'Acid ionization constant' presentation slideshows

Chapter 16

Chapter 16. Ionic Equilibria: Acids and Bases. Chapter Goals. A Review of Strong Electrolytes The Autoionization of Water The pH and pOH Scales Ionization Constants for Weak Monoprotic Acids and Bases Polyprotic Acids Solvolysis Salts of Strong Bases and Strong Acids. Chapter Goals.

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Acids and Bases

Acids and Bases. Acids and Bases. Acid : a substance that, when dissolved in water, increases the concentration of H + (protons) HCl H + + Cl - HCl + H 2 O H 3 O + + Cl - Strong acid : an acid that completely ionizes/dissociates in water HNO 3 + H 2 O H 3 O + + NO 3 -

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Acids and Bases

Acids and Bases. Chapter 19. 19.1 Acids and Bases: An Intro. All aqueous solutions contain hydrogen ions (H + ) and hydroxide (OH - ) ions. An acidic solution contains more H + ions than OH - . A basic solution contains more OH - ions than H + ions.

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acid ionization constant K a

acid ionization constant K a. HX ? X - + H + [ X - ] [ H + ] K a = ------------------ [ HX ]. base ionization constant K b. X + H 2 0 ? HX + + OH - [ HX + ] [ OH - ] K b = ------------------ [ X ].

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The Ka and Kb of it

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Basic Concepts

Basic Concepts. One of the fundamental ideas of chemical equilibrium is that equilibrium can be established from either the forward or reverse direction. The rates of the forward and reverse reactions can be represented as:. When system is at equilibrium: Rate f = Rate r.

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Ch.16. Acids and Bases (the fundamentals)

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Buffer solutions

Buffer solutions. Conjugate Acid and Base. Conjugate acid and base , HA/A - , differ by one proton. The conjugate acid of a base, is the base plus the attached proton. And the conjugate base of an acid is the acid minus the proton. Example:. Acid And Base Ionization Constants.

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Strengths of Acids and Bases

Strengths of Acids and Bases. Electrical Conductivity. Acidic and basic solutions conduct electricity. Strengths of Acids. Acids that completely ionize (dissociate) are called strong acids. Strong acids produce a strong electric current = strong electrolyte

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Ka, Kb

Ka, Kb. Acid and Base Dissociation Constants. How do we calculate [H + ] for a weak acid?. We know that strong acids dissociate 100% and that, therefore, the [H + ] equals that [acid] that we start with What about weak acids?

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Kinetics and Equilibria

Kinetics and Equilibria. By definition, kinetic processes are not equilibrium processes . In fact, we may think of kinetic processes as the mechanism that nature uses to reach the equlibrium state. Binary Collision rate in forward direction. Binary Collision rate in reverse direction.

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Ionic equilibrium

Ionic equilibrium . Lec.9. Introduction . Ionization : a process in which unionized molecules are changed into ions. Types of electrolytes:. Where: K a = acid ionization constant K b = base ionization constant. Ostwald Law(1888):

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