Experiment - chemical changes
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This document outlines six experiments to observe chemical changes. The experiments involve adding iron wool to copper sulfate solution, placing marble chips in hydrochloric acid, mixing sodium sulfate and barium chloride drops, combining bicarbonate of soda and vinegar solutions, adding magnesium to hydrochloric acid, and burning magnesium strips. The goal is to observe signs of chemical reactions occurring and identify common indicators that a chemical reaction has taken place.
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Chemistry 201 Laboratory- Harold Washington College Reac
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Reactions of Copper and Percent Recovery
Introduction
In Chapter 4 of your textbook, we have covered the 3 main classes of reactions in aqueous
solution: precipitation reactions, acid-base reactions, and oxidation-reduction reactions. These
can be summarized as follows:
• In Precipitation reactions: a solid product forms from aqueous reactants. The product can
be predicted by using solubility rules.
• In Acid-base neutralization reactions: an acid (proton donor) reacts with a base (proton
acceptor) to form an ionic salt and sometimes water. You can recognize this type of
reaction by the presence of an acid and base in the reactants.
• In Oxidation-reduction reactions (or redox for short): electrons are transferred between
reactants. So you will always see changes in oxidation number within this type of
reaction.
In this lab, we will be examining these reactions by carrying out a sequence of reactions
starting from metallic copper in the form of a wire. According to the Law of Mass Conservation,
covered in section 2.3 of your textbook, mass is neither created nor destroyed. So since no
copper is added or removed during the course of these reactions, you should be able to
quantitatively recover all of the copper metal you started with at the end of these reactions (if
everything goes well).
You need to carefully observe and record your observations. You should be able to
carefully describe the reactions in terms of color change (color of solution or solid forming), gas
formation (as bubbles), heat generation (change in temperature), or precipitate formation,
throughout the experiment.
At the end of the reactions series, you will collect the copper recovered and calculate the
percent recovery (% yield) of copper using this formula:
% yield = actual amount of Cu recovered x 100 %
original amount of Cu
Materials and Equipment
• Piece of copper wire (about 0.5 g)
• concentrated HNO3 (aq)
• 3.0M NaOH
• 6.0M H2SO4
• solid zinc
• 2-250 mL beakers, 400 mL beaker
• 50 mL graduated cylinder
• boiling chips
• stirring rod
• iron ring and ring stand, wire gauze,
• Bunsen burner
• evaporating dish
• electronic balance
Chemistry 201 Laboratory- Harold Washington College
SAFETY NOTES
• Safety goggles should be worn at all times
• Sulfuric acid, nitric acid, and sodium hydroxide are corrosive chemicals and should be
handled with care.
• Gloves are to be worn when handling these chemicals.
• Waste should be put in the designated container in the hood. Never throw chemicals
down the drain.
PROCEDURE
1. Obtain a piece copper wire, measure its mass to the nearest 0.01 g, and place it in a 400
mL beaker.
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Be careful not to get any of the nitric acid on yourself. If you do, wash it o ...
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2. Procedures are provided for purifying salts through crystallization and filtration. The effects of heat on different salts are also outlined, such as carbonates decomposing to metal oxides and carbon dioxide.
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Pre-lab Questions
1. What is a limiting reagent?
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Procedure
**Take photographs of your experiment set up and your results. Submit them with your laboratory report.**
1. Table 1 provides an example set of data for 1.0 g CaCl2.
2. For Trial 1, weigh into a 250 mL beaker the amount of calcium chloride (CaCl2) shown in Table 1. Record the exact mass you weigh out in the Trial 1 column of the Data section.
3. Measure 50.0 mL of distilled water into a 100 mL graduated cylinder. Pour the water into the 250 mL beaker with the calcium chloride.
4. Stir the solution with a stirring rod until all of the calcium chloride is dissolved.
5. Weigh out 2.5 g of potassium carbonate (K2CO3) in a 50 mL beaker. Record the exact mass in the Data section.
6. Measure 25.0 mL of distilled water into a 100 mL graduated cylinder. Add the water into the 50 mL beaker containing the potassium carbonate.
7. Stir the potassium carbonate in the distilled water with a stirring rod until it is all dissolved.
8. Pour the K2CO3 solution into the 250 mL beaker that has the CaCl2 solution. Rinse the beaker that contained the K2CO3 with a few mL of water and add this to the CaCl2 solution. Stir the mixture.
9. As soon as the reaction begins, record your observations in the Data section. Continue stirring until you see no more precipitate forming.
