Name _______________________________
General Chemistry Virtual Lab: Titration Simulation
You will be performing a virtual titration as practice before
our lab later this week. Go to the following website and then
follow the set-up directions listed below. ***If you go to Mr.
Trows webpage, this activity is hyperlinked already.
http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/flashfiles/stoichiometry/acid_base.html
SETUP
1. Select Type of Reaction: STRONG ACIDS VS. STRONG BASE 2. Fill
the Burette with: BASE 3. Select the Acid and Base: H2SO4 and KOH
(You will need to click on the box to see the selections.) 4.
Select the Indicator: Phenolphthalein
Before beginning the titration, collect or determine the
following information
Molarity of Acid (M): __________________
Volume of Acid (mL): __________________
Convert the Volume of Acid to Liters (L): __________________
PROCEDURE
Your flask contains H2SO4 (an acid) and your burette contains
KOH (a base). We will titrate the acid little by little until we
see the color change from clear to pink. When the color changes for
a second but then returns to colorless, we know we are getting
close to the equivalence point. Continue titrating until the
solution in the flask keeps its color without changing back to
colorless. You have two options for adding more base into your
flask:
1. Add drop by drop from the burette using the DROPWISE button.
2. Slide the bar on the right to add a larger amount of base at one
time. Be careful though - you do not want to
overshoot your end point. If you go too far, you can start over
by hitting CONCORDANT VALUES. Collect or determine the following
data after your solution has changed color
Total Volume of Base in mL: __________________
Convert the Volume of Base to L: __________________
*** Complete the calculations on the following page before you
complete the rest of the simulation ***
CALCULATIONS 1. From your data collected on page 1, fill in the
following given values:
Molarity of Acid = ________________ Molarity of Base =
________________
Volume of Acid = ________________ Volume of Base =
________________
2. Calculate the number of moles of H2SO4 (acid) that were
present in the flask: (show your work) 3. Write the chemical
equation for this particular neutralization reaction below. Make
sure the formulas are correct and that the equation is
balanced.
________________ + ________________ ________________ +
________________
4. What is the molar ratio between H2SO4 and KOH?
____________
Using this ratio, how many moles of KOH must have been added to
the flask? ______________ 5. Using the moles of base (#4) and the
volume of base (#1), calculate the molarity of the KOH solution. 6.
Type the molarity of your KOH solution into box #6 in the online
window. Click OK. a) If your value was correct, the word CORRECT
will appear below the box. Print this page and turn it in
with this lab. b) If your value is incorrect, you will have to
double-check your calculations to find your error. You can then
re-enter the correct value and follow step 6a.
7. Click on the GRAPH button this will only appear if you solved
for the correct molarity. On the grid to the right, draw an
accurate sketch of what your titration curve looks like. Include:
X-axis label and units
Sketch of the curve
?
14 13 12 11 10 9 8 7 6 5 4 3 2 1 0
pH
