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Transcript

Mole to Ratio Lab Presentation

By: Erika Book, Gina Blase, Ty Shaffer, and Connor Paulshock

Chart Data

NaOH

Overview

Data

A balanced chemical equation gives the mole ratios of the reactants and the products as coefficients. When some of the chemical formulas are not known, there is an experiment that can be conducted to help determine the mole ratios.

Volume acid (mL)

Volume NaOH (mL)

Temperature change (°C)

Data Analysis

Procedure

In this experiment, we use two substances, sodium hydroxide (NaOH) and an unknown acid. The prelab chemical reaction is: a A + b NaOH → products. At the end of the experiment, we will find the actual chemical equation.

50

45

40

30

20

15

10

10

15

20

30

40

45

50

1.92

2.67

3.99

6.52

8.50

9.38

6.89

1. Acquire safety equipment

2. Collect materials

3. Set up the Logger Pro program on your computer

4. Measure out the amounts of NaOH and the unknown acid

5. Record the temperature of just the NaOH solution

6. Add the unknown acid and stir the solution until the temperature becomes constant

7. Repeat the previous steps for seven different measurements of the base and acid

Materials

  • The whole number mole ratio of moles of NaOH to moles of acid is 3:1 which equals 3.
  • NaOH is the limiting reactant up until the highest temperature change. After the highest temperature change, the acid is the limiting reactant when there is 50mL of the base because the acid runs out.
  • The mole ratio that we determined in our experiment matched the actual reaction equation’s coefficients. The actual mole ratio, 3:1, was equal to the mole ratio we got, 3:1.
  • The unknown acid, citric acid, is triprotic because its identity is citric acid and because it is able to donate up to 3 protons.

Errors in the Experiment

Objectives

  • Vernier computer interface
  • Two 50 mL graduated cylinders
  • Computer
  • 1.0 M sodium hydroxide, NaOH, solution
  • Logger Pro
  • 1.0 M unidentified acid solution
  • Temperature Probe
  • Three 250 mL beakers
  • Two 10 mL graduated cylinders
  • Foam plastic coffee cups
  • Two 25 mL graduated cylinders

The experiment had two known errors.

The first error was that for one of the measurements the initial temperature was not consistent with the other intial temperatures. We redid that measurement and got better results.

The other error was that one of our peers spilled the unknown acid. So we had to properly clean up our station and redo that measurement.

  • Measure the temperature changes of a series of reactions.
  • Determine the stoichiometry of a reaction in which one of the reactants is known but the other reactant and the products are unknown.
  • Determine whether the unidentified acid is monoprotic, diprotic, or triprotic.

Image of Citric Acid Chemical Formula

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