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How to Make Copper Sulphate in a Science Lab

Last Updated: May 26, 2022

This article was co-authored by Chris Hasegawa, PhD . Dr. Chris Hasegawa was a Science Professor and the Dean at California State University Monterey Bay. Dr. Hasegawa specializes in teaching complex scientific concepts to students. He holds a BS in Biochemistry, a Master’s in Education, and his teaching credential from The University of California, Davis. He earned his PhD in Curriculum and Instruction from The University of Oregon. Before becoming a professor, Dr. Hasegawa conducted biochemical research in Neuropharmacology at the National Institute of Health. He also taught physical and life sciences and served as a teacher and administrator at public schools in California, Oregon, and Arizona. This article has been viewed 163,449 times.

Copper sulfate is an inorganic compound commonly found in pesticide products used to kill bacteria, algae, plants, snails, and fungi. [1] X Trustworthy Source National Pesticide Information Center Organization run by Oregon State University providing objective, science-based information about pests and pesticides Go to source It is a combination of copper oxide and sulfuric acid. Copper sulfate is also often used to grow brilliant blue crystals as a fun science experiment.

Making a Copper Sulfate Solution

• Eye Protection
• Latex Gloves
• Glass Beaker
• Conical Flask
• Glass Stirring Rod
• Evaporating Dish
• Bunsen Burner
• Filter Paper
• Filter Funnel

Filtering the Copper Sulfate Solution

• Polythene filter funnels are cheaper and safer than glass funnels. The filter funnel diameter is should not be too big. Otherwise, the filtration set-up will be unstable. [13] X Research source

Growing Copper Sulfate Crystals

• This evaporative crystallization method may take a few weeks depending on how warm the area where the beaker is being stored is. Well-formed crystals will grow. [18] X Research source
• You can also heat the solution over a Bunsen burner until one half to two thirds of the water has evaporated. Allow the solution to cool. This cooling crystallization method will most likely result in irregularly shaped crystals. [19] X Research source

Community Q&A

Remember, copper sulfate is a harmful irritant. Do not ingest. Handle with care, and always wash your hands after touching it.

Things You'll Need

• Copper Oxide
• Sulphuric Acid

You Might Also Like

• ↑ http://npic.orst.edu/factsheets/cuso4gen.html
• ↑ http://www.nuffieldfoundation.org/practical-chemistry/reacting-copperii-oxide-sulfuric-acid
• ↑ Chris Hasegawa, PhD. Retired Science Professor & Dean. Expert Interview. 29 July 2021.
• ↑ http://www.scienceprojectlab.com/growing-crystal.html

About this article

To make copper sulfate in a science lab, start by pouring sulfuric acid into a glass beaker and heating it until it's almost boiling. Then, carefully add small pieces of copper oxide to the hot solution, stirring the mixture lightly for 30 seconds after each addition. Keep heating the solution for 1-2 minutes or until it looks cloudy with black powder. Finally, turn off the burner and set the copper sulfate solution aside to cool. To learn how to make crystals with your copper sulfate solution, scroll down! Did this summary help you? Yes No

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Copper crystals in a beautiful pattern

Some people are familiar with the process of growing crystals of copper sulfate, or even copper acetate. However, very few people know that you can make beautiful metallic copper crystals through a simple oxidation-reduction reaction with zinc . This is easily done on a piece of filter paper in a petri-dish.

Procedure for beautiful copper crystals

• Prepare a solution of copper sulfate pentahydrate. You won’t need much. I usually dissolve 7.5 grams of copper sulfate in 50ml of distilled water.
• Cut a piece of filter paper so it just fits inside a petri dish
• Place a dry filter paper into the petri dish
• Pour a small amount of copper sulfate solution into the petri dish, soaking the filter paper.
• After a few seconds, pour out the solution, so you are left with a wet piece of filter paper.
• Place a tiny piece of zinc metal, or a small amount of zinc powder, in the middle of the filter paper.
• Wait until the metallic copper forms around the zinc. You should see some within minutes.

