Acid- Base Reactions Chapter 4 part IV. Characteristics of acids Sour Sour Red litmus test Red litmus test Low pH <7 Low pH <7 Arrhenius: Produce H+ in.

Slides:



Advertisements
Similar presentations
Acids, Bases, and Salts Chapter 19.
Advertisements

There are 3 theories… Arrhenius (most common) Bronsted-Lowry Lewis.
Dr. Namphol Sinkaset Chem 152: Introduction to General Chemistry
Acids & Bases Acids: acids are sour tasting
Stoichiometry of Precipitation Reactions
UNIT 5 Aqueous Reactions and Solution Stoichiometry Acid-Base Neutralization.
Introductory Chemistry: Concepts & Connections Introductory Chemistry: Concepts & Connections 4 th Edition by Charles H. Corwin Acids and Bases Christopher.
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.
Chapter 4.  Definitions  Bronsted - acids are proton donors, bases are proton acceptors  Arrhenius – acids produce H + ions in water and bases produce.
Acid/Base Indicators Substance that changes color in the presence of an acid or a base – Red or Blue Litmus – Phenolphthalein (phth) – Bromothymol blue.
Strong Acid-Base Titrations Chapter 17. Neutralization Reactions Review Generally, when solutions of an acid and a base are combined, the products are.
ACIDS AND BASES.
Acids and Bases.
Jeopardy Acid/Base Reactions And Indicators pH Molarity/ Dilutions Acid/Base Definitions Acid/Base Properties Q $100 Q $200 Q $300 Q $400 Q $500 Q $100.
Volumetric Analysis Titration Dr.Riham Hazzaa
Review 4 Exam 4 on Chapters 9, 15 and 16. Chapter 9 Chemical Reactions Sections (9.1, ) omit Rest of the sections Moles  moles of reactants and.
Acid/Base Review.
Chemistry 101 : Chap. 4 Aqueous Reactions and Solution Stoichiometry (1) General Properties of Aqueous Solutions (2) Precipitation Reactions (3) Acid-Base.
Acids and Bases.
Aim: What are acids and bases?. Acids 1.Acids can be strong or weak electrolytes in aqueous solutions. 2.Acids (ex: HCl) react with certain metals to.
Chapter Arrhenius Concept: Acids produce H + in solution, bases produce OH  ion. In aqueous solutions. Brønsted-Lowry: Acids are H + donors, bases.
Acid/Base Neurtalization. Acid-Base Reactions Acid – substance that increases the H + concentration in aqueous solutions HCl → H + + Cl - H 2 SO 4 → H.
Objectives To learn about reactions between strong acids and strong bases To learn about the reaction between a metal and a nonmetal To understand how.
ACID-BASE THEORIES Svante ArrheniusJohannes BrönstedThomas Lowry.
1 Acids, Bases and Salts Version Acid Properties sour taste change the color of litmus from blue to red. react with –metals such as zinc and magnesium.
Acids and Bases Chapters 15 I. Introduction A. Characteristics of acids 1) formulas BEGIN with Hydrogen 2) taste sour 3) turn blue litmus paper to RED.
Roselyn Dooley, Tyler Schmidt, Kyle Doubleday and Deondré Robinson
Acids and Bases Unit 12. Properties of an Acid  Sour taste  Turns litmus paper red (and responds uniquely to other indicators)  Reacts with:  Hydroxide.
Ch 14.1 Properties of Acids and Bases. Acids  Are sour to taste  React with bases to produce salts and water.  React with metals and release H 2 gas.
1 Reactions in Aqueous Solutions I. 2 Properties of Aqueous Solutions of Acids & Bases Acidic properties taste sour change the colors of indicators turn.
1 Acids, Bases and PH. 2 Some Properties of Acids þ Produce H + (as H 3 O + ) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule)
ACIDS, BASES & SALTS The Arrhenius Theory of Acids and Bases.
Acids and Bases. Acids from the Latin word acere  “ sharp ” or “ sour ” taste sour (but you wouldn ’ t taste an acid to see) change litmus paper red.
Acids & Bases Acids:  acids are sour tasting  Arrhenius acid  Arrhenius acid: Any substance that, when dissolved in water, increases the concentration.
1 Acids, Bases and Salts and Covalent Solutes Chapter 14 Tro, 2 nd ed.
1 Acids, Bases and Salts Version Acid Properties sour taste change the color of litmus from blue to red. react with –metals such as zinc and magnesium.
Acid & Base Solutions. Properties of Acids  What we know about acids:  Sour taste  pH 0 – 7  Turns blue litmus to red  Turns methyl orange to red.
Types of Chemical Reactions and Solution Stoichiometry.
Acids, Bases, and pH. Acids and Bases Acids produce H + ions Bases produce OH - ions.
Introduction to Acids and Bases Chapter 19. What is and Acid? Arrhenius Acid Defined as any chemical that increases the concentration of hydrogen ions.
ACID-BASE REACTIONS.
Acids & Bases. Acids vs. Bases Acids Taste Sour Are Corrosive Bases Taste Bitter Feel Slippery.
Definition of Acids Traditional (Arrhenius)- a chemical compound that contains hydrogen and ionizes in aqueous solutions to form hydrogen ions Examples:
Chapter 15 Acids bases acids Sour Turns litmus red Reacts with some metals to produce H 2 Phenolphthalein-clear Corrosive Conducts electricity bases Bitter.
Acids and Bases Chapter 19. Naming Acids Binary Acids- two different elements in the formula, H is one of them Prefix= hydro Root= second element ends.
Different models help describe the behavior of acids and bases. Section 1: Introduction to Acids and Bases K What I Know W What I Want to Find Out L What.
Unit 14 Acids, Bases, Salts and Titrations. Acids & Bases Acids :  acids are sour tasting  Arrhenius acid: Any substance that, when dissolved in water.
Acid Base Battleship Challenge!!!!. Question 1: If the concentration of NaOH is [0.01], what is the pH? – A.) 2 – B.) 14 – C.) 12 – D.) 0.01.
“K” Chemistry (part 3 of 3) Chapter 15: Acids and Bases.
Acids and Just the Bases Mrs. Herrmann Concentrations of Solutions Concentration—quantitive; a measure of the amount of solute in a given amount of solvent.
Chapter 19 Acids and Bases.
Chapters 14 & 15: Acids and Bases
More on Acids and Bases.
Acids Lesson 1 Acid and Base Properties.
Chapter 4 Acid/base, precipitaton, redox
Acid-Base Reactions - Definitions
Chapter 16 Acids and Bases.
Nonmusical Chairs Review
Homework 3-8 Acid/Base Reactions
Acid/Base Chemistry.
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.
Acid/Base pH and pOH Solubility Molarity Neutral- ization
Aqueous Reactions and Solution Stoichiometry
Acid/Base pH and pOH Solubility Molarity Neutral- ization
Net Ionic Equations Balance the equation
Acids and Bases.
Acid- Base Reactions Chapter 4 part IV.
Acids & Bases Acids: acids are sour tasting
Descriptions & Reactions
Presentation transcript:

