Chemistry Notes: Neutralization Chemistry 2014-2015.

Slides:

Advertisements

Similar presentations

1/7/2014Regular Chemistry Assignment #74 Intro to Acids & Bases.

Advertisements

Modern Theories of Acids & Bases

General Properties Indicators Neutralization Reactions

Chapter 14 Acids and Bases 2006, Prentice hall.

LECTURE ELEVEN CHM 151 ©slg Topics: 1. Precipitation Reactions 2. Acid / Base Reactions.

Section 2.4—Defining, Naming & Writing Acids & Bases

 Svante Arrhenius  Acids produce H + ions in water  Bases produce OH - ions in water  A salt is any ionic compound that has formed from the reaction.

Strong and Weak Acids and Bases Pg The strength of an acid is determined by the extent to which it ionizes, its percent ionization, not the concentration.

Acids and Bases Chapter 19. Acids pH less than 7 Sour taste Conduct electricity Reacts with metals to produce hydrogen gas Higher [H + ] concentration.

Conjugate acids and bases. When a substance loses ONE hydrogen ion, the species produced is called a “conjugate base” What’s the conjugate base of H 2.

1 Acid-Base Acid-Base Chemistry acidH + (proton) donor An acid is a H + (proton) donor. acid = H-A General formula of acid = H-A. H-A H + + A - acid proton.

Acid Anything that increases the hydronium ion (H 3 O + ) concentration.

Precipitation reaction – reaction in which an insoluble product forms Precipitate – an insoluble solid that separates from the solution Solubility – maximum.

Day 13– Naming Acids & Bases Sci 10 Chemistry. What is an Acid?  Acid: a compound that makes hydrogen ions H + (aq) when dissolved in water i.e.: HCl.

Modern Theories of Acids & Bases The Arrhenius and Bronsted-Lowry Theories.

Acid-Base Neutralization Reactions Chem 12 Acid + Base  Salt + Water Orange juice + milk  bad taste Orange juice + milk  bad taste Evergreen shrub.

Acid-Base Theories pH Reactions Indicators Titration Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400 Q $500 Final JeopardyJeopardy.

Acids and Bases Acid-Base Theories.  Objectives  Define and recognize Brønsted-Lowry acids and bases  Define a Lewis acid and a Lewis base  Name compounds.

Acid –Base Theories 19.1 A. Acids. Describing an Acid  Tastes “sour”  Common compound in fruits and vegetables  corrosive  Forms electrolytes when.

THIS IS With Host... Your Misc.Acid misc.Base misc.Acid base definitions Titration pH/pOH.

Ch. 14 Acids & Bases.

Acids and Bases. Acids are substances that turn blue litmus red, and usually react with metals such as zinc, releasing hydrogen. Examples: hydrochloric.

Strengths and Naming of Acids + Bases What is a strong acid/base? What is a weak acid/base? Naming Acids + Bases.

Acids and Bases Introduction

Double Displacement 2 compounds are reacted together and the first part of each compound will switch places general equation : WX + YZ  WZ + YX.

Acids and Bases.

Bronsted-Lowry Acid – Base Reactions Chemistry. Bronsted – Lowry Acid Defined as a molecule or ion that is a hydrogen ion donor Defined as a molecule.

Acid/Base Neurtalization. Acid-Base Reactions Acid – substance that increases the H + concentration in aqueous solutions HCl → H + + Cl - H 2 SO 4 → H.

Converting Hydrogen Ion Concentrations to pH Practice Problems.

Definitions. Arrhenius Acids and Bases Acids release hydrogen ions in water. Bases release hydroxide ions in water. An acid is a substance that produces.

Acids, Bases, & pH. I. Macroscopic Properties Easily Observable A. Acids taste sour, bases taste bitter B. Bases feel slippery (soap) C. Acids & Bases.

Acids and Bases. Common household acids Citric acid Ethanoic acid Lactic acid Stearic acid Acetylsailicylic Acid.

Acids and Bases General Formula ACID + BASE  H 2 O + SALT A salt is an ionic ioniccompound.

ACIDS, BASES & SALTS The Arrhenius Theory of Acids and Bases.

Chemistry SM-1232 Week 7 Lesson 1 Dr. Jesse Reich Assistant Professor of Chemistry Massachusetts Maritime Academy Fall 2008.

Acid Base Chemistry. The Electrolyte family Acid Base Salt (Water) Electrolytes conduct electricity.

ACID/BASE Theories & Review

Acid and Base Ch 15 and 16. acids 1. tastes sour. 2. conducts an electric current. 3. Causes certain dyes ( indicators) to change color. 4. Liberates.

Acids & Bases. What is an Acid? Acids are substances that dissociate (fall apart into ions) in water to form hydrogen ions (H + ). Acids are: –Sour-tasting.

Acids, Bases and pH Chapter 19. Compounds That Become Acids When Dissolved in Water General Formula: HX H + X - monatomic or polyatomic anion.

According to the Arrhenius concept, a base is a substance that produce OH - ions in aqueous solution. According to the Brønsted-Lowry model, a base is.

Get Ready for your Quiz! You need When you’re done Tonight’s homework

Chapter 14 Section 2 Acid-Base Theories p Sections 1 -3 Properties of Acids & Bases Acid-Base Theories Acid-Base Reactions MODERN CHEMISTRY.