Tips and tricks

• If you don’t get the beautiful tree / fractal pattern like shown in our photo, try soaking the filter paper with more or less copper sulfate
• Copper sulfate is toxic, keep the solution away from eating and living areas, and use proper PPE (gloves and goggles)
• Copper sulfate can be purchased at hardware stores as Rooto root killer. It is once of the most useful compounds for chemistry experiments.
• It’s normal for it to take a little while for all of the CuSO 4 to dissolve
• The copper crystals will be very small, use a magnifying glass to see them better.
• Give the crystals an hour or two to form.

Explanation of the chemistry

The copper is being reduced from copper (II) ions to elemental copper, by zinc which is possibly the most useful reducing agent you can have. The zinc is oxidized from elemental zinc to the zinc (II) ion. The sulfate ion acts as a spectator ion.

Net ionic reaction: Cu +2 + Zn(s) -> Cu(s) + Zn +2

This reaction occurs spontaneously because zinc is higher than copper in the activity series of metals . You will find memorizing the order of the activity series helpful in mastering chemistry .

Large amounts of elemental copper can be more easily formed from a copper sulfate solution via a different method, which we will explore in a different article. Like gallium , elemental copper is non-toxic.

Additional Experiments

Make copper powder from aluminum foil Make beautiful tin crystals

2:42 practical: prepare a sample of pure, dry hydrated copper(II) sulfate crystals starting from copper(II) oxide

Excess Solid Method :

Preparing pure dry crystals of copper sulfate (CuSO 4 ) from copper oxide (CuO) and sulfuric acid (H 2 SO 4 )

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How to Make Copper Sulfate Crystals: A Step-by-Step Guide

Are you interested in creating your own copper sulfate crystals this step-by-step guide will walk you through the process, helping you produce stunning, blue crystals that can be used for various purposes. let’s get started.

What You’ll Need

Before diving into the process, gather the following materials:

• Copper oxide or copper carbonate
• Sulfuric acid
• Distilled water
• Glass container or beaker
• Plastic spoon or stirring rod
• Paper towels
• Safety goggles and gloves

Step 1: Safety First

Prioritize your safety by wearing goggles and gloves throughout the entire process. Copper sulfate can cause irritation, so take necessary precautions to avoid direct contact with your skin, eyes, or inhaling any fumes.

Step 2: Mixing the Ingredients

Add the copper oxide or copper carbonate to the glass container or beaker. Measure and pour the sulfuric acid into the container, making sure to follow the recommended ratios provided by the manufacturer. Then, carefully add distilled water to dilute the mixture.

Step 3: Stirring and Dissolving

Using the plastic spoon or stirring rod, mix the ingredients thoroughly. Make sure the copper oxide or copper carbonate is fully dissolved in the solution. Gradually, you will observe the solution changing color, indicating the formation of copper sulfate.

Step 4: Filtering the Solution

To remove any impurities or undissolved particles, filter the solution using a paper towel. This will ensure that your final crystal product is of high purity and quality.

Step 5: Crystallization

Set the filtered solution aside in a cool and undisturbed location. Allow evaporation to occur gradually over the next few days. As the water dissipates, copper sulfate crystals will start to form.

Step 6: Harvesting the Crystals

After several days, carefully examine the container. You should notice beautiful blue crystals at the bottom. Use a spoon or any suitable tool to collect the crystals and let them dry on a paper towel.

Step 7: Additional Tips

Here are some extra tips to enhance your copper sulfate crystal-making experience:

• Experiment with different concentrations of chemicals to achieve varying crystal sizes and shapes.
• Consider growing crystals using different methods, such as with a seed crystal or through slow cooling.
• Store your copper sulfate crystals in a dry and airtight container to prevent moisture absorption and preserve their quality.

Now that you have a step-by-step guide on making copper sulfate crystals, why not give it a try? Remember to always prioritize safety and enjoy the magical process of crystal formation!