10. Set up the funnel in the Erlenmeyer flask as shown in Figure 2.
HINT: Do NOT begin filtering yet!
11. Zero the scale and weigh a piece of filter paper and a watch glass. Record the masses of both items in the Data section.
12. Prepare a filtering funnel as shown in Figure 2: fold a piece of filter paper in half twice to make quarters, and open the paper to make a small cone (three quarters are open on one side and one quarter is on the opposite side). Place the paper cone into the funnel and hold it in place with your fingers. Pour a small amount of distilled water through the paper to secure it inside the funnel.
13. Filter the mixture by pouring it into the filter paper in the funnel. Use the stirring rod and distilled water in a wash bottle to transfer the entire solid into the filter paper.
HINT: For best results, be sure to transfer all of the precipitate into the filter paper. Use a rubber policeman if it is available to help with the transfer.
14. Rinse the remaining solid in the filter paper twice with distilled water from a wash bottle to rinse off excess sodium chloride (NaCl). After all the liquid has filtered through, rinse the product with approximately 5 mL of ethanol to aid in its drying. Allow the ethanol to completely finish filtering through the paper.
15. Remove the filter paper carefully so as to not lose any product. Gently unfold the filter paper and lay it flat on the pre-weighed wat ...
TOPIC 4. CHEMICAL REACTIONS -LAB
This document provides instructions and background information for several chemistry experiments involving chemical reactions. The first experiment demonstrates that mixing ammonium nitrate and water is a physical, endothermic reaction that produces a cold pack. The second experiment shows that mixing calcium chloride and sodium bicarbonate produces carbon dioxide gas and causes a color change, indicating a chemical reaction. The document explains how to set up, carry out, observe, and analyze the results of these experiments. It also provides safety precautions and questions to help students understand the differences between physical and chemical reactions.
2p9 reaction rates 221110
This document describes two experiments on the effects of concentration and temperature on reaction speed. The concentration experiment found that calcium carbonate reacted faster with concentrated hydrochloric acid due to more reactant particles. The temperature experiment found that the sodium thiosulfate reaction was faster at 55°C than at 22°C, suggesting higher temperatures increase reaction speed by giving particles more energy to collide. Both experiments demonstrate that higher concentrations and temperatures increase reaction speed.
Unit 4 Lab StoichiometryCHEM 1806Purpose To practice the conce.docx
Unit 4 Lab: StoichiometryCHEM 1806
Purpose: To practice the concept of Stoichiometry
Materials: Student Supplied – Distilled water, paper towels, small paper cup, mug
LabPaq materials: 100 mL glass beaker, Funnel, 25 mL cylinder, Goggles, Digital Scale, Weighing boat, 2.5 g Calcium chloride, dehydrate, Filter paper, 2 g Sodium carbonate.
Procedure:
1. While wearing goggles, weigh out 1.0 g CaCl2 and put it into the 100 mL beaker. Record the actual mass of CaCl2 you are using in Table 1.
2. Add 25 mL of distilled water to the beaker and stir. This is now the “Calcium chloride solution”
3. Calculate how much sodium carbonate you will need for a full reaction. Write that calculation in the Results and Discussion section.
4. Weigh out the calculated amount of Na2CO3 and put it in a small paper cup. (Record actual mass in Data Table 1)
5. Add 25 mL distilled water to the paper cup and stir to make “sodium carbonate solution.”
6. Pour the sodium carbonate solution into the beaker with the calcium chloride solution.
7. Record observations. Write out the reaction of what occurred in the results section. (The solid is calcium carbonate.)
8. Fold the filter paper in half, then in quarters. Record the mass of the filter paper.
9. Place the filter paper in the funnel and open one side.
10. Place the funnel in a mug or other cup to balance it.
11. Carefully swirl and pour the contents of the beaker into the filter paper. (Don’t let the solution overflow.)
12. Rinse the beaker with 1-3mL of distilled water and pour that water into the filter paper as well. (If there is a little solid left in the beaker, leave it. It is experimental error.)
13. When the liquid has drained, lay the filter paper and precipitate on a plate or paper towels to allow it to dry. (mine took overnight, some people take 3 days)
14. When dry, weigh the precipitate + filter paper, record it, and calculate the mass of the precipitate.
15. In the discussion, calculate the theoretical yield and percent yield.
(4 pts) Data:
Table 1: Data
Mass of CaCl2
Mass of Na2CO3 needed
Actual mass of Na2CO3 used
Observation of reaction
Mass of filter paper
Mass of filter paper + precip
Actual yield of Calcium Carbonate
1. (3 pts) Calculate how much Na2CO3 you need to completely react your mass of CaCl2. (Show that calculation here)
2. (2 pts) Write out the reaction that occurred to form calcium carbonate. Remember to identify the phases and balance the equation.
