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Neutralization Reactions in Chemistry

Explore the process of neutralization when mixing acids and bases, understanding equilibrium, reactions, and titrations. Learn about net ionic equations, salt formation, and calculating concentrations in this informative guide.

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Neutralization Reactions in Chemistry

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  1. Mixing Acids and Bases

  2. Is Dilution the Solution? • Some industries produce acidic wastes. Do acids become harmless as they are diluted? • Howmuch H2O is needed to neutralize an acid? • What other choice do we have?

  3. Recall… • In a neutral solution [H+] = [OH-] = 1.0 x 10-7 mol/L • the lower the pH, the more acidic the solution, [H+] > [OH-] • the higher the pH, the more basic the solution, [H+] < [OH-]

  4. Neutralization Equations ACID + BASE  WATER + SALT • Neutralization is a double displacement reaction which produces water and a soluble salt. • HBr (aq) + NaOH (aq) H2O (l) + NaBr (aq) http://www.chem.ox.ac.uk/vrchemistry/chapter16/Movies/Neutralization.swf

  5. Writing neutralization equations When acids and bases are mixed, a salt forms NaOH + HCl  H2O + NaCl base + acid  water + salt Question: Write the chemical reaction when lithium hydroxide is mixed with carbonic acid. Step 1: write out the reactants LiOH(aq) + H2CO3(aq) Step 2: determine products … LiOH(aq) + H2CO3(aq) Li2CO3(aq) + H2O(l) Step 3: balance the equation 2LiOH(aq)+H2CO3(aq)Li2CO3(aq)+2H2O(l) lithium hydroxide + carbonic acid  lithium carbonate + water Ca(OH)2 + H2SO4  2H2O + CaSO4

  6. http://www.saskschools.ca/curr_content/chem30/swf/neutralize.swfhttp://www.saskschools.ca/curr_content/chem30/swf/neutralize.swf

  7. Neutralization • Net Ionic Equation for Neutralization H+ + OH- HOH or H2O • When acids and bases ionize in water, the hydrogen ions (H+) and the hydroxide ions (OH-) are attracted to one another and combine to form water (HOH). • The salt produced from the reaction is soluble in water and therefore becomes the spectator ions.

  8. Neutralization • When a base is added to an acid, 1 mole of the OH- ions react with one mole of the H+ ions, decreasing the concentration of H+ ions. This causes the pH to increase to 7. • When an acid is added to a base, 1 mole of the H+ ions react with one mole of the OH- ions, decreasing the concentration of OH- ions. This causes the pOH increase and the pH to decrease to 7. • Neutralization destroys the properties of acids and bases.

  9. Titration • the progressive addition of an acid to a base, or vice versa, drop by drop from a burette, until the neutralization has occurred • Usually performed to analyse an unknown concentration of acid or base

  10. Some Vocab… • Titrant – a solution of known concentration (standard solution) dispensed from the burette. • Burette – a graduated glass tube with a valve at the bottom used for titrations • Pipette – a glass tube used for transferring small amounts of a solution very accurately

  11. When is a titration finished? • End point – the point at which the indicator changes colour during a titration • We select an indicator based on the the desired equivalence point. • Equivalence point – the point at which the number of moles of acid (H+ ions) added equals the number of moles of base (OH- ions) present or vice versa. n base= nacid

  12. Calculating Concentration • If the concentration of one of the solutions is known (standard solution), the concentration of the second solution can be calculated using stoichiometry. • http://web.fccj.org/~ksanchez/flash/Measurements/titration.swf titration demo

  13. Acid and Base Stoichiometry • A 35.00 mL sample of vinegar requires 51.74 mL of 0.4298 M sodium hydroxide to react with all of the acetic acid. What is the concentration of acetic acid (molarity) in the vinegar?

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