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Practical: Prepare Copper(II)Sulfate ( Edexcel IGCSE Chemistry )

Revision note.

Chemistry Lead

Practical: Prepare Copper(II)Sulfate

To prepare a pure, dry sample of hydrated copper(II) sulfate crystals

• 1.0 mol / dm 3  dilute sulfuric acid
• Copper(II) oxide
• Spatula & glass rod
• Measuring cylinder & 100 cm 3  beaker
• Bunsen burner
• Tripod, gauze & heatproof mat
• Filter funnel & paper, conical flask
• Evaporating basin and dish.

Preparation of a soluble salt from an insoluble base and acid

The preparation of copper(II) sulfate by the insoluble base method

• Add 50 cm 3  dilute acid into a beaker and warm gently using a Bunsen burner
• Add the copper(II) oxide slowly to the hot dilute acid and stir until the base is in excess (i.e. until the base stops dissolving and a suspension of the base forms in the acid)
• Filter the mixture into an evaporating basin to remove the excess base
• Gently heat the solution in a water bath or with an electric heater to evaporate the water and to make the solution saturated
• Check the solution is saturated by dipping a cold glass rod into the solution and seeing if crystals form on the end
• Leave the filtrate in a warm place to dry and crystallise
• Decant excess solution and allow the crystals to dry

Practical Tip

• The base is added in excess to use up all of the acid, which would become dangerously concentrated during the evaporation and crystallisation stages
• Hydrated copper(II) sulfate crystals should be bright blue and regularly shaped

Make sure you learn the names of all the laboratory apparatus used in the preparation of salts.

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How to Make Copper Sulfate (Copper Sulphate)

It’s easy to make copper sulfate using readily available materials. Copper(II) sulfate is also known as copper sulphate, blue vitriol, or bluestone. Usually, it is a vibrant blue salt encountered as copper sulfate pentahydrate (CuSO 4 ·5H 2 O). The chemical has several uses, but most people use it for growing blue blue copper sulfate crystals .

Here is how you make copper sulfate yourself, using a battery, copper wire, and dilute sulfuric acid.

Materials for Making Copper Sulfate

The easiest and safest method of making copper sulfate uses electrochemistry.

• Copper wire (which is high-purity copper )
• Sulfuric acid (H 2 SO 4 or battery acid )
• 6-volt Battery

Concentrated sulfuric acid (like the kind in a lab) is 98% sulfuric acid and 2% water, with a concentration of 18.4 M. That is too strong for this project, so you need to dilute it. If you have dilute sulfuric acid, go ahead and use that. If you’re making copper sulfate at home, you’re probably using battery acid, which averages around 37% acid in water or about 4 M. You don’t need to dilute it much in this project.

While the instructions call for a 6-volt battery, a 9-volt battery or a constant power supply work fine.

Make Copper Sulfate

• Pour 30 ml of water and then 5 ml concentrated sulfuric acid into a small glass jar or beaker. Always add acid to water , not the other way around. This minimizes the chance of the acid splashing. For battery acid, use less water. The concentration of acid is not critical, so either 30 milliliters of acid in 40 milliliters of water or mixing half battery acid and half water is fine.
• Inspect your wires. If they are insulated, strip enough insulation that you have bare copper ends to put in the liquid. Attach a copper wire to each battery terminal and immerse the exposed ends in the solution to that the wires are not touching each other.
• The liquid turns blue as copper sulfate is produced.

Concentrate the Copper Sulfate

The reaction between sulfuric acid and copper yields a dilute copper(II) sulfate solution. If left undisturbed, copper sulfate crystals form as the water evaporates. However, the solution still contains some sulfuric acid, so use care when removing the crystals (which are your solid product).

Alternatively, concentrate the solution by boiling it. After evaporating the liquid, blue copper sulfate powder remains. Any remaining liquid that does boil away is concentrated sulfuric acid. Pour this liquid off and save it for future science experiments.