Acid- Base Reactions Chapter 4 part IV

Characteristics of acids Sour Sour Red litmus test Red litmus test Low pH <7 Low pH <7 Arrhenius: Produce H+ in water. Arrhenius: Produce H+ in water. Brømsted Lowry: produce protons. Brømsted Lowry: produce protons. Lewis: Electron acceptor. Lewis: Electron acceptor.

Characteristics of bases Slippery & bitter Slippery & bitter Blue litmus test Blue litmus test High pH >7 High pH >7 Arrhenius: forms OH- in water. Arrhenius: forms OH- in water. Brømsted Lowry: accept protons. Brømsted Lowry: accept protons. Lewis: Electron donor. Lewis: Electron donor.

Net Ionic Equation Of all strong acids plus strong bases: H+ + OH-  H2O But what about weak acids and bases? In a strong acid or base, it dissociates completely in water (strong electrolyte) Weak acids and bases do not dissociate completely in water

Weak electrolytes In fact about 90% of acetic acid remains intact in aqueous solution. Therefore the net ionic equation of a weak acid or base includes the intact weak acid or base. Example: HC2H3O2 +Na++ OH-  H2O+ C2H3O2- +Na+ Net Ionic: HC2H3O2 + OH-  H2O + C2H3O2-

Weak electrolytes An example of a weak base is NH 3. An example of a weak base is NH 3. So what is the net ionic equation for hydrochloric acid and ammonia? So what is the net ionic equation for hydrochloric acid and ammonia? HCl + NH 3  NH Cl - HCl + NH 3  NH Cl - H + + Cl - + NH 3  NH Cl - H + + Cl - + NH 3  NH Cl - H + + NH 3  NH 4 + H + + NH 3  NH 4 +

Stoichiometry of an acid/base reaction: The steps. 1. L ist species present in the combined solution, before any reaction occurs. 2. D ecide what reaction will occur. 3. W rite out net ionic equation. 4. C alculate moles of reactant in solution. Use volume of the original solution and its molarity. 5. D etermine the Limiting reagent.

Stoichiometry of an acid/base reaction: The steps. 6. Calculate the moles of required reactant or product formed. 7. Convert to grams or volume as required. 8. In other words, after you answer the question, reread the question and make sure.

Example: What volume of 0.1 M HCl solution is needed to neutralize 25.0 mL of M NaOH? What volume of 0.1 M HCl solution is needed to neutralize 25.0 mL of M NaOH?

Answer List the species: H+ Cl- Na+ OH- List the species: H+ Cl- Na+ OH- What are the possible products? What are the possible products? NaCl (s) And H 2 O (l) NaCl (s) And H 2 O (l) NaCl is soluble therefore it is not a possible product in solution. NaCl is soluble therefore it is not a possible product in solution. Write the balanced equation. Write the balanced equation. H+(aq) + OH-(aq)  H 2 O(l) H+(aq) + OH-(aq)  H 2 O(l)

Answer Calculate moles of reactants: Calculate moles of reactants: OH- = 25 mL NaOH x (1L/1000mL)x (0.350 mol OH-/L NaOH) = OH- = 25 mL NaOH x (1L/1000mL)x (0.350 mol OH-/L NaOH) = 8.75 x10 -3 mol OH x10 -3 mol OH- No limiting reagent, finding volume of HCl No limiting reagent, finding volume of HCl Moles of reactant needed: molar ration is 1:1 therefore need 8.75 x mols acid. Moles of reactant needed: molar ration is 1:1 therefore need 8.75 x mols acid. Convert to volume: V x M=mol Convert to volume: V x M=mol

Therefore V x mol H+ /L = 8.75 x mol H+ V x mol H+ /L = 8.75 x mol H+ V= 8.75 X L V= 8.75 X L