Titrations
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Titration Definition- To ascertain the concentration of a constituent (here NaCl) by mixing with a constituent of a known concentration
There are two types of Titrations, rough and exact. The differences between the two are...
Rough Titrations- Gives the person(s) conducting the experiment a general idea of how much acid is needed to neutralize the base/alkali
Exact Titrations- Gives the person(s) conducting the experiment the exact amount of acid needed to neutralize the base/alkali
There are two types of Titrations, rough and exact. The differences between the two are...
Rough Titrations- Gives the person(s) conducting the experiment a general idea of how much acid is needed to neutralize the base/alkali
Exact Titrations- Gives the person(s) conducting the experiment the exact amount of acid needed to neutralize the base/alkali
Titration Video
Here is a video showing me conducting a titration experiment.
Titration Procedure
Follow these steps to perform a Titration
1. Take off all loose articles of clothing, tie hair back if you have long hair, put on goggles and smock
2. Gather materials
3. Wash and dry beakers and flask
4. Label one beaker "A" for acid and one beaker "B" for base
5. Pour around 50 cc of Hydrochloric Acid (HCl) into the acid beaker (has a
6. Pour around 50 cc of Sodium Hydroxide (NaOH3) into the base beaker
7. Clean burette by drawing water into it and squirting out
8. Clean burette by drawing HCL into it and squirting out (we do this to make sure there is no water left in the burette)
9. Place burette in clamp stand
10. Place funnel at top of burette
12. Pour around 25 cc of HCL into burette through funnel
13. Record exact amount of HCL in burette
14. Wash flask with water
15. Wash pipette pump with water
16. Wash pipette pump with NaOH
17. Draw 10 cc of NaOH into volumetric pipette using dial/wheel on the side
18. Squirt 10 cc of NaOH into flask using button on side of pipette pump
19. Use pipette to squirt 3 drops of phenolphthalein (NaOH will turn purple, if you didn't know that click here)
20. Place flask under burette
21. Turn dial on burette to allow for the HCL to flow into the NaOH, while this is occurring continually swish the flask in a circular motion by rotating your wrist
22. Watch for the solution in the flask to change from purple to clear
23. Quickly turn the dial on the burette to cease the flow of HCL
24. Record amount of HCL left in burette (should be around 15 cc)
25. Subtract the final amount of HCL from the initial amount of HCL (answer should range from 8-12)
1. Take off all loose articles of clothing, tie hair back if you have long hair, put on goggles and smock
2. Gather materials
3. Wash and dry beakers and flask
4. Label one beaker "A" for acid and one beaker "B" for base
5. Pour around 50 cc of Hydrochloric Acid (HCl) into the acid beaker (has a
6. Pour around 50 cc of Sodium Hydroxide (NaOH3) into the base beaker
7. Clean burette by drawing water into it and squirting out
8. Clean burette by drawing HCL into it and squirting out (we do this to make sure there is no water left in the burette)
9. Place burette in clamp stand
10. Place funnel at top of burette
12. Pour around 25 cc of HCL into burette through funnel
13. Record exact amount of HCL in burette
14. Wash flask with water
15. Wash pipette pump with water
16. Wash pipette pump with NaOH
17. Draw 10 cc of NaOH into volumetric pipette using dial/wheel on the side
18. Squirt 10 cc of NaOH into flask using button on side of pipette pump
19. Use pipette to squirt 3 drops of phenolphthalein (NaOH will turn purple, if you didn't know that click here)
20. Place flask under burette
21. Turn dial on burette to allow for the HCL to flow into the NaOH, while this is occurring continually swish the flask in a circular motion by rotating your wrist
22. Watch for the solution in the flask to change from purple to clear
23. Quickly turn the dial on the burette to cease the flow of HCL
24. Record amount of HCL left in burette (should be around 15 cc)
25. Subtract the final amount of HCL from the initial amount of HCL (answer should range from 8-12)
Molarity
![Picture](/uploads/2/8/7/2/28729727/9702168.jpeg)
Molarity- the number of moles (unit for amount of chemical substance) of solute per liter of solution
To find an unknown molarity in a titration we use this equation...
Molarity of acid x Volume of acid=Molarity of base x Volume of base (M1V1=M2V2)
Ex. If I were to conduct a titration with 20 cc of HCl (HCl has a molarity of 1) and 20 cc of NaOH but I do not know the molarity of NaOH
1 x 20= M x 20
20=20M
M=1
To find an unknown molarity in a titration we use this equation...
Molarity of acid x Volume of acid=Molarity of base x Volume of base (M1V1=M2V2)
Ex. If I were to conduct a titration with 20 cc of HCl (HCl has a molarity of 1) and 20 cc of NaOH but I do not know the molarity of NaOH
1 x 20= M x 20
20=20M
M=1
Click here to learn about making salts!