Once you have copper sulfate, dissolve it in water and grow copper sulfate crystals.

Tips for Success

When you run electricity through the copper electrodes, expect bubbling from the anode (negative electrode) in the liquid. These bubbles contain hydrogen gas. Meanwhile, the copper at the cathode (positive electrode) dissolves. Some of the dissolved copper ions make their way to the anode and are reduced. When this happens, it reduces the copper sulfate yield. But, a little care with the set-up reduces the loss.

If you have enough wire, coil the copper for the cathode (connected to the “+”) and place it on the bottom of the jar or beaker. Either leave the wire insulation in place above the coil or else slide a section of plastic tubing (such as aquarium tubing) over exposed wire just above the coil. This minimizes the reaction between the cathode and anode. Place the anode (connected to the “-“) higher in the liquid and distant from the coil. Ideally, hydrogen bubbles only form from the anode. If both electrodes bubble, move the copper wires further apart. With this set-up, copper sulfate forms at the bottom of the container, near the cathode.

Make Copper Sulfate Using Sulfuric Acid and Nitric Acid

While the electrochemical method is the safest way of making copper sulfate, there are other synthesis routes. Another method uses sulfuric acid, nitric acid, and copper (either as a chunk or wire). The disadvantage is that nitric acid and concentrated sulfuric acid are not common home chemicals. They come from a chemical supply store. The acid mixture is highly corrosive and produces toxic vapor, so the procedure is best done in a fume hood. This reaction is popular as a chemistry demonstration because of the color changes. Note that the product includes both copper(II) sulfate and copper(II) nitrate.

• 70% nitric acid
• concentrated (98%) sulfuric acid
• Place 30 milliliters of water in a beaker.
• Add 5 milliliters of nitric acid and 3 milliliters of concentrated sulfuric acid.
• Gently drop about 6 grams of copper into the acid solution. The reaction releases a brown gas and the solution turns blue.
• Within the fume hood, let the acid evaporate. Collect the copper sulfate crystals.

Make Copper Sulfate Using Sulfuric Acid and Hydrogen Peroxide

You can make copper sulfate from copper in a mixture of sulfuric acid and hydrogen peroxide called piranha solution . This is not a recommended synthesis method. It is not very efficient and the acid and peroxide often boil during mixing and may overflow or break a glass container. While 30% hydrogen peroxide is available from a beauty supply store, the concentrated sulfuric acid comes from a chemical supply store.

• 30% hydrogen peroxide (H 2 O 2 )
• concentrated (98%) sulfuric acid (H 2 SO 4 )
• Pour 10 milliliters of 30% hydrogen peroxide into a borosilicate glass beaker.
• Add 3 milliliters of concentrated sulfuric acid. This reaction is exothermic , so expect heat!
• Carefully add about 3 grams of copper. The copper bubbles and the clear liquid turns blue.
• Pour the liquid onto a shallow glass dish. Leave any remaining copper in the original container. Copper sulfate crystals form as the liquid evaporates.

Copper Sulfate Safety and Disposal

• Wear gloves and eye protection. Sulfuric acid is corrosive and causes burns upon contact. Do not touch or inhale the acid. In the event of a splash, immediately rinse the affected are with lots of water. Neutralize a spill using a weak acid, such as baking soda. Then, rinse with plenty of water.
• Avoid skin contact with the copper sulfate solution. Copper sulfate is a skin irritant. It is only mildly toxic, but please don’t drink the liquid. It still contains some acid and may be corrosive. In case of accidental contact, rinse affected skin with water.
• While municipal water treatment can handle copper just fine, copper sulfate is toxic to invertebrates, so don’t dump copper sulfate outdoors. Rinse unused product down the drain with plenty of water.
• Clayton, G. D.; Clayton, F. E. (eds.) (1981). Patty’s Industrial Hygiene and Toxicology (3rd ed.). Vol. 2, Part 6 Toxicology. NY: John Wiley and Sons. ISBN 0-471-01280-7.
• Copper Development Association Inc. “ Uses of Copper Compounds: Copper Sulphate .”
• Wiberg, Egon; Nils Wiberg; Arnold Frederick Holleman (2001). Inorganic Chemistry . Academic Press. ISBN 978-0-12-352651-9.
• Zumdahl, Steven; DeCoste, Donald (2013). Chemical Principles . Cengage Learning. ISBN 978-1-285-13370-6.

