Microsoft PowerPoint - Chapter 6 Lecture2

Microsoft PowerPoint - Chapter 6 Lecture2 - Exam 1...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
Exam 1 • Location: Lecture Room • 8:00 – 9:00am but we will be her at 7:45am Review – Today in SZB 416 Review Time – 1:00 to 2:30pm • Exam Covers – All lecture notes, homework, all of Chapter 5 in text and Sections 6.1 and 6.2 in Chapter 6 Exam 1 • Bring your own calculator • NO PROGRAMMABLE CALCULATORS! • Test will be multiple choice and scantron (bubble sheets) • Answers will be posted on Quest within 1 hour after exam • Grades will be posted on Quest by end of day 6.3 Neutralization: Bases Are Antacids The Arrhenius Theory • Neutralization reactions are the combination of H + (or H 3 O + ) with OH - to form H 2 O. • Strong acids are acidic substances that ionize 100% in water. – List of aqueous strong acids: – HCl, HBr, HI, H 2 SO 4 , HNO 3 , HClO 4 , HClO 3 • Strong bases are basic substances that ionize 100% in water. – List of aqueous strong bases: – LiOH, NaOH, KOH, RbOH, CsOH, – Ca(OH) 2 , Sr(OH) 2 , Ba(OH) 2 6.3 When acids and bases react with each other, we call this a neutralization reaction . HCl( aq ) + NaOH( aq ) NaCl( aq ) + H 2 O( l ) In neutralization reactions, hydrogen ions from an acid combine with the hydroxide ions from a base to form molecules of water. The other product is a salt (an ionic compound). Neutralization Reactions • Neutral Solutions are neither acids nor base, that is they have equal concentrations of H + and OH -
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
6.3 2 HBr( aq ) + Ba(OH) 2 ( aq ) BaBr 2 ( aq ) + 2 H 2 O( l ) Consider the reaction of hydrobromic acid with barium hydroxide. This reaction may be represented with a molecular, ionic, or net ionic equation: Molecular: Ionic: 2 H + ( aq ) + 2 Br ( aq ) + Ba 2+ ( aq ) + 2 OH ( aq ) Ba 2+ ( aq ) + 2 Br ( aq ) + 2 H 2 O( l ) Net Ionic: 2 H + ( aq ) + 2 OH ( aq ) 2 H 2 O( l ) or by dividing both sides of the equation by 2 to simplify it: H + ( aq ) + OH ( aq ) H 2 O( l ) 45 Reactions in Aqueous Solutions Net ionic equation – Shows ions that participate in reaction and removes spectator ions. Spectator ions do not participate in the
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 11/08/2009 for the course CH 53455 taught by Professor Rowland during the Fall '09 term at University of Texas at Austin.

Page1 / 5

Microsoft PowerPoint - Chapter 6 Lecture2 - Exam 1...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online