RATE OF REACTION OF CALCIUM Carbonate and HCL
Purpose: This lab was completed to find the rate of reaction of hydrochloric acid with calcium
carbonate, to examine the effects of amount of reactant and concentration on rate of reaction
between HCl and CaCO3, and to examine different methods of determining rate of reaction.
Background: The rate of reaction is defined as how fast or slow a reaction takes place; for the
purposes of this lab, this is essentially equivalent to how quickly reactants are consumed.
According to collision theory, reactions occur at different rates because of the amount of
collisions between reactants with the correct orientation and energy to occur. Reactants must
collide to react, and if they do not collide in the right direction, the particles which must react
will not come into contact with one another; in addition, if they do not have enough energy, the
particles will not be able to react with one another. Number of effective collisions can be
changed through a number of factors, including temperature, pressure, and concentration of
reactant. In this lab, concentration of reactant and amount of reactant were examined for their
effect on the rate of reaction.
Hypothesis: Increase in concentration will speed up a reaction, and increase in amount of
reactant will speed up a reaction. The order of HCl will be one, and the order of CaCO3 will be
one.
Materials:
❏ Calcium carbonate (marble chips and powder)
❏ Hydrochloric acid (6 M, 4 M, 2 M, & 1 M)
❏ Silicon grease
❏ Lab aprons
❏ Goggles
❏ Distilled water
❏ Balance
, ❏ 2 Erlenmeyer flasks
❏ Single buret clamp
❏ Test tube
❏ 2 100 mL beakers
❏ Syringe
❏ Syringe adapter
❏ Stopcock
❏ Stopper, one-hole (must fit flask)
❏ Graduated cylinders
❏ Mortar and pestle
❏ Support stand
❏ Timer (can be stopwatch or phone)
❏ Hot plate
❏ Thermometer
❏ Scoopula
❏ Filter paper
Procedure:
Collection of Gas in a Syringe
1. Measure out about 0.50 g of calcium carbonate (about 3 marble chips. Make sure that the
scale is zeroed before weighing. Place the marble chips in the erlenmeyer flask
2. Lubricate the black tip of the syringe using the silicon grease. Do not put any directly on
the top, but only on the sides.
3. Measure 10 mL of 6 M HCl in a graduated cylinder.
4. Before adding the acid, attach the syringe adapter and stopper to the syringe and secure
the erlenmeyer flask onto the support stand using the buret clamp. Rest the syringe so
that
the rubber stopper is right above the flask.
5. Add the HCl and immediately after secure the stopper in the flask. Have a member in
the group start a timer as soon as the HCl is added. Take measurements of the syringe
every 30 seconds for 10 minutes or until the reaction is finished. Push the syringe down
gently
before taking each measurement.
6. After the 10 minutes is up or the reaction is complete, thoroughly clean the flask with
soap and distilled water.
7. Repeat steps 1-6 using different masses of calcium carbonate, and different
Purpose: This lab was completed to find the rate of reaction of hydrochloric acid with calcium
carbonate, to examine the effects of amount of reactant and concentration on rate of reaction
between HCl and CaCO3, and to examine different methods of determining rate of reaction.
Background: The rate of reaction is defined as how fast or slow a reaction takes place; for the
purposes of this lab, this is essentially equivalent to how quickly reactants are consumed.
According to collision theory, reactions occur at different rates because of the amount of
collisions between reactants with the correct orientation and energy to occur. Reactants must
collide to react, and if they do not collide in the right direction, the particles which must react
will not come into contact with one another; in addition, if they do not have enough energy, the
particles will not be able to react with one another. Number of effective collisions can be
changed through a number of factors, including temperature, pressure, and concentration of
reactant. In this lab, concentration of reactant and amount of reactant were examined for their
effect on the rate of reaction.
Hypothesis: Increase in concentration will speed up a reaction, and increase in amount of
reactant will speed up a reaction. The order of HCl will be one, and the order of CaCO3 will be
one.
Materials:
❏ Calcium carbonate (marble chips and powder)
❏ Hydrochloric acid (6 M, 4 M, 2 M, & 1 M)
❏ Silicon grease
❏ Lab aprons
❏ Goggles
❏ Distilled water
❏ Balance
, ❏ 2 Erlenmeyer flasks
❏ Single buret clamp
❏ Test tube
❏ 2 100 mL beakers
❏ Syringe
❏ Syringe adapter
❏ Stopcock
❏ Stopper, one-hole (must fit flask)
❏ Graduated cylinders
❏ Mortar and pestle
❏ Support stand
❏ Timer (can be stopwatch or phone)
❏ Hot plate
❏ Thermometer
❏ Scoopula
❏ Filter paper
Procedure:
Collection of Gas in a Syringe
1. Measure out about 0.50 g of calcium carbonate (about 3 marble chips. Make sure that the
scale is zeroed before weighing. Place the marble chips in the erlenmeyer flask
2. Lubricate the black tip of the syringe using the silicon grease. Do not put any directly on
the top, but only on the sides.
3. Measure 10 mL of 6 M HCl in a graduated cylinder.
4. Before adding the acid, attach the syringe adapter and stopper to the syringe and secure
the erlenmeyer flask onto the support stand using the buret clamp. Rest the syringe so
that
the rubber stopper is right above the flask.
5. Add the HCl and immediately after secure the stopper in the flask. Have a member in
the group start a timer as soon as the HCl is added. Take measurements of the syringe
every 30 seconds for 10 minutes or until the reaction is finished. Push the syringe down
gently
before taking each measurement.
6. After the 10 minutes is up or the reaction is complete, thoroughly clean the flask with
soap and distilled water.
7. Repeat steps 1-6 using different masses of calcium carbonate, and different
