'Dissociation constant' presentation slideshows

Chapter 7

Chapter 7. Acids and Bases. Chapter 7 Acids and Bases. 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The pH Scale 7.4 Calculating the pH of Strong Acid Solutions 7.5 Calculating the pH of weak Acid Solutions 7.6 Bases 7.7 Polyprotic Acids

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18 Acids and Bases (AHL)

18 Acids and Bases (AHL). DP Chemistry Rob Slider. Acid-Base Calculations. Product constant of water K w. Note that water slightly dissociates in equilibrium with hydrogen and hydroxide ions: H 2 O ?? H + + OH - So, the equilibrium constant is:

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18 Acids and Bases (AHL)

18 Acids and Bases (AHL). DP Chemistry Rob Slider. Acid-Base Calculations. Product constant of water K w. Note that water slightly dissociates in equilibrium with hydrogen and hydroxide ions: H 2 O ?? H + + OH - So, the equilibrium constant is:

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Introduction to Analytical Chemistry

Introduction to Analytical Chemistry. Chapter 7 Principles of eutralization Titrations : Determining Acids, Bases, and the p H of Buffer Solutions. 7A-2 Acid/Base Indicators.

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Chapter 15

Chapter 15. Complex Acid/Base Systems. Complex systems may be described as solutions made up of two acids or two bases of different strengths, (2) an acid or a base that has two or more acidic or basic functional groups, or (3) an amphiprotic substance, acting as both an acid and a base.

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It is considered that Water is abundant and common

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Binding

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Chemistry 19.3

Chemistry 19.3. Strengths of Acids and Bases. 19.3.

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Chemistry 19.3

Chemistry 19.3. Strengths of Acids and Bases. 19.3.

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Acids and Bases

Acids and Bases. Properties of Acids. 1. Taste sour or tart and feels like water ex. Oranges, grapefruit, yogurt, sour milk, carbonated beverages, vinegar 2. React vigorously with many metals (produces hydrogen gas) 3. Electrolyte 4. Reacts with bases to make salt and water.

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THEME : Acid-base equilibrium in biological systems. Buffer solutions .

THEME : Acid-base equilibrium in biological systems. Buffer solutions. Plen Ionization of water . Acid-base theory . Buffer solutions. Buffer in blood. Water is ? neutral molecule with ? slight tendency to ionize. We usually express this ionization as: ? 2 ? = ? + + ?? -.

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Weak Acids and Bases

Weak Acids and Bases. Mg (s) + 2HCl (aq) --> MgCl 2 (aq) + H 2 (aq) Mg (s) + 2CH 3 COOH (aq) --> Mg(CH 3 COO 2 ) 2 (aq) + H 2 (aq). Working with Weak Acids and Bases. In a solution of a weak acid, what do we have? Acid molecules Small amount of H 3 O +

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Spectrophotometric Method for Determination of Dissociation Constant of weak acid like 2, 4-Dinitrophenol in 1-Propanol-

Spectrophotometrically dissociation constant (pKa) of the indicator acid, 2,4-Dinitrophenol in 5,10,20,30 and 40 wt. % 1-propanol – water mixtures at 24.5±0.5ºC were determined. The experimental values of ЄIn- potassium salt of indicator acid and the derived values of intercept of ЄIn- values using Ion-pair intermediate model equation shows a good consistency ,suggesting the ion-pair intermediate model is applicable in the present instance. The maximum drop in pka was found to occur around 20 wt. % 1-propanol- water mixtures. This has been explained as due to increase in solvation energy for anion of the acid by London- dispersion force mechanism. The drastic increase in pka values above 20 wt% propanol has been assumed to be due to decrease in dielectric constant of the medium. This method is suitable for determination of dissociation constant for weak acid and this method will be helpful for determination of dissociation constant for drugs are weak acid in nature.

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Spectrophotometric Method for Determination of Dissociation Constant of weak acid like 2, 4-Dinitrophenol in 1-Propanol-

Spectrophotometrically dissociation constant (pKa) of the indicator acid, 2,4-Dinitrophenol in 5,10,20,30 and 40 wt. % 1-propanol – water mixtures at 24.5±0.5ºC were determined. The experimental values of ЄIn- potassium salt of indicator acid and the derived values of intercept of ЄIn- values using Ion-pair intermediate model equation shows a good consistency ,suggesting the ion-pair intermediate model is applicable in the present instance. The maximum drop in pka was found to occur around 20 wt. % 1-propanol- water mixtures. This has been explained as due to increase in solvation energy for anion of the acid by London- dispersion force mechanism. The drastic increase in pka values above 20 wt% propanol has been assumed to be due to decrease in dielectric constant of the medium. This method is suitable for determination of dissociation constant for weak acid and this method will be helpful for determination of dissociation constant for drugs are weak acid in nature.

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Equilibria of Weak Acids and Bases

Equilibria of Weak Acids and Bases. Strong/Weak Acids. Strong HBr, HI, HCl, HNO 3 , H 2 SO 4 , HClO 4 Readily transfer H + ion to water Completely dissociated Strong electrolyte Weak HC 2 H 3 O 2 , HCN, HNO 2 , HClO, HCO 3 - Does not readily transfer H+ ion Most remains un-ionized.

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Calculating Net Protein Charge

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Chemistry Objectives Unit VI- Ch. 17

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Determining the Strengths of Acids and Bases

Determining the Strengths of Acids and Bases. Objectives: 1. Define the term dissociation constant and explain what it indicates about and acid or a base 2. Explain what happens when acids and bases are mixed together. Vocabulary

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