3. (2 pts) Calculate the actual yield of Calcium Carbonate. (Show your work)
4. (2 pts) Calculate the theoretical yield of Calcium Carbonate. (Show your work)
5. (2 pts) Calculate your percent yield of Calcium Carbonate. (Show your work)
Insert a picture of your filter paper with yield for 2 pts extra credit. ;-)
When you are finished, save the file as LASTNAME_Stoich and upload it to the Dropbox for Unit 4 Labs.
Unit 4 Lab: Ionic ReactionCHEM 1806
Purpose: To observe several ionic reactions and practice net ionic equations
...
TOPIC 5. RATE OF REACTION-LAB
The document discusses several experiments on factors that affect the rate of chemical reactions:
1. Particle size - Comparing the reaction of dilute HCl with large vs. small marble chips to see how particle size impacts the reaction rate. Smaller particles react faster due to a greater surface area.
2. Catalyst - Adding manganese dioxide speeds up the decomposition of hydrogen peroxide into oxygen and water, showing how a catalyst increases the reaction rate without being used up in the reaction.
3. Temperature - Measuring the time it takes for tablets to dissolve in hot, room temperature, and cold water, demonstrating that higher temperatures increase molecular motion and collision frequency, speeding up reactions.
CBSE class 12th Chemistry project on antacids for cbse aissce 2017-2018
Cbse class 12th investigatory project of chemistry for AISSCE board Examination
To analyse the given samples of commercial antacids by determining the amount of hydrochloric acid they can neutralize.” for class XII practical examination of the Central Board of Secondary Education in the year 2017-2018.
ebt method.docx
This document provides instructions for titrating HCl against a standard NaOH solution potentiometrically. A known volume of HCl is placed in a beaker and connected to a saturated calomel electrode and hydrogen electrode. Small additions of NaOH are made from a burette and the potential is measured after each addition. The potential readings are plotted against volume added to obtain the titration curve. The equivalence point is identified as the point of maximum slope on the curve or differential curve, indicating where the H+ concentration has changed the most with small volume additions of NaOH base. The experiment allows for the potentiometric titration of a strong acid against a strong base.
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Experiment - chemical changes
- 1. CHEMICAL CHANGES YEAR 8 – CHEMICAL CHANGES
- 2. AIM Aim: To observe chemical changes
- 3. EQUIPMENT • copper sulfate solution • iron wool • 2 beakers • marble chips • dilute hydrochloric acid • 1 test tube • vinegar • bicarb soda • 100 mL measuring cylinder • magnesium strip • sodium sulfate • barium chloride • dropper plate
- 4. RISK ASSESSMENT Risk Injury Prevention Write your risk assessment here.
- 5. METHOD For each of the 6 experiments, make as many observations as you can. Part A: Steel wool and copper sulfate 1. Add 20 mL of copper sulfate solution to a beaker. 2. Put a small amount of iron wool into a beaker. 3. Observe what happens to the iron wool and write this description in your book.
- 6. METHOD Part B: Marble chips and hydrochloric acid 1. Put 5 small marble chips into 1cm depth of hydrochloric acid in a test tube. 2. Record your observations. Part C: Sodium sulfate and barium chloride 1. Add 3 drops of sodium sulfate and 3 drops of barium chloride on a dropper plate. 2. Record your observations.
- 7. METHOD Part D: Bicarb and vinegar 1. Dissolve a level teaspoon of bicarbonate of soda in 50 mL of water. 2. Add 50 mL of white vinegar in another beaker. 3. Tip the bicarbonate solution into the beaker with the vinegar. 4. Record your observations.
- 8. METHOD Part E: Magnesium and hydrochloric acid 1. Add a small amount (5 cm) of hydrochloric acid in a test tube. 2. Add a small strip of hydrogen to this test tube. 3. Gently feel the test tube. 4. Record your observations.
- 9. METHOD Part F: Burning magnesium (DEMO if necessary) 1. Light a Bunsen burner. 2. Using tongs to hold a small strip of magnesium near the flame. 3. Record your observations.
- 10. RESULTS Compile a list of all of the signs of chemical reactions you have encountered today.
- 11. DISCUSSION 1. Using your results, identify some common signs that show a chemical reaction has taken place. 2. Were any of your results reversible? Explain why this might be so?
- 12. CONCLUSION Write your conclusion here.