Today’s Objective Predict the products of neutralization reactions. Acid-Base Chemistry Tentative Test Date Monday, April 19th Today’s Objective Predict the products of neutralization reactions.

Neutralization Reactions Acid + Base  Salt + Water Salt = Ionic Compound Example HCl + Ca(OH)2  CaCl2 + H2O Acid Water Base Salt

Example #1 Carbonic acid is used to neutralize potassium hydroxide. H2CO3 2 + KOH  K2CO3 2 + H2O Most neutralization reactions are double replacement reactions, so the two positive ions switch places!

Example #2 Magnesium hydroxide is a common active ingredient in antacids. It can neutralize the excess hydrochloric acid in your stomach. Mg(OH)2 + HCl 2  MgCl2 + H2O 2

Acid-Base Chemistry Tentative Test Date Today’s Objective Monday, April 19th Today’s Objective Determine the relative pH of salts produced in neutralization reactions. Perform calculations related to titrations.

Strong versus Weak Strong Electrolytes Weak Electrolytes Completely Dissociate HA  H+ + A- Partially Dissociate HA  H+ + A- Assume you have a strong acid and a weak acid of the same concentration. Which acid would have a higher concentration of H+ ions? Which acid would have a lower pH or be more acidic? The Strong Acid The Strong Acid

List of Strong Acids & Bases Strong Bases Hydrochloric Acid (HCl) Hydrobromic Acid (HBr) Hydroiodic Acid (HI) Nitric Acid (HNO3) Sulfuric Acid (H2SO4) Perchloric Acid (HClO4) Group 1A Hydroxides Example: NaOH Barium Hydroxide Ba(OH)2 Strontium Hydroxide Sr(OH)2 MEMORIZE ME!!

Concentrated vs Dilute Larger Quantities of Solute in a Given Amount of Solvent Higher Molar Concentrations Does not depend on whether the solute is strong or weak Larger Quantities of Solute in a Given Amount of Solvent Lower Molar Concentrations Does not depend on whether the solute is strong or weak

What’s What? Looking at the Petri dish models, categorize them as one of the following. Strong and Concentrated Strong and Dilute Weak and Concentrated Weak and Dilute

Salts of Neutralization Reactions Acid Base Salt Strong Neutral Weak Basic Acidic Need More Information

Example #1 Write the neutralization reaction that occurs between nitric acid and aluminum hydroxide. Determine if the salt produced will be acidic, basic, neutral, or if more information would be needed. 3 HNO3 + Al(OH)3  Al(NO3)3 + 3 H2O Strong Acid Weak Base Acidic Salt

We would need more information! Example #2 Write the neutralization reaction that occurs between phosphoric acid and calcium hydroxide. Determine if the salt produced will be acidic, basic, neutral, or if more information would be needed. 2 H3PO4 + 3 Ca(OH)2  Ca3(PO4)2 + 6 H2O Weak Acid Weak Base ???? Salt We would need more information!

Titrations A titration is a laboratory procedure used for determining the concentration of an unknown solution. A Buret Filled with the Titrant An Erlenmeyer Flask with the Analyte Ring Stand

Example #1 In the prep room, there is a mystery solution of NaOH. Mrs. Stiles wants to determine its concentration, so she titrates a 25.0mL sample of NaOH solution using 0.25M sulfuric acid. If it takes 33.0mL of sulfuric acid to neutralize the base, determine the concentration of the NaOH solution. Steps to Solve Write a BALANCED chemical reaction. Determine the moles of “KNOWN” solution. Use a molar ratio to determine the moles of “UNKNOWN” solution. Determine the concentration of the “UNKNOWN” solution.

Example # 1 - Continued H2SO4 + 2 NaOH  Na2SO4 + 2 H2O Moles of “KNOWN” = Moles of Sulfuric Acid 0.00825 mol H2SO4

Example #1 - Continued H2SO4 + 2 NaOH  Na2SO4 + 2 H2O

Example #2 A 10.0mL sample of acetic acid is analyzed using calcium hydroxide as the base. If a student used 30.0mL of a 0.15M solution of calcium hydroxide to completely react with the sample of acetic acid, determine the concentration of the acetic acid. 2 HC2H3O2 + Ca(OH)2  Ca(C2H3O2)2 + 2 H2O

2 HC2H3O2 + Ca(OH)2  Ca(C2H3O2)2 + 2 H2O Example #2 - Continued A 10.0mL sample of acetic acid is analyzed using calcium hydroxide as the base. If a student used 30.0mL of a 0.15M solution of calcium hydroxide to completely react with the sample of acetic acid, determine the concentration of the acetic acid. 2 HC2H3O2 + Ca(OH)2  Ca(C2H3O2)2 + 2 H2O 0.0045 mol Ca(OH)2

2 HC2H3O2 + Ca(OH)2  Ca(C2H3O2)2 + 2 H2O Example #2 - Continued A 10.0mL sample of acetic acid is analyzed using calcium hydroxide as the base. If a student used 30.0mL of a 0.15M solution of calcium hydroxide to completely react with the sample of acetic acid, determine the concentration of the acetic acid. 2 HC2H3O2 + Ca(OH)2  Ca(C2H3O2)2 + 2 H2O