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A reversible reaction of hydrated copper(II) sulfate

In association with Nuffield Foundation

• Five out of five

In this experiment the water of crystallisation is removed from hydrated blue copper(II) sulfate. After cooling the anhydrous copper(II) sulfate formed is then rehydrated with the same water

Students remove the water of crystallisation from hydrated copper(II) sulfate by heating. Condensing the vapour produced in a second test tube collects the water. The white anhydrous copper(II) sulfate is then rehydrated and the blue colour returns.

This experiment can be carried out in pairs by students. It should take no more than 30–40 minutes.

• Eye protection
• Test tubes x2
• Delivery tube (right-angled)
• Beaker, 250 cm 3
• Bunsen burner
• Clamp and stand
• Copper(II) sulfate(VI)–5–water (powdered), (HARMFUL, DANGEROUS FOR THE ENVIRONMENT), about 5 g

Health, safety and technical notes

• Read our standard health and safety guidance
• Wear eye protection. 
• Copper(II) sulfate(VI)-5-water, CuSO 4 .5H 2 O(s), (HARMFUL, DANGEROUS FOR THE ENVIRONMENT) – see CLEAPSS Hazcard  HC027c .

Source: Royal Society of Chemistry

• Set up the apparatus as shown (but without water in the receiving tube – this is to be collected during the experiment), placing about 5 g of powdered hydrated copper(II) sulfate in the test tube. Make sure that the tube is clamped near the bung as shown.
• Heat the blue copper(II) sulfate until it has turned white. Move the flame along the length of the test tube from time to time (avoiding the clamp) to prevent water condensing on the cooler regions and then running down on to the hot solid, possibly cracking the test tube. Do not heat too strongly, nor allow the white colour to darken, as the copper sulfate may decompose to produce toxic sulfur oxides.
• Act quickly to prevent suck-back if the level of water collecting in the test-tube reaches the end of the delivery tube. Lift the clamp stand so that the delivery tube does not reach into the water in the test tube.
• Allow the anhydrous copper(II) sulfate to cool back to room temperature.
• Holding the test tube containing anhydrous copper(II) sulfate in one hand, pour the collected water very slowly on to the white powder. What observations can you make?
• Record any observations made during the heating process and when the water was poured back onto the anhydrous copper(II) sulfate.

Teaching notes

Ensure that the students have clamped the test-tube at the end nearest the bung before they start the experiment, otherwise they will be heating the clamp as well as the test tube.

Warn about, and watch for, suck-back. Demonstrate how to lift the entire clamp stand and apparatus.

The reaction involved is:

CuSO 4 .5H 2 O(s) (pale blue solid)  ⇌ CuSO 4 (s) (“dirty” white solid) + 5H 2 O(l)

Students should observe the colour change from pale blue to white and the change back to blue when water is added. The colour change on adding water to anhydrous copper(II) sulfate has been used as a test for the presence of water in a liquid.

The more observant should notice that the addition of water to anhydrous copper(II) sulfate is exothermic, as the tube becomes noticeably hot if the water is added very slowly. They should therefore conclude that the same quantity of energy is absorbed when the endothermic thermal decomposition takes place.

Perhaps in subsequent class discussion students could be asked why anhydrous copper(II) sulfate would not be a feasible fuel for the future.

More able and older students might be asked to calculate the enthalpy change occurring during this process. They will need to find out from a data book the standard enthalpies of formation for anhydrous and hydrated copper(II) sulfate, as well as that for water.

