Monday, December 9, 2013

Titration Lab

Titration Lab Period 3 5/20/12 Objective: The main heading of this lab was to determine the marrow squash of atomic number 11 hydroxide call for to offset 10 milliliters of hydrochloric acid. We also had to calculate the one thousand of the atomic number 11 hydroxide using our info. Concepts: Some different concepts used in this lab: indicators, titration formula, titration curves, pH levels, acids, and bases. Materials: Materials used in this lab: a 250mL beaker, ring stand, burette, Erlenmeyer flask, wait cock, burette clamp, 10mL HCL, 10mL NaOH, 3 drops of phenolphthalein, and pH paper. process: 1. Pour 10mL of water into the Erlenmeyer flask. 2. Pour 10mL of HCl into the Erlenmeyer flask. 3. Put terzetto drops of phenolphthalein into the flask. 4. pull wires the flask under the burette. 5. Pour the NaOH by twisting the correspond cock. Shake the flask while spill overing. Pour until a marvelous garden pink co lor starts to appear. At this point pour actually slowly until the whole solution turns a color pink. 6. place down the amount of NaOH poured into the flask. 7. Repeat steps 1-6 until three trials have been recorded. Results: psychometric test| Initial tidy vegetable marrow| Final Volume| Total Volume| Color of the ancestor| pH | 1| .60mL| 8.6mL| 8mL| Bright tip| N/A| 2| 8.6mL| 14.9mL| 6. is a professional essay writing service at which you can buy essays on any topics and disciplines! All custom essays are written by professional writers!
3mL| Semi-Bright ping| N/A| 3| 14.9mL| 21.3mL| 6.3mL| Pale Pink| 7 Yellow| Analysis: The information that we collected, made us infer that the indicator, phenolphthalein, changes to a bright pink color in the presence of a basic! solution. Our data also showed that the electroneutral solution had a lesser amount of NaOH than HCl. This would mean that the NaOH was to a greater extent concentrated than the HCl. We then calculated the molar concentration of NaOH with the masses found in our data. After calculating the molarity of NaOH, we were apt(p) the actual molarity. We compared our calculated molarity to the actual molarity to develop our percent error. Errors: There could have been many...If you want to describe a full essay, order it on our website:

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