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# Acid-Base Titration

Joshua Godwin and Andrew Richardson

Chemistry-Fall 2014

Simulation

A acid base titration happens when a acid base reactant is used.

A titration is a technique where a solution of concentration used to find a unknown solution.

There is a indicator for the endpoint of these reactions.

To calculate Acid Base Titration you must find the unknown molarity

Ex. Suppose an aqueous NaOH solution of unknown concentration is added dropwise to 15.5 mL of a 0.150 M aqueous solution of HCl (with an indicator – bromthymol blue). You find that the endpoint (= the inflection point on the graph) is reached when you have added 20.6 mL of NaOH. Find the molarity of the NaOH solution.

Formula: endpoint X (the amount of endpoint and original amount) X (moles divided)

(0.0155 L HCl X 0.150 mol HCl/1 L) X (1 mol NaOH / 1 mol HCl) = 0.00233

mol HCl 0.00233 / mol HCl0.0206 L = 0.113 M HCl

Sources:

http://josephineyeo.files.wordpress.com/2008/09/ti...

http://chemistry.wiki.elanco.net/file/view/titration.jpg/181160813/titration.jpg

http://www.chemistryrules.me.uk/images/titration.png

https://gcs.haikulearning.com

Questions

1) 31.0 mL of an unknown solution of H2SO4 was titrated to the end point with 37.0 mL of 0.425 M KOH. What is the concentration of the sulfuric acid?

2) In a titration, 23.5 mL of a .370 M solution of H2CO3 was used to neutralize 28.6 mL of LiOH. What is the molarity of LiOH?

3) In the titration of 42.0 mL of an NH3 solution, the end point was reached when 36.4 mL of 0.153 M HCl was added. What is the concentration of the ammonia solution?

4) 36.0 mL of HC2H3O2 was neutralized by 17.2 mL of 0.347 M Ca(OH)2. Calculate the concentration of the acetic acid.

5) What volume of 0.320 M H3PO4 neutralizes 25.0 mL of 0.410 M Ba(OH)2?