More resources

Add context and inspire your learners with our short career videos showing how chemistry is making a difference .

Additional information

This is a resource from the  Practical Chemistry project , developed by the Nuffield Foundation and the Royal Society of Chemistry. This collection of over 200 practical activities demonstrates a wide range of chemical concepts and processes. Each activity contains comprehensive information for teachers and technicians, including full technical notes and step-by-step procedures. Practical Chemistry activities accompany  Practical Physics  and  Practical Biology . 

© Nuffield Foundation and the Royal Society of Chemistry

• 11-14 years
• 14-16 years
• 16-18 years
• Practical experiments
• Compounds and mixtures
• Properties of matter
• Rates of reaction

Specification

• Using mass of substance, Mᵣ, and amount in moles.
• 8. be able to calculate reacting masses from chemical equations, and vice versa, using the concepts of amount of substance and molar mass
• d) the terms anhydrous, hydrated and water of crystallisation and calculation of the formula of a hydrated salt from given percentage composition, mass composition or based on experimental results
• If a reversible reaction is exothermic in one direction, it is endothermic in the opposite direction. The same amount of energy is transferred in each case. For example: hydrated copper sulfate (blue) ⇌ anhydrous copper sulfate (white) + water.
• In some chemical reactions, the products of the reaction can react to produce the original reactants. Such reactions are called reversible reactions and are represented: A + B ⇌ C + D.
• Recall that some reactions may be reversed by altering the reaction conditions.
• 4.13 Recall that chemical reactions are reversible, the use of the symbol ⇌ in equations and that the direction of some reversible reactions can be altered by changing the reaction conditions
• C6.3.1 recall that some reactions may be reversed by altering the reaction conditions including: reversible reactions are shown by the symbol ; reversible reactions (in closed systems) do not reach 100% yield
• C5.3a recall that some reactions may be reversed by altering the reaction conditions
• C6.3.1 recall that some reactions may be reversed by altering the reaction conditions including: reversible reactions are shown by the symbol ⇌; reversible reactions (in closed systems) do not reach 100% yield
• C5.2a recall that some reactions may be reversed by altering the reaction conditions
• 9. Consider chemical reactions in terms of energy, using the terms exothermic, endothermic and activation energy, and use simple energy profile diagrams to illustrate energy changes.
• Demonstration of an exothermic and endothermic reaction
• Chemical reactions can result in a change in temperature. Exothermic and endothermic reactions (and changes of state).
• Transition metal elements: general chemical properties (colour, variable valency, use as catalysts).

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Copper Sulfate Crystals Recipe

• Ph.D., Biomedical Sciences, University of Tennessee at Knoxville
• B.A., Physics and Mathematics, Hastings College

Copper sulfate crystals are among the easiest and most beautiful crystals that you can grow . The brilliant blue crystals can be grown relatively quickly and can become quite large. 

Grow Copper Sulfate Crystals

• Copper sulfate crystals are vivid blue diamond-shaped crystals.
• Copper sulfate crystals are actually crystals of copper sulfate pentahydrate. The compound incorporates water into its structure.
• The crystals are easy to grow using an inexpensive, common chemical.

Copper Sulfate Crystal Materials

All you need for this project is copper sulfate, water, and a clear container. The chemical is sold as copper sulfate (CuSO4), although it readily picks up water and becomes copper sulfate pentahydrate (CuS0 4  . 5H 2 0). Buy it as a pure chemical or look for it as the only ingredient in root killer products at home supply stores.

• Copper sulfate

Make a Saturated Copper Sulfate Solution

Stir copper sulfate into very hot water until no more will dissolve. You can just pour the solution into a jar and wait a few days for crystals to grow, but if you grow a seed crystal , you can get much larger and better-shaped crystals.

