'Aq hco 3 aq' diaporamas de présentation

Applications of Aqueous Equilibria

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Applications of Aqueous Equilibria

1.06k views • 91 slides

Applications of Aqueous Equilibria

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Chemical Equilibrium

Chemical Equilibrium. Chemical Equilibrium.

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Introduction to Acids and Bases

Introduction to Acids and Bases. Pure or distilled water undergoes a very slight ionization as shown below. H 2 O(l) H + (aq) + OH - (aq) The equilibrium constant for water is given by: K w = [H + ][OH - ] = 1.00 x 10 -14. Note that the product of [H + ] and [OH - ] is a

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Acid Base Equilibria

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Stoichiometry

Stoichiometry. Predicting amounts of reagents needed or amounts of products made. Stoichiometry. Composition stoichiometry Mass relationships of elements in compounds Reaction stoichiometry Mass relationships between participants in a chemical reaction

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Stoichiometry

Stoichiometry. Predicting amounts of reagents needed or amounts of products made. Stoichiometry. Composition stoichiometry Mass relationships of elements in compounds Reaction stoichiometry Mass relationships between participants in a chemical reaction

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Polyprotic Acids

Polyprotic Acids. Acids that contains more than one dissociable proton Dissociate in a stepwise manner Each dissociation step has its own Ka Stepwise dissociation constants decreases in the order Ka 1 > Ka 2 > Ka 3 More difficult to remove a positively charge proton from negative ion.

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pH = - log [H 3 O + ] [H 3 O + ] = 10 - pH mol/L For pure water at 25 o C

pH = - log [H 3 O + ] [H 3 O + ] = 10 - pH mol/L For pure water at 25 o C pH = - log (1.0 x 10 -7 ) = 7.00 For a change in pH by 1, H 3 O + concentration changes by 10 Higher pH, lower H 3 O + concentration pH of pure water is 7 pH of an acidic solution is less than 7

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Acids and Bases

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Chapter 6: Neutralizing the Threat of Acid Rain

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Equilibrium

Equilibrium. I love chemistry!!!. What is Equilibrium?. A dynamic condition in which 2 opposing changes occur at equal rates in a closed system Ex. A phase change can be a physical condition that can be described to be in equilibrium Solid + ?H Liquid.

613 views • 20 slides

Chapter 13 Water: Rivers of Life; Seas of Sorrows

Chemistry for Changing Times, 11 th edition John W. Hill and Doris K. Kolb. Chapter 13 Water: Rivers of Life; Seas of Sorrows. James A. Noblet California State University San Bernardino, CA ? 2007 Prentice Hall.

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Bases

Acids. and. Bases. Properties of Acids and Bases. *Usually, but not always. NaOH(aq). HCl(aq). Taste. Bitter. Sour. Feel. Slippery. Not slippery. pH. 14. 1. Litmus. Blue. Red. Phenolphthalein. *Pink. *Cloudy/ white. Bromothymol. *Blue. *Yellow. Magnesium. NR. Bubbles.

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Bases

Acids. and. Bases. Ionization. +. H. Cl. Cl. H. Oxygen (e.g. H 2 SO 4 ) was originally thought to cause acidic properties. Later, Hydrogen was implicated, but it was still not clear why CH 4 was neutral.

81 views • 6 slides