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

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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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Presentation Transcript
slide1

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
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.

slide3
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

slide4
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 :

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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?

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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.

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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?

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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?

slide9

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?

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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.

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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?

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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?

slide13

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.

slide14

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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