H2O H3O Br- NOTE: H3O+ called “hydronium ion”
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Conjugate Acids and Bases
Try These: Label acid, base, conjugate acid and conjugate base. HCl OH HOH Cl-
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Conjugate Acids and Bases
Try These: Label acid, base, conjugate acid and conjugate base. CO H2O HCO OH -
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Conjugate Acids and Bases
Try These: Label acid, base, conjugate acid and conjugate base. CO H2O HCO OH - NOTE: H2O can act as an acid or a base. Substances that can do this called ‘amphoteric’!
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To Summarize… • Acids donate a proton, become conjugate bases.
• Bases accept a proton, become conjugate acids.
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Check Your Understanding
Write the conjugate acid to the following bases: SO4 2- Cl - NO2 - HCO3 -
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Check Your Understanding
Write the conjugate acid to the following bases: SO4 2- HSO4 - Cl - HCl NO2 - HNO3 HCO3 - H2CO3
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Check Your Understanding
Write the conjugate base to the following acids: HNO3 H2SO3 NH3 HCO3 -
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Check Your Understanding
Write the conjugate base to the following acids: HNO3 NO3 - H2SO3 HSO3 - NH3 NH2 - HCO3 - CO3 2-
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