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7.03 pH Lab Report

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Erichelle Goitia

on 22 October 2014

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Transcript of 7.03 pH Lab Report

7.03 pH Lab Report
Erichelle Goitia
Conclusion
1. Increasing the amount of the base dilutes the acid resulting in a less acidic reaction. In this case, the NaOH is the base and HCl is the acid. My graph increases because the NaOH is being added.
Data & Observations
Part 1
Trial 1 Trial 2 Trial 3
Initial volume of NaOH in the buret: 0.25 0.25 0.25
Volume of HCl in the flask: 35 25 30
Volume of NaOH remaining at end: 26 34 30
Data & Observations
Part 2
Calculations
1. Volume of sodium hydroxide
Titration with an indicator
Titration with a pH meter
Initial volume of NaOH in buret: 0.25 0.25 0.25
Volume of HCl in flask: 24 30 38
pH when 0 mL of NaOH has been added: 0.7 0.7 0.7
Volume of NaOH remaining at end: 30 30 30
pH of solution each time an increment
of 5 mL of NaOH is added :
pH of solution each time an increment
of 5 mL of NaOH is added :
5|10|15|20|25
30|35|40|45|50
Trial 1 Trial 2 Trial 3
0.91|1.17|1.57|7.00|12.47
0.87|1.06|1.3|1.7|7.00
0.83|0.97|1.14|1.35|1.67
12.7|12.83|12.91|12.91|12.97|13.02
12.4|12.63|12.76|2.85|12.91
2.83|7.00|12.49|12.64|12.75
50mL - 30 mL = 20 mL of NaOH
Since the initial volume was 50 mL, you would subtract that from the end volume which was 30 mL.
2. Molarity of Hydrochloric acid
pH = -log [H3O+]
H+ = -log [-0.30]
H+ = -0.5228
You start by plugging in the pH then solve using log.
2. It's important to stir the solution in the flask as you add titrant from the buret because it ensures that everything in the reaction is complete.
The color in the flask was clear then changed to a light pink as I titrated the NaOH into the HCl.
3. If a student did not remove all of the bubbles from inside the buret, the concentration of the hydrochloric acid would be higher. You probably thought you added more base(NaOH) than what you really added.
4. In this lab, you could've made lots of mistakes. Adding not enough base would leave you with a reaction that is too acidic. The calculated molarity would be too low. Adding too much base would result in a calculated molarity that is too high. You could also make a mistake in calculating the molarity of the hydrochloric acid which could result in being either too high or too low.
As I titrated the NaOH into the HCl, the pH always rises.
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