'Ph log 1' diaporamas de présentation

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Bellwork Thursday

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The Chemistry of Acids and Bases

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The Chemistry of Acids and Bases

The Chemistry of Acids and Bases. Acid and Bases. Acid and Bases. Acid and Bases. Acids. General Descriptions. Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain metals to produce hydrogen gas.

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NEUTRALIZATION

NEUTRALIZATION. Prepared By Michigan Department of Environmental Quality Operator Training and Certification Unit. NEUTRALIZATION. Addition of an acid or alkali (base) to a liquid to cause the pH of the liquid to move towards a neutral pH of 7.0. ACID. Adds Hydrogen Ions. H +.

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Acids and Bases

Acids and Bases. Ionization of Water The pH Scale. Ionization of Water. Occasionally, in water, a H + is transferred between H 2 O molecules . . . . . . . . H : O : + : O : H H : O : H + + : O : H -

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EQUILBRIUM OF Acids and Bases

EQUILBRIUM OF Acids and Bases. Chapter 17. Water. AUTOIONIZATION. H 2 O can function as both an ACID and a BASE. Equilibrium constant for water = K w K w = [H 3 O + ] [OH - ] = 1.00 x 10 -14 at 25 o C. Water. K w = [H 3 O + ] [OH - ] = 1.00 x 10 -14 at 25 o C

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Chapter 14 Acids and Bases

Chapter 14 Acids and Bases. 14.6 The pH Scale. pH Scale. The pH of a solution is used to indicate the acidity of a solution has values that usually range from 0 to 14 is acidic when the values are less than 7 is neutral with a pH of 7 is basic when the values are greater than 7.

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Chapter 12: Principles of Neutralization Titrations

Chapter 12: Principles of Neutralization Titrations. By: Andie Aquilato. Solutions and Indicators Used. Slides 2-6. Standard Solutions: strong acids or strong bases because they will react completely Acids: hydrochloric (HCl), perchloric (HClO 4 ), and sulfuric (H 2 SO 4 )

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pH Scale and Calculations

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pH and pOH

pH and pOH. Ionization of water. Experiments have shown that pure water ionizes very slightly: 2H 2 O ? H 3 O + + OH - Measurements show that: [ H 3 O + ] = [OH - ]=1 x 10 -7 M Pure water contains equal concentrations of H 3 O + + OH - , so it is neutral. pH.

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Chapter 17 Additional Aspects of Aqueous Equilibria

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pH Scale

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Common ion effect

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CHEM100_11

Lecture #33. Chapter 17. Buffers. CHEM100_11. This week: Labs. Reports should be completed in the lab. Bring calculators and rulers. Class average 63%. Dr. Orlova PS-3026 Ph: 867-5237 gorlova@stfx.ca. Student Chemical Society Tutorials:

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Chap. 2. Problem 2a.

Chap. 2. Problem 2a. pH = - log [H + ] pH = - log (1.75 x 10 -5 ) pH = - (-4.76) pH = 4.76. Chap. 2. Problem 3a. pH = - log [H + ] [H + ] = 10 -pH [H + ] = 10 -3.82 [H + ] = 1.51 x 10 -4 M. Chap. 2. Problem 12. Part a .

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Chap. 2. Problem 2a.

Chap. 2. Problem 2a. pH = - log [H + ] pH = - log (1.75 x 10 -5 ) pH = - (-4.76) pH = 4.76. Chap. 2. Problem 3a. pH = - log [H + ] [H + ] = 10 -pH [H + ] = 10 -3.82 [H + ] = 1.51 x 10 -4 M. Chap. 2. Problem 12. Part a .

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pH Indicators

pH Indicators. The One Only Adrian Arias. What is pH Indicator. A pH indicator is a halochromic chemical compound that is added in small amounts to a solution so that the pH (acidity or basicity) of the solution can be determined visually. How does a pH Indicator work (Litmus).

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pH and pOH

pH and pOH. Chapter 16.2 and 16.3. What is pH and pOH?. pH is the concentration of hydronium ions in a solution pOH is the concentration of hydroxide ions in a solution pH tells you the strength of an acid or a base (more hydronium = more acidic) Strongest acid = 0.0 Neutral = 7.0

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