In this website you will find an overall description of calcium chloride, with many interesting facts, a procedure, observations and pictures of a reaction to create calcium chloride, and calculations of how much of each substance was used and produced.
Calcium Chloride
Calcium Chloride CaCl2 is an inorganic salt. This chemical exists in the form of a solid and liquid solution. Calcium Chloride appears as white, crystalline substance in the forms of flake, granule, or powder. When calcium chloride is in the form of a liquid it is a colorless solution. Calcium Chloride is used as a desiccant, deicing and freezing point depression, source of calcium ions, food, medicine, animal sterilizations and others.
Chemical properties of calcium chloride is that it’s exothermic in nature, or, during any chemical reaction heat is released. When calcium chloride is exposed to water a vast amount of heat is released. When the heat is released it can cause sputtering and boiling. The end product of a chemical reaction with water is calcium hydroxide and chlorine gas. When calcium chloride is merged with sulfuric acid, hydrochloric acid is formed, and it is highly abrasive in nature. Even though calcium chloride is a non-flammable substance, when it comes in contact with metals, such as zinc or sodium, hydrogen is produced, and hydrogen is highly flammable. (1)
One physical property of calcium chloride is that in a physical state it can be found as a solid at room temperature in flake, granule, and powder forms. Calcium Chloride is a salt. It’s added to many food products, mainly canned goods. Calcium Chloride, white in color, but in liquid form it is colorless. At a molten state, calcium chloride is a good conductor of electricity. But to contradict its thermal conductivity, it is a bad conductor of heat. Calcium Chloride has a boiling point as high as 1600o C. Calcium Chloride is soluble in both organic and inorganic solvents. It is hygroscopic in nature and absorbs moisture from air. If exposed to open air, it tends to become liquid. For that reason it is often called a deliquescent substance. It also has a low melting point, which means it can be dissolved at a very low temperature. (2)
Calcium + Chlorine → Calcium Chloride; in this reaction the metal atom gives electrons to the non-metal atom. The metal atoms become positive ions and the non-metal atoms become negative ions. This force of attraction between the two ions is called an ionic bond. (3)
Calcium Chloride is often used as a desiccant. This substance is often packed into drying tubes. Calcium Chloride also a source of calcium ions used to increase the water hardness in swimming pools. Calcium Chloride is sometimes used in brewing beer to correct mineral deficiencies in the brewing water. It affects flavor and chemical reactions during the brewing process, and can also affect yeast function during fermentation. Calcium chloride can be injected as intravenous therapy for the treatment of hypocalcaemia. It is also used in ceramic slipware. It suspends clay particles so that they float within the solution making it easier to use in a variety of slip casting techniques. (2)
When using calcium chloride safety measures should always be in effect. It can cause irritation to the skin, eyes, and respiratory tract and is harmful if swallowed or inhaled. If Calcium Chloride comes contact with skin, you should wipe off excess material from skin then immediately flush skin with plenty of water for at least 15 minutes. This chemical is not considered to be a fire hazard. Calcium Chloride should be stored in a tightly closed container, stored in a cool, dry, ventilated area. (6)
Original equation: Ca (OH) 2 + SrCl2 → CaCl2 + Sr (OH) 2
Balanced equation: Ca(OH)2 + SrCl2 → CaCl2 + Sr(OH)2
Materials Needed:
· Safety glasses
· Test Tubes
· Calcium Hydroxide
· Strontium Chloride
· Water
· Graduated cylinder
· Beaker
Step 1: Put safety glasses on
Step 2: Measure 5 grams of Calcium Carbonate. Then measure 5mL of Strontium Chloride. Afterwards measure out 50mL of water using the graduated cylinder. First add the Strontium Chloride to the water and stir and allow to dissolve. Then add Calcium Carbonate and wait.
Step 3: Make observations and see that a reaction occurred.
1. http://www.calciumchloride.co.uk/calcium_chloride_info.html
2. http://www.buzzle.com/articles/properties-of-calcium-chloride.html
3. http://www.chemguide.co.uk/atoms/bonding/ionic.html
4. http://www.chess.cornell.edu/safety/manual/msds/clcmchld.htm
5. FDA Compliance Articles. US Food and Drug Administration. March 1995.
6. Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002.
Calcium Chloride CaCl2 is an inorganic salt. This chemical exists in the form of a solid and liquid solution. Calcium Chloride appears as white, crystalline substance in the forms of flake, granule, or powder. When calcium chloride is in the form of a liquid it is a colorless solution. Calcium Chloride is used as a desiccant, deicing and freezing point depression, source of calcium ions, food, medicine, animal sterilizations and others.
