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Understanding Neutralization Reactions and Titration Process

Learn about neutralization reactions when acids and bases react to form salts and water. Discover how titration is used to determine solution concentrations. Explore the key concepts of equivalence, normality, and gram equivalent mass.

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Understanding Neutralization Reactions and Titration Process

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  1. Chapter 21 Section 1 neutralization reaction- when an acid and a base react in an aqueous solution to produce a salt and water *all neutralization reactions are double-replacement ex- RS + TU  TS + RU *must be balanced acid + base  salt + water salt- compound consisting of an anion from an acid and a cation from a base

  2. -The concentration of acid (or base) in a solution can be determined by a neutralization reaction -use acid-base indicators ex- phenolphthalein turns from clear to pink as pH changes from acidic to basic pg 616 figure 21.3 pg 617 figure 21.4

  3. Steps of a Neutralization Reaction -Read and record from page 617 (#1, 2 and 3) standard solution- solution of known concentration *added using a buret titration- process of adding a known amount of solution of known concentration to determine the concentration of another solution end point- point at which the indicator changes color *solution is neutralized

  4. equivalent (equiv)- the amount of acid (or base) that will give one mole of H+ or OH- ions ex- 1mol of HCℓ = 1 equiv of HCℓ 1 mol of H2SO4 = 2 equiv of H2SO4 1 mol of NaOH = 1 equiv of NaOH 1 mol of Ca(OH)2 = 2 equiv of Ca(OH)2 *1 mol of HCℓ will neutralize 1 mol of NaOH *1 mol of HCℓ will not neutralize 1 mol of Ca(OH)2 b/c you need 2 mol

  5. -in a neutralization reaction, the equiv of acid must equal the equiv of base gram equivalent mass- the mass of 1 equiv of a substance

  6. Normality N= equiv/L equiv= (N)(L) *Normality and molarity are equal for acids and bases that give 1 equiv/mol of H+ and OH- ex- 1M HCℓ = 1N HCℓ 1 M NaOH = 1N NaOH *but 1M Ca(OH)2 = 2N Ca(OH)2

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