Acids and Bases. Arrhenius Theory Acids produce H + ions. Acids produce H + ions. Bases produce OH - ions. Bases produce OH - ions. HCl  H + + Cl - NaOH.

ACIDS AND BASES CHEMISTRY CHAPTER 12.

Acid-Base Theories The “Boyz”. Acid and Base Theories2 Arrhenius Theory of Acids Acid: molecular substances that breaks-ups in aqueous solution into H+

CHEMISTRY PART 9 Acids and Bases. Acids  A compound that makes hydrogen ions when dissolved in water.  H + (aq)  Look for the (aq) (which means aqueous)

Bronsted-Lowry Acid Base Chemistry Just a few reminders.

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.

Chapter 8.3b.  Neutralization: reaction between an acid and a base  Neutralization reaction produces a salt and water.  Salt  The negative ions in.

Ch 9: Acids, Bases and Salts Suggested Problems: 2, 6, 10, 12, 28-44, 82, , Bonus: 118.

Acids and Bases Acids: often have a tart or sour taste - Examples include citrus fruits, vinegar, carbonated beverages, car batteries Properties of Acids:

Chapter 15: Acids & Bases Ridgewood High School

© Houghton Mifflin Harcourt Publishing Company Acids 1.Aqueous solutions of acids have a sour taste. 2.Acids change the color of acid-base indicators.

 Acids produce hydrogen ions  HCl  H + + Cl -  Bases produce hydroxide ions  NaOH  Na + + OH - H+H+ OH -

ACIDS AND BASES Chapter 18. Properties of Acids taste SOUR acids change litmus RED their aqueous (water) solutions CONTAIN HYDRONIUM (H 3 O + ) IONS react.

19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 19 Acids, Bases, and Salts 19.1 Acid-Base.

ACIDS AND BASES. Acids 1.Aqueous solutions of acids have a sour taste. 2.Acids change the color of acid-base indicators. 3.Some acids react with active.

Concentrations of Solutions Chapter 10.2 and 10.3 Notes.

Acids, Bases, and Salts. Properties of acids: - contain the hydronium ion, H 3 O + - react with metals to form hydrogen gas, H 2 - taste sour - have pH.

Arrhenius acids Produce H + ions in solutions H + produced by acids is the only positive ion in acidic solutions Properties of acids are related to properties.

Acids, Bases and Salts.

Salt Hydrolysis.

Acids and Bases.

Acid/Base Chemistry Chemistry.

Neutralisation Starter: What ions are found in acids?

Knowledge Organiser – Formulae and equations

Acid/Base Review Honors Chemistry.

Chapter 19.1 Acid-Base Theories

Presentation transcript:

Chemistry Notes: Neutralization Chemistry

When acids and bases react, the products most commonly formed are water and a salt (ionic compound). This is called a neutralization reaction. Examples:HCl + KOH  H 2 O + KCl H 2 SO NaOH  2 H 2 O + Na 2 SO 4 Acid-Base Reactions

What products would you get from the reaction of nitric acid and calcium hydroxide? Write the balanced equation for this reaction. What is the name of the salt created in this reaction?

What products would you get from the reaction of potassium hydroxide and dichromic acid? Write the balanced equation for this reaction. What is the name of the salt created in this reaction?

 When an acid reacts with a base, the base often takes a proton (hydrogen ion) from the acid, which converts the acid to a base (called a conjugate base) and the base to an acid (called a conjugate acid). Conjugate Acid-Base Pairs

For example, when ammonia reacts with hydrochloric acid (shown above), the ammonia removes a proton from the hydrochloric acid. This results in the formation of an ammonium ion (the conjugate acid of ammonia) and a chloride ion (the conjugate base of hydrochloric acid).

Tip for identifying conjugate acid-base pairs— look at the last part of the formula (the anion). It is the same for both members of a conjugate acid-base pair.

For example, when water reacts with nitrous acid, it behaves as a base by removing a proton from nitrous acid. The conjugate base of nitrous acid is the nitrate ion, and the conjugate acid of water is H 3 O +, the hydronium ion. HNO 2 + H 2 O  NO H 3 O + Water is an amphoteric substance— it can behave as an acid or a base.

On the other hand, when water reacts with ammonia, NH 3, it behaves as an acid. The ammonia removes a proton from the water molecule. The conjugate base of water is the hydroxide ion, OH -, and the conjugate acid of ammonia is the ammonium ion, NH 4 +. NH 3 + H 2 O  NH OH -

Nitric acid reacts with ammonia according to the equation HNO 3 + NH 3  NH NO 3 - What is the conjugate base of nitric acid? What is the conjugate acid of ammonia?

Sulfuric acid reacts with lithium hydroxide according to the equation H 2 SO LiOH  2 H 2 O + Li 2 SO 4 What is the conjugate base of sulfuric acid? What is the conjugate acid of lithium hydroxide?

Water reacts with phosphoric acid according to the equation H 2 O + H 3 PO 4  H 3 O + + H 2 PO 4 - Does water act as an acid or a base in this reaction? What is the conjugate acid of water? What is the conjugate base of phosphoric acid?