Chemical properties of calcium chloride is that it’s exothermic in nature, or, during any chemical reaction heat is released. When calcium chloride is exposed to water a vast amount of heat is released. When the heat is released it can cause sputtering and boiling. The end product of a chemical reaction with water is calcium hydroxide and chlorine gas. When calcium chloride is merged with sulfuric acid, hydrochloric acid is formed, and it is highly abrasive in nature. Even though calcium chloride is a non-flammable substance, when it comes in contact with metals, such as zinc or sodium, hydrogen is produced, and hydrogen is highly flammable. (1)
One physical property of calcium chloride is that in a physical state it can be found as a solid at room temperature in flake, granule, and powder forms. Calcium Chloride is a salt. It’s added to many food products, mainly canned goods. Calcium Chloride, white in color, but in liquid form it is colorless. At a molten state, calcium chloride is a good conductor of electricity. But to contradict its thermal conductivity, it is a bad conductor of heat. Calcium Chloride has a boiling point as high as 1600o C. Calcium Chloride is soluble in both organic and inorganic solvents. It is hygroscopic in nature and absorbs moisture from air. If exposed to open air, it tends to become liquid. For that reason it is often called a deliquescent substance. It also has a low melting point, which means it can be dissolved at a very low temperature. (2)
Calcium + Chlorine → Calcium Chloride; in this reaction the metal atom gives electrons to the non-metal atom. The metal atoms become positive ions and the non-metal atoms become negative ions. This force of attraction between the two ions is called an ionic bond. (3)
Calcium Chloride is often used as a desiccant. This substance is often packed into drying tubes. Calcium Chloride also a source of calcium ions used to increase the water hardness in swimming pools. Calcium Chloride is sometimes used in brewing beer to correct mineral deficiencies in the brewing water. It affects flavor and chemical reactions during the brewing process, and can also affect yeast function during fermentation. Calcium chloride can be injected as intravenous therapy for the treatment of hypocalcaemia. It is also used in ceramic slipware. It suspends clay particles so that they float within the solution making it easier to use in a variety of slip casting techniques. (2)
When using calcium chloride safety measures should always be in effect. It can cause irritation to the skin, eyes, and respiratory tract and is harmful if swallowed or inhaled. If Calcium Chloride comes contact with skin, you should wipe off excess material from skin then immediately flush skin with plenty of water for at least 15 minutes. This chemical is not considered to be a fire hazard. Calcium Chloride should be stored in a tightly closed container, stored in a cool, dry, ventilated area. (6)
Original equation: Ca (OH) 2 + SrCl2 → CaCl2 + Sr (OH) 2
Balanced equation: Ca(OH)2 + SrCl2 → CaCl2 + Sr(OH)2
Materials Needed:
· Safety glasses
· Test Tubes
· Calcium Hydroxide
· Strontium Chloride
· Water
· Graduated cylinder
· Beaker
Step 1: Put safety glasses on
Step 2: Measure 5 grams of Calcium Carbonate. Then measure 5mL of Strontium Chloride. Afterwards measure out 50mL of water using the graduated cylinder. First add the Strontium Chloride to the water and stir and allow to dissolve. Then add Calcium Carbonate and wait.
Step 3: Make observations and see that a reaction occurred.
1. http://www.calciumchloride.co.uk/calcium_chloride_info.html
2. http://www.buzzle.com/articles/properties-of-calcium-chloride.html
3. http://www.chemguide.co.uk/atoms/bonding/ionic.html
4. http://www.chess.cornell.edu/safety/manual/msds/clcmchld.htm
5. FDA Compliance Articles. US Food and Drug Administration. March 1995.
6. Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002.
Sources of error that could occur are measuring wrong, not stirring long enough, not waiting long enough for reaction.
The final product turned out to be really cloudy and white.
The reaction that occurred is Ca(OH)2 + SrCl2 → CaCl2 + Sr(OH)2
The final product turned out to be really cloudy and white.
The reaction that occurred is Ca(OH)2 + SrCl2 → CaCl2 + Sr(OH)2
Weight in grams of each element: 3g SrCl2, 2.1g CaCl2
33.5g beaker with SrCl2 3g SrCl2 1 Mol. SrCl2 1 Mol. CaCl2 110.98g CaCl2 =
30.5g beaker 158.52g SrCl2 1 Mol SrCl2 1g CaCl2 = 2.1g CaCl2
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3g SrCl2
30.5g beaker 158.52g SrCl2 1 Mol SrCl2 1g CaCl2 = 2.1g CaCl2
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3g SrCl2