'Hydroxide ion concentration' diaporamas de présentation

Table of Contents

Acid-Base Titration and pH. Chapter 15. Table of Contents. Section 1 Aqueous Solutions and the Concept of pH Section 2 Determining pH and Titrations. Section 1 Aqueous Solutions and the Concept of pH. Chapter 15. Lesson Starter.

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Chapter 14

Chapter 14. Acids and Bases. Acid/Base Theories. Arrhenius Theory Acids produce H + ions in solution Bases produce OH - ions in solution Downside Must be in solution and must have those ions Bronsted-Lowry Theory Acids are H + donors (Proton donors)

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D- WATER, acids, bases, and buffers

D- WATER, acids, bases, and buffers. WATER, acids, bases, and buffers I. WATER

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Chapter 6 Problems

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There are several ways to define acids and bases:

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Arrhenius Definition of

Arrhenius Definition of. Acids Bases. - Substances that produce hydrogen ions, H + when dissolved in water. HCl ? H + + Cl -. - Substances that produce hydroxide ions, OH - when dissolved in water. NaOH ? Na + + OH -. What is ammonia?. NH 3. Acid or base?.

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Chapter 2

Chapter 2. Homework- 5, 6, 8, 9, 13, 19. Water. Water is the predominate chemical component of living organisms It is important in Biochemistry because of: Ability to solvate due to dipole and H-Bond capacity Interaction of molecules and water helps dictate structure (ex. Proteins)

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Acid-Base Equilibrium DrillProblems

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Hydronium Ions and Hydroxide Ions Self-Ionization of Water

Section 1 Aqueous Solutions and the Concept of pH. Chapter 15. Hydronium Ions and Hydroxide Ions Self-Ionization of Water. In the self-ionization of water, two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton.

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Acid/Base review

Acid/Base review. In an acid/base titration, one has an equal amount of acid and base 1 ) at the beginning of the titration. 2 ) after all the base has been added . 3 ) all the time throughout the titration . 4 ) at the middle of the large change of pH during the titration.

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Acids and Bases

Acids and Bases. Electrolytes. Substance that conducts electricity when dissolved in water Ionizes in water Examples: aqueous ionic solutions, acids, bases. Properties of Acids. Acids have a pH less than 7.0 Acids will burn your skin Dilute acids have a sour taste

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Acids

Acids. A Swedish chemist, named Arrhenius in 1890 proposed that an acid be defined as any substance that, when added to water, increases the hydronium ion concentration. Hydronium is defined as H 3 O +. Water will attract a H + ion to produce a hydronium ion. H 2 O + H + ? H 3 O +.

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Unit Twelve Acids and Bases

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Modern Chemistry Chapter 15 Acid-Base Titration & pH

Modern Chemistry Chapter 15 Acid-Base Titration & pH. Section 1. self-ionization of water occurs when two water molecules produce a hydronium (H 3 O + ) and a hydroxide (OH - ) ion 2 H 2 O ? H 3 O + + OH -

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STRONG BASES LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH) 2 , Sr(OH) 2 , Ba(OH) 2

STRONG BASES LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH) 2 , Sr(OH) 2 , Ba(OH) 2. Equations for Strong Arrhenius bases - ionize completely to form OH - LiOH (s) ? Li + + OH - Ca(OH) 2 (s) ? Ca 2+ + 2 OH -. Calculate the pH of 0.15M Calcium hydroxide solution.

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A bit more on the pH scale

A bit more on the pH scale. CONCENTRATION. ACIDS. BASES. (molar concentrations of H + and OH - ions). Contain greater number of H+ ions than OH- ions pH of (0-6.9)). Contain less H+ ions than OH- ions pH of (7.1-14). Neutral Solutions.

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STRONG BASES LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH) 2 , Sr(OH) 2 , Ba(OH) 2

STRONG BASES LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH) 2 , Sr(OH) 2 , Ba(OH) 2. Equations for Strong Arrhenius bases - ionize completely to form OH - LiOH (s) ? Li + + OH - Ca(OH) 2 (s) ? Ca 2+ + 2 OH -. Calculate the pH of 0.15M Calcium hydroxide solution.

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Definitions and Formulas

pH. Definitions and Formulas. The pH scale is defined as the negative log of the concentration of H + : pH = -log[H + ] The pOH scale is defined as the negative log of the concentration of OH - , [OH - ]. pOH = -log[OH - ]

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