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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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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.


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


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 :


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?


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.


3. This solution is titrated and reaches an equivalence point when 21.88ml of a 0.70M solution H 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?


4 This solution is titrated and reaches an equivalence point when 21.88ml of a 0.70M solution H. 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?


  • 5. This solution is titrated and reaches an equivalence point when 21.88ml of a 0.70M solution HA volume of 25mL of 2M aluminum hydroxide neutralizes a 75-mL sample of nitric acid solution. What is the concentration of the nitric acid?


6. This solution is titrated and reaches an equivalence point when 21.88ml of a 0.70M solution HA 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.


7. This solution is titrated and reaches an equivalence point when 21.88ml of a 0.70M solution HSuppose 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?


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?


9. 18.83mL of a 3.64 M solution of phosphoric acid for complete titration, what is the molarity of the base solution? 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.


The student will: 18.83mL of a 3.64 M solution of phosphoric acid for complete titration, what is the molarity of the base solution?

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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