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Understanding Acids, Bases, and Neutralization Reactions

This unit focuses on the fundamentals of acid-base reactions and neutralizations. We examine how acids and bases react in aqueous solutions to form salts and water, alongside the general, complete ionic, and net ionic equations for these reactions. Titration techniques are introduced as a method for determining the concentration of unknown acids or bases by measuring the precise amounts needed to reach the endpoint, marked by indicators that change color based on pH. Practice problems enhance understanding and application of these concepts.

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Understanding Acids, Bases, and Neutralization Reactions

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  1. Unit TwelveAcids and Bases

  2. Neutralizations • Are reactions in which an acid and a base react in an aqueous solution to produce a salt and water • General Equation: HX(aq) + MOH(aq) → MX(aq) + H2O(l) (or: H—OH) • Complete Ionic Equation: H+(aq) + X-(aq) + M+(aq) + OH-(aq) → M+(aq) + X-(aq) + H2O(l) • Net Ionic Equation: H+(aq) + OH-(aq) → H2O(l)

  3. Neutralization Practice • HCl(aq) + NaOH(aq) → • _____________________→ K2SO4(aq) + ________ • HNO3(aq) + Mg(OH)2(aq) → H2O(l) + NaCl(aq) H2SO4(aq) + 2KOH(aq) 2 H2O(l) 2 2H2O(l) + Mg(NO3)2(aq)

  4. Titration - An experimental technique for determining the concentration of an unknown acid/base by comparing it to an acid/base solution of known concentration • How is this done? • By gradually adding and carefully measuring the amount of acid added to a measured amount of base (or vice versa) until the endpoint is reached • What is an endpoint? • The point in the titration when the number of moles of OH- added equals the number of moles of H+ originally in solution • How do we know when the endpoint is reached? • The endpoint is usually signaled by an indicator

  5. Indicators • A dye whose color depends on the pH of the solution • There are many different indicators to indicate different ranges of pH • Phenolphthalein turns from clear (when acidic) to pink (when basic)

  6. Practice Problems • 100.0 mL of an unknown acid is neutralized by 75.0 mL of 3.0 M NaOH. What is the concentration of the unknown acid? • During a titration experiment, 0.250 L of 0.200 M NaOH was needed to completely neutralize 1.00 L of an HCl solution. What was the molarity of the original HCl solution? • In another titration experiment, 30.0 mL of 0.150 M KOH is needed to neutralize 50.0 mL of a fresh HNO3 solution. What was the concentration of the nitric acid?

  7. 10 - 14 6 – 7.6

  8. Worksheet Three is due Friday • Tomorrow there will be an opportunity to retake the Unit Eleven test if you choose. You need to let me know by the end of the day (3-14)

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