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Titrations!

Titrations!. Titrations. Titration : adding a known amount of solution of known concentration to a solution with an unknown concentration Goal: To determine the unknown concentration. Titrations. Endpoint : the point of neutralization in a titration.

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Titrations!

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  1. Titrations!

  2. Titrations Titration: adding a known amount of solution of known concentration to a solution with an unknown concentration Goal: To determine the unknown concentration

  3. Titrations Endpoint: the point of neutralization in a titration How do we know we reached the endpoint in a titration? We can use an indicator and look for a color change! http://www.youtube.com/watch?v=g8jdCWC10vQ

  4. Titration Example #1 A 0.25 L solution of H2SO4 is completely neutralized by 0.5 L of 1.0 M NaOH. What is the concentration (molarity) of the H2SO4 solution? In buret: 1.0 M NaOH In Erlenmeyer flask: ? M H2SO4

  5. 0.5 L NaOH x 1 mol NaOH 1 L NaOH Titration Example #1 A 0.25 L solution of H2SO4 is completely neutralized by 0.5 L of 1.0 M NaOH. What is the concentration of the H2SO4 solution? 1. Write the balanced neutralization reaction H2SO4 + 2 NaOH  Na2SO4 + 2 H2O 2. Start with your known value 0.5 L of 1.0 M NaOH 3. Find the moles of your known using the volume and concentration = 0.50 mol NaOH

  6. 0.50 mol NaOH x 1 mol H2SO4 2 mol NaOH 0.25 mol H2SO4 0.25 L H2SO4 Titration Example #1 continued A 0.25 L solution of H2SO4 is completely neutralized by 0.5 L of 1.0 M NaOH. What is the concentration of the H2SO4 solution? H2SO4 + 2 NaOH  Na2SO4 + 2 H2O 4. Use the molar ratio (the coefficients) to determine the unknown number of moles = 0.25 mol H2SO4 5. Divide the moles by the volume to get concentration = 1.0 M H2SO4

  7. Titration Example #2 A 0.015 L solution of HCl is completely neutralized by 0.025 L of 0.5 M Al(OH)3. What is the concentration of the HCl solution? Show your work for each step: 1. Write the balanced neutralization reaction 2. Start with your known value 3. Find the moles of your known using the volume and concentration 4. Use the molar ratio (the coefficients) to determine the unknown number of moles 5. Divide the moles by the volume to get concentration

  8. 0.025 L Al(OH)3 x 0.5 mol Al(OH)3 1 L Al(OH)3 Titration Example #2 A 0.015 L solution of HCl is completely neutralized by 0.025 L of 0.5 M Al(OH)3. What is the concentration of the HCl solution? 1. Write the balanced neutralization reaction 3HCl + 1 Al(OH)3 1AlCl3 + 3 H2O 2. Start with your known value 0.025 L of 0.5 M Al(OH)3 3. Find the moles of your known using the volume and concentration = 0.0125 mol Al(OH)3

  9. 0.0125 mol Al(OH)3x 3 mol HCl 1 mol Al(OH)3 0.0375 mol HCl 0.015 L HCl Titration Example #2 A 0.015 L solution of HCl is completely neutralized by 0.025 L of 0.5 M Al(OH)3. What is the concentration of the HCl solution? 3HCl + 1 Al(OH)3 1AlCl3 + 3 H2O 4. Use the molar ratio (the coefficients) to determine the unknown number of moles = 0.0375 mol HCl 5. Divide the moles by the volume to get concentration = 2.5 M HCl

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