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The student will: be able to explain the experimental technique of titration.

The student will: be able to explain the experimental technique of titration. math calculate the molarity or volume of an unknown solution using the titration formula. ws.19.3. Neutralization Reaction. Strong acid + Strong Base salt + water HCl + H 2 0 H + + Cl -

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The student will: be able to explain the experimental technique of titration.

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  1. The student will: be able to explain the experimental technique of titration. math calculate the molarity or volume of an unknown solution using the titration formula. ws.19.3

  2. Neutralization Reaction Strong acid + Strong Base salt + water HCl + H20 H+ + Cl- NaOH + H20 OH- + Na+ Put them together HCl + NaOH NaCl + H2O Salt: a compound composed of a cation+ from an base and an anion- from a acid.

  3. Stomach Ache CaCO3 ….tums HCl + Mg(OH)2 …milk of magnesia NaCO3 …. Rolaids Neutralize …………..salt + H20 HCl + CaCO3 CaCl + CO2 + H20 HCl + Mg(OH)2 MgCl + H20 HCl + NaCO3 NaCl + CO2 + H2O

  4. Titration: the controlled addition and measurement of of a solution of known concentration required to react completely with a measured amount of solution of unknown concentration Titration:an experiment, a laboratory technique chemist use to determine concentration of an unknown solution. Resources :

  5. ws 19. 3 Titration Problems nMV1 = nMV2 1. Your company produces vinegar, acetic acid (HC2H3O2). Acetic acid is monoprotic. You as the chemist do a quality control experiment. What is the molarity of your company’s vinegar if you titrate a 50mL sample with 30mL of 0.25M LiOH? The vinegar must have a molarity of 0.67M before it can be sold in grocery stores. Is your company’s vinegar ready for market?

  6. 2. A flask contains 50ml sample of potassium hydroxide. This solution is titrated and reaches an equivalence point when 21.88ml of a 0.70M solution H2SO4 is added. Calculate the molarity of this base sample.

  7. 3. A solution of a triprotic acid H3PO4 is used to titrate a 16.25mL sample of .5M RbOH solution. The neutralization point required 25.72mL of the acid. What is the concentration of the acid?

  8. 4. The chemist used a known concentration of .5M HCl to titrate an unknown solution of NaOH. Using a 50mL sample of NaOH the end point was achieved at 32.75mL. What is the molarity of the NaOH?

  9. 5. A volume of 25mL of 2M aluminum hydroxide neutralizes a 75-mL sample of nitric acid solution. What is the concentration of the nitric acid?

  10. 6. A 18.5 mL sample of 0.493M KOH solution required 27.7mL of Carbonic acid in a titration experiment. Calculate the molarity of the acid.

  11. 7. Suppose in a titration experiment it took 22.48mL of 0.454M calcium hydroxide is required to neutralize 10.7mL of hydrofluoric acid. What is the molarity of the acid solution?

  12. 8. If 25.02mL of a solution of Barium hydroxide requires 18.83mL of a 3.64 M solution of phosphoric acid for complete titration, what is the molarity of the base solution?

  13. 9.Find the molarity of a Magnesium hydroxide solution, given that 442mL of it is neutralized in a titration using 65.8mL of 0.0078M Nitric acid.

  14. The student will: be able to explain the experimental technique of titration. math calculate the molarity or volume of an unknown solution using the titration formula. ws.19.3

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