logging in or signing up Chem 120 Acids and Bases aSGuest6757 Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 187 Category: Education License: All Rights Reserved Like it (0) Dislike it (0) Added: December 16, 2008 This Presentation is Public Favorites: 1 Presentation Description No description available. Comments Posting comment... Premium member Presentation Transcript Chapter 19 : Chapter 19 ACIDS AND BASES Chapter 19 : Chapter 19 pH: Power of the Hydrogen ion concentration Hydrogen: P – 1 N – 0 E – 1 Hydrogen +1 P – 1 N – 0 E – 0 Hydrogen Ion Concentration : Hydrogen Ion Concentration Concentration: Measured in Molarity Moles/Liter [H+] = Hydrogen Ion Concentration Brackets mean Concentration [H+] = .01 moles/liter = 1x10-2 M pH = 1x10-2 M = 2 pH Scale : pH Scale 1 – 6 = Acid 7 = Neutral 8 – 14 = Base Objectives: : Objectives: Compare Arrhenius and Bronsted-Lowry definitions. Explain why Bronsted-Lowry is more widely used Describe the similarities and differences in physical and chemical properties of acids and bases Conjugate Acid Base Pairs Definitions Arrhenius vs. Bronsted-Lowry : Arrhenius vs. Bronsted-Lowry Arrhenius: Acids – Yield H+ Bases – Yield OH- Bronsted-Lowry: Acids – Proton Donators Bases – Proton Accepters Properties of Acids and Bases : Properties of Acids and Bases Acids: Sour Taste Change Litmus to Red React with Oxides and Hydroxides of metals to form water and salt Electrolytes: Conducts electricity when dissolved in water Strong Acids and Weak Acids based on how well they disassociate Bases: Bitter Taste Change Litmus to Blue When neutralized with acids, they produce salt and water Slippery to the touch Electrolytes: Conducts electricy in aqueous solutions Strong Acids : Strong Acids HCl HBr HI HNO3 H2SO4 Back Weak Acids : Weak Acids HC2H3O2 HCN HNO2 Back Conjugate Acid Base Pairs : Conjugate Acid Base Pairs Definitions: : Definitions: Neutralization: A reaction between an acid and a base that destroys the properties of both and yields water and a salt PH Indicator: Compounds that change color when going between acidic and basic solutions. They do not enter the reaction. pH<7=Acidic, pH=7=Neutral, pH>7=Basic Definitions: : Definitions: Hydronium Ion: H+ in water is often H3O because the attraction between H+ and H2O is so strong Amphoteric: A substance which can be both an acid and a base H2O H+ + OH- Prelab/homework : Prelab/homework Complete the following equations and balance them: HCl + NaOH HCl + KOH HCl + Ca(OH)2 HCl + NH4OH Prelab/homework : Prelab/homework Complete the following equations and balance them: H2SO4 + NaOH H2SO4+ KOH H2SO4+ Ca(OH)2 H2SO4+ NH4OH You do not have the permission to view this presentation. In order to view it, please contact the author of the presentation.
Chem 120 Acids and Bases aSGuest6757 Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 187 Category: Education License: All Rights Reserved Like it (0) Dislike it (0) Added: December 16, 2008 This Presentation is Public Favorites: 1 Presentation Description No description available. Comments Posting comment... Premium member Presentation Transcript Chapter 19 : Chapter 19 ACIDS AND BASES Chapter 19 : Chapter 19 pH: Power of the Hydrogen ion concentration Hydrogen: P – 1 N – 0 E – 1 Hydrogen +1 P – 1 N – 0 E – 0 Hydrogen Ion Concentration : Hydrogen Ion Concentration Concentration: Measured in Molarity Moles/Liter [H+] = Hydrogen Ion Concentration Brackets mean Concentration [H+] = .01 moles/liter = 1x10-2 M pH = 1x10-2 M = 2 pH Scale : pH Scale 1 – 6 = Acid 7 = Neutral 8 – 14 = Base Objectives: : Objectives: Compare Arrhenius and Bronsted-Lowry definitions. Explain why Bronsted-Lowry is more widely used Describe the similarities and differences in physical and chemical properties of acids and bases Conjugate Acid Base Pairs Definitions Arrhenius vs. Bronsted-Lowry : Arrhenius vs. Bronsted-Lowry Arrhenius: Acids – Yield H+ Bases – Yield OH- Bronsted-Lowry: Acids – Proton Donators Bases – Proton Accepters Properties of Acids and Bases : Properties of Acids and Bases Acids: Sour Taste Change Litmus to Red React with Oxides and Hydroxides of metals to form water and salt Electrolytes: Conducts electricity when dissolved in water Strong Acids and Weak Acids based on how well they disassociate Bases: Bitter Taste Change Litmus to Blue When neutralized with acids, they produce salt and water Slippery to the touch Electrolytes: Conducts electricy in aqueous solutions Strong Acids : Strong Acids HCl HBr HI HNO3 H2SO4 Back Weak Acids : Weak Acids HC2H3O2 HCN HNO2 Back Conjugate Acid Base Pairs : Conjugate Acid Base Pairs Definitions: : Definitions: Neutralization: A reaction between an acid and a base that destroys the properties of both and yields water and a salt PH Indicator: Compounds that change color when going between acidic and basic solutions. They do not enter the reaction. pH<7=Acidic, pH=7=Neutral, pH>7=Basic Definitions: : Definitions: Hydronium Ion: H+ in water is often H3O because the attraction between H+ and H2O is so strong Amphoteric: A substance which can be both an acid and a base H2O H+ + OH- Prelab/homework : Prelab/homework Complete the following equations and balance them: HCl + NaOH HCl + KOH HCl + Ca(OH)2 HCl + NH4OH Prelab/homework : Prelab/homework Complete the following equations and balance them: H2SO4 + NaOH H2SO4+ KOH H2SO4+ Ca(OH)2 H2SO4+ NH4OH