An amphiprotic substance can do either! Strong acid Strong base Weak acid Weak base.

Slides:

Advertisements

Similar presentations

Go over Ch Test Summary of this week Questions over the reading Discussion / explanation Homework.

Advertisements

14.1 Arrhenius Definition Acids produce hydrogen ions (H+) in aqueous solution. Bases produce hydroxide ions (OH-) when dissolved in water. Limits to.

Section 18.3 Hydrogen Ions and pH

Ch.15: Acid-Base and pH Part 1.

Acids, Bases, and Salts Chapter 19.

1 Weak Acids and Bases A weak acid or base is an acid or base that partially (less than 100%) dissociated in water. The equilibrium constant is usually.

Acid and Base Equilibrium

Acid Strength and Structure Acid-Base Properties of Salts AP Chemistry.

A salt is an ionic compound consisting of a cation other than H+ and an anion other than OH minus. Here, we’ll show you all about hydrolysis of ions in.

Chapter 16: Aqueous Ionic Equilibria Common Ion Effect Buffer Solutions Titrations Solubility Precipitation Complex Ion Equilibria.

Acid - Base Equilibria AP Chapter 16. Acids and Bases Arrhenius acids have properties that are due to the presence of the hydronium ion (H + ( aq )) They.

Acid / Base Equilibria A Practical Application of the Principles of Equilibrium.

1 Chapter 10 Acids and Bases 10.3 Strengths of Acids and Bases 10.4 Dissociation Constants.

EQUILIBRIUM Part 1 Common Ion Effect. COMMON ION EFFECT Whenever a weak electrolyte and a strong electrolyte share the same solution, the strong electrolyte.

Polyprotic Acids And Acid and Base Salts.

Buffers AP Chemistry.

Students should be able to: 1. Identify strong electrolytes and calculate concentrations of their ions. 2. Explain the autoionization of water. 3. Describe.

Ch. 15: Applications of Aqueous Equilibria 15.1 Common Ion Effect.

  Weak acid/conjugate base mixtures OR weak base/conjugate acid mixtures  “buffers” or reduces the affect of a change in the pH of a solution  Absorbs.

Acids and Bases Chapter 20 Lesson 2. Definitions Acids – produce H + Bases - produce OH - Acids – donate H + Bases – accept H + Acids – accept e - pair.

ACID AND BASES Definition and properties of Acid: Acid is defined as a substance whose aqueous solution possesses the following characteristic properties:

Maths and Chemistry for Biologists

Acids-Bases Arrhenius:

Acids-Bases Arrhenius: Acid…. A substance that increases the hydrogen ion, H +, concentration when dissolved in H 2 O. Eg. HCl, H 2 SO 4, HC 2 H 3 O 2.

Acids and Bases The concept of acidic and basic solutions is perhaps one of the most important topics in chemistry. Acids and bases affect the properties.

Properties of acids n Taste Sour (kids, don’t try this at home). n Conduct electricity. n Some are strong, some are weak electrolytes. n React with metals.

PH calculations. What is pH? pH = - log 10 [H + (aq) ] where [H + ] is the concentration of hydrogen ions in mol dm -3 to convert pH into hydrogen ion.

1 TitrationsTitrations pHpH Titrant volume, mL At what point in a reaction does neutralization occur?

Acid-Base Equilibria (Buffers ) Green & Damji Chapter 8, Section 18.2 Chang Chapter 16 Copyright © The McGraw-Hill Companies, Inc. Permission required.

Weak Acids & Weak Bases. Review Try the next two questions to see what you remember Try the next two questions to see what you remember.

Acid and Base Equilibria Electrolytes Strong Conduct electricity Weak Poor conductors of electricity Nonelectrolytes Do not conduct electricity.

Acid-base equilibrium

Determining the Strengths of Acids and Bases

Finding the pH of Weak Acids. Strengths of Acids and Bases “Strength” refers to how much an acid or base ionizes in a solution. STRONGWEAK Ionize completely.

Aqueous Solutions. Solution Homogeneous mixture Solute – substance be dissolved Solvent- substance solute is dissolved in.

Hydrolysis and Neutralization

Buffer or Common Ion problems. Identify the weak acid or base in the problem. There has to be one or the other to create a buffer. Write the ionization.

8.3 Bases Similar to weak acids, weak bases react with water to a solution of ions at equilibrium. The general equation is: B(aq) + H2O(l)  HB+(aq) +

Hydrolysis and Neutralization

CMH 121 Luca Preziati Chapter 8: Acids and Bases Acid = produces H + An acid is a compound that: 1. Has H somewhere 2. Has the tendency (is capable) of.