Grow a Seed Crystal

Pour a little of the saturated copper sulfate solution into a saucer or shallow dish. Allow it to sit in an undisturbed location for several hours or overnight. Select the best crystal as your 'seed' for growing a large crystal. Scrape the crystal off of the container and tie it to a length of nylon fishing line.

Growing a Large Crystal

• Suspend the seed crystal in a clean jar that you have filled with the solution you made earlier. Don't allow any undissolved copper sulfate to spill into the jar. Don't let the seed crystal touch the sides or bottom of the jar.
• Place the jar in a location where it won't be disturbed. You can set a coffee filter or paper towel over the top of the container, but allow air circulation so that the liquid can evaporate .
• Check the growth of your crystal each day. If you see crystals starting to grow on the bottom, sides, or top of the container then remove the seed crystal and suspend it in a clean jar. Pour the solution into this jar. You don't want extra crystals growing because they will compete with your crystal and will slow its growth.
• When you are pleased with your crystal, you can remove it from the solution and allow it to dry.

For the best results, grow the crystal in a location with a stable temperature . Temperature fluctuations alternately dissolve the crystal (warm) and deposit crystal (cold). For example, a countertop is a better location than a sunny window sill.

Copper Sulfate Tips & Safety

• Copper sulfate is harmful if swallowed and can irritate skin and mucous membranes. In case of contact, rinse skin with water. If swallowed, give water and call a physician.
• If you choose to handle the crystals, wear gloves. The gloves protect your skin from irritation and also from intense blue staining.
• Even a small increase in the temperature of the water will greatly affect the amount of copper sulfate (CuS0 4  . 5H 2 0) that will dissolve.
• Copper sulfate pentahydrate crystals contain water, so if you want to store your finished crystal, keep it in a sealed container. Otherwise, water will evaporate from the crystals, leaving them dull and powdery from efflorescence . The gray or greenish powder is the anhydrous form of copper sulfate.
• Copper sulfate is used in copper plating, blood tests for anemia, in algicides and fungicides, in textile manufacturing, and as a desiccant .
• While municipal water utilities can deal with copper sulfate if you dump it down the drain, take care you don't toss it out into the environment. Copper sulfate is toxic to plants, invertebrates, and algae.
• Anthony, John W.; Bideaux, Richard A.; Bladh, Kenneth W.; Nichols, Monte C., eds. (2003). "Chalcocyanite". Handbook of Mineralogy. Vol. V. Borates, Carbonates, Sulfates . Chantilly, VA, US: Mineralogical Society of America. ISBN 978-0962209741.
• Clayton, G. D.; Clayton, F. E. (eds.) (1981). Patty's Industrial Hygiene and Toxicology (3rd ed.). Vol. 2, Part 6 Toxicology. NY: John Wiley and Sons. ISBN 0-471-01280-7.
• Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. ISBN 978-1439855119.
• Wiberg, Egon; Wiberg, Nils; Holleman, Arnold Frederick (2001). Inorganic Chemistry . Academic Press. ISBN 978-0-12-352651-9.
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• Chemistry Practicals
• CBSE Class 9 Chemistry Practical
• Experiment on the Reaction of Heating of Copper Sulphate Crystals and Classify it as Physical or Chemical Changes

Experiment on the reaction of Heating of copper sulphate crystals and classify it as physical or chemical changes

A physical change occurs when there is no change in the composition of a substance and no change in the chemical nature of the substance.

The interconversion of state occurs during physical change.

SOLID ⇄ LIQUID ⇄ GAS

A chemical change is a change that causes a change in the chemical properties of matter, resulting in the formation of a new substance. As an example, consider the burning of oil or fuel.

Heat is evolved or taken in, the formation of bubbles, gas, and fumes, as well as a change in the colour of the reactants, can take place when they form a product.

Reactants → Products

A + B → C (Chemical reaction)

Table of Contents

Materials required, observation, precautions.

• Frequently Asked Questions – FAQs

To carry out the reaction of Heating of copper sulphate crystals and classify it as physical or chemical changes.

