a) Write a procedure that you would follow to demonstrate the effect of increasingly higher concentrations of hydrochloric acid on its rate of reaction with antacid tablets. You have seen examples of procedures involving the effects of surface area and temperature on this reaction in the lesson and in the Support Questions. Only use the materials listed in the lesson. (5 marks) b) Design a table (giving headings only) for your observations. (2 marks) c) Describe and explain three safety procedures you would have to follow when performing your procedure in a laboratory setting. (3 marks) d) For the procedure that you designed in part (a), describe three different controls you used
measure 10 ml of 1.0M acid and dilute
it with 100 ml of water to make .1M acid
measure 10 ml of .1M acid and dilute it with 100 ml water to make
.01M acid
Keep track of which is which!
Grind up several antacid tablets and weigh out one portion, about
.5g and record how much it weighs. Drop the powder into a beaker
filled with one molarity of acid with your scoop and time how long
it takes for the reaction to stop. Record this and repeat for the
different concentrations of acid.
Detailed procedure:
Some (but not all) antacid tablets contain primarily calcium carbonate, along with flavoring, binders, and other inactive ingredients. These tablets neutralize excess stomach acid, which is actually dilute hydrochloric acid, according to the following equation:
CaCO3(s) + 2HCI(aq) → CaCI2(aq) + CO2(g) + H2O(I)
We’ll use exactly this reaction to observe and quantify the effect of concentration of reaction rates.
Required Equipment and Supplies
Substitutions and Modifications
Procedure
CAUTION: Add Acid to Water and Wait
Table: Effect of concentration on reaction rate – observed and calculated data
Item |
Trial A (4 M HCI) |
Trial B (2 M HCI) |
Trial C (1 M HCI) |
A. mass of tablet |
___.__g |
___.__g |
___.__g |
B. mass of cup + hydrochloric acid |
___.__g |
___.__g |
___.__g |
C. temperature of hydrochloric acid |
___.__°C |
___.__°C |
___.__°C |
D. mass at 0:00 (A + B) |
___.__g |
___.__g |
___.__g |
E. mass at 0:05 |
___.__g |
___.__g |
___.__g |
F: mass at 0:10 |
___.__g |
___.__g |
___.__g |
G: mass at 0:15 |
___.__g |
___.__g |
___.__g |
H: mass at 0:20 |
___.__g |
___.__g |
___.__g |
I: mass at 0:25 |
___.__g |
___.__g |
___.__g |
J: mass at 0:30 |
___.__g |
___.__g |
___.__g |
K: mass at 0:35 |
___.__g |
___.__g |
___.__g |
L: mass at 0:40 |
___.__g |
___.__g |
___.__g |
M: mass at 0:45 |
___.__g |
___.__g |
___.__g |
N: mass at 0:50 |
___.__g |
___.__g |
___.__g |
O: mass at 0:55 |
___.__g |
___.__g |
___.__g |
P: mass at 1:00 |
___.__g |
___.__g |
___.__g |
Q: mass at completion of reaction |
___.__g |
___.__g |
___.__g |
R: mass loss (D – Q) |
___.__g |
___.__g |
___.__g |
S: mass loss percentage [(R/A)·100] |
___.__% |
___.__% |
___.__% |
Safety Procedures:
1. Always add acid to water. Adding water to a concentrated acid can cause splattering.
2. Diluting acid produces heat. Because we want concentration to be the only variable, it’s important to ensure that all three acid solutions are at the same initial temperature.
3. Make your dilute acid solutions ahead of time and allow all three cups to cool to room temperature before proceeding.
a) Write a procedure that you would follow to demonstrate the effect of increasingly higher concentrations...
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