We are faced with different types of solutions that we should know how to calculate the pH or pOH for. These include calculation of pH for 1. Strong acids.

O 2 vs CO binding a heme. Understand and identify weak and strong electrolytes OWL – 7.6 o Strong electrolyte Dissolve & 100% Dissociate Strong electrolyte.

Chapter 15 Applications of Aqueous Equilibria

Acids & Bases. Acids and Bases an Introduction A. Properties of Acids and Bases –1. Acids Ionize when put into water React with active metals (Group I,

Chapter 16 Acids and Bases. Characteristics Acids: – Bases: – Change the color of dyes.

Acid and Base Strength Chapter How can we test how strong an acid is? electrical conductivity can be used to determine the strength of an acid or.

Salt Hydrolysis. Salts Ionic compound made up of CATION and ANION Has acidic and basic properties Based on ions produced when salts dissociate No acid/base.

Section 16.2 Determining the Acidity of a Solution 1.To understand and determine pH and pOH 2.To learn methods for measuring pH of a solution Objectives.

Acid Base Review Standard 5 Chapter 19. TRUE / FALSE 1.Acids produce OH- ions in water. True False How do you know if it’s an acid or base? HCl  H +

Chapter 16 Acids and Bases. Characteristics Acids: Sour taste –Lemons, Oranges (citric acid) Bases: Slippery, bitter taste –Soaps Change the color of.

BASE IONIZATION Section 8.3. Base-Ionization Constant - K b ■The following equation represents a weak base, B, dissolving in water: ■B (aq) + H 2 O (l)

Chapter 16 Sections 8-9. © 2009, Prentice-Hall, Inc. K a and K b K a and K b are related in this way: K a  K b = K w Therefore, if you know one of them,

CH 13 Acids and Bases.

Hydrolysis  dissociation with water  reaction with water

Complete table Calculate Kc with units if any A + B = 2C component A B

Acids and Bases.

Chapter 19 Review “Acids, Bases, and Salts”

SAMPLE EXERCISE 17.6 Calculating pH for a Strong Acid–Strong Base Titration Calculate the pH when the following quantities of M NaOH solution have.

Unit 5: Acid-Base Calculations Lesson 1: Kw, Ka, and Kb

Acids and bases.

Calculate the pH of a solution that is 0

Acids and Bases.

Salts neutralization reactions acids bases strong acid+ strong base

Salts neutralization reactions acids bases strong acid+ strong base

Section 18.2 Strengths of Acids and Bases

Chapter 19 Review “Acids, Bases, and Salts”

AP Chem Take out HW to be checked Today: Acid-Base Titrations.

Dissociation Equilibria for weak acids and bases

Chapter 9: 1. Which of the following statements about water is TRUE?

The Common Ion Effect The solubility of a partially soluble salt is decreased when a common ion is added. Consider the equilibrium established when acetic.

Presentation transcript:

An amphiprotic substance can do either!

Strong acid Strong base Weak acid Weak base

For weak acids we ignore the water as it is constant in aqueous solutions K becomes Ka. The acid dissociation constant

In a question, decide whether you write an expression for Ka or Kb. OH - as a product means Kb. H 3 O + means Ka

Product of [H 3 O + ] and [OH - ] always equals

Ions will not react with water so therefore neutral Use the formula to determine the [OH - ] Write the equation for dissolving then the ion reacting with water

Pick out the strong acid and base. Remember these go to completion when writing equations Pick out the acidic salt then the weak base

Don’t be scared! Use the formula as given for the acid and write equation

What equation links H 3 O + with pH?

Volume Conc. Moles

Look back over the question to see what you have You have [H 3 O + ] You have [HPab] You have the Ka expression Make your assumptions and insert How do we get from Ka to pKa?

Amines are weak bases... Hmmmm...no info. We’ll have to use the equations logically Weak bases only partially dissociate so it must be greater than conjugate [OH - ] = [CH 3 NH 3 + ] Weak base so [OH - ] must be greater than [H 3 O + ] Use both equations. Use first formula to predict Cl- [NH 4 + ] would have been the same as [Cl - ] at start, but at equilibrium, some would be changed to NH 3 [NH 4 + ] would be greater than its conjugate as weak acids only partially dissociate [NH 3 ] is the same as [H 3 O + ] In a weak acid, [H 3 O + ] is greater than [OH - ]

Ions that move in an electric field With water

Salt of a weak acid Must be a weak base Show the equation to show the salt dissolves Show the equation with water only one works!

Write equilibrium equation of NH 3 What happens when NH 4 Cl dissolves? Show equation So the NH 4 + increases...what effect will this have on the equilibrium What effect will this have on the H 3 O + conc?