Hydrated copper sulphate, Test Tube, Test Tube Holder, Bunsen Burner, pH paper or

Blue Litmus Paper.

CuSO 4 .5H 2 O is the chemical formula for copper sulphate crystals. It is known as copper sulphate pentahydrate. It has a water content of five moles per mole of copper sulphate. Copper sulphate pentahydrate has a blue colour due to water hydration. It loses water molecules and transforms into white anhydrous copper sulphate when heated.

• Heat copper sulphate crystals in a dry test tube.
• Observe the colour of the copper sulphate crystals after heating.
• Observe the water droplets along the sides of the boiling tube.
• Remove the test tube from the flame and allow it to cool for some time.
• Add 2 – 3 drops of water to the sample of heated copper sulphate.

• The colour of the copper sulphate crystals changes from blue to white on heating.
• Water droplets can be clearly observed on the walls of the boiling tube.
• White copper sulphate turns blue on adding 2 – 3 drops of water.

• Copper sulphate crystals contain water of crystallisation.
• Hydrated copper sulphate crystals lose their water of crystallisation on being heated and become anhydrous.
• Anhydrous copper sulphate changes to hydrated copper sulphate.
• It is a reversible chemical change.
• Copper sulphate is a highly toxic substance. It is not to be touched or tasted.
• Sulphuric acid is formed when sulphur trioxide reacts with atmospheric moisture. As a result, contact with sulphur trioxide should be avoided.
• Copper sulphate should be gently heated at the start of the experiment. However, after the formation of anhydrous copper sulphate, the test tube should be strongly heated.

Frequently Asked Questions

In the formula of copper sulphate crystals, what does 5h2o means.

In the formula of copper sulphate crystals, 5H2O means it contains five moles of water of crystallisation. It is because of water of crystallization that the colour of the copper sulphate pentahydrate is blue.

Is the reaction a chemical change or a physical change?

The reaction is a chemical change because new products are formed.

What type of reaction is it?

The reaction is reversible in nature.

What is the colour of copper sulphate crystals?

The colour of copper sulphate crystals is blue.

What is the formula of copper sulphate crystals?

The formula of copper sulphate crystals is CuSO 4 .5H 2 O.

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“Copper sulfate crystals” experiment

How to grow a beautiful blue crystal with a copper salt

We all like sto­ries about he­roes who go on end­less quests to find trea­sure. But some­times trea­sures can be found very near­by. In this ex­per­i­ment, we’ll show you how to grow a beau­ti­ful blue crys­tal, with­out trav­el­ing to the ends of the Earth.

Safe­ty pre­cau­tions

Wear pro­tec­tive gloves and glass­es.

Warn­ing! Only un­der adults su­per­vi­sion.

Reagents and equip­ment:

• cop­per(II) sul­fate pen­tahy­drate (70 g);
• hot wa­ter (100 ml);
• plas­tic twine;
• fun­nel with cot­ton wool;

Step-by-step in­struc­tions

Sprin­kle cop­per(II) sul­fate pen­tahy­drate into a beaker and pour hot wa­ter over it. Stir thor­ough­ly for 10-15 min­utes. In this way, we make a sat­u­rat­ed so­lu­tion. Re­move the re­main­ing crys­tals and dust from the so­lu­tion us­ing the fun­nel with cot­ton wool. Cov­er the so­lu­tion with foil and leave in a dark place for 24 hours.

Then pour the so­lu­tion into an­oth­er beaker and take out the crys­tals that have formed. It’s im­por­tant to choose a crys­tal with the right form, with­out cracks and oth­er de­fects. Tie twine around the crys­tal and im­merse it in the so­lu­tion we made pre­vi­ous­ly, so that the crys­tal does not touch the walls of the beaker. Cov­er with foil and put in a dark place. Af­ter a month a large crys­tal will grow on the twine!

Dozens of experiments you can do at home

One of the most exciting and ambitious home-chemistry educational projects The Royal Society of Chemistry