Abstract
Zinc Chloride is synthesized from a single replacement reaction of hydrogen chloride mixed with granular zinc. The beginning features a hefty chemical analysis including uses and hazards. There is a specified procedure, materials list, calculations and data table as well as a citation for all information.
Introduction
Zinc chloride otherwise known as (ZnCl2) is a colorless or white compound of zinc and chlorine (1). Zinc chloride can be derived from a zinc hydrogen chloride reaction. (4). Zinc is a transition metal and has an oxidation number of +2, and chloride is a halogen with an oxidation number of +1(1). The compound has an overall oxidation number of two (1). They combine to create and ionic bond. Ionic compounds usually have a high melting point because they have such strong bonds (in comparison to molecular bonds) (1). But zinc chloride has an unusually low melting point of 275° Celsius or 527°Farnheit(2) and a boiling point of 756 °C or 1393 °F (2). It can even weigh up to 136.29 g/mol (1).
There are nine different reported structures with one being a liquid (1). Four structures are composed of crystals (4). Five are composed of hydrates (4). Hydrates are water infused crystals (4). Due to their high affinity for water, zinc chloride should be kept in water tight containers. Otherwise, one could end up with a lovely zinc chloride brick (1). It should also have all water, (including evaporated) removed from the surrounding air (1). Zinc chloride is aqueous meaning soluble in water. (2). It is soluble in acetone, ethanol, and diethyl ether (5). Once dissolved in water, it has a ph. of four (3).
Zinc chloride has a linear shape in its gas phase. There are no lone pairs on zinc, and a single bond to each chlorine atom (3). The most interesting property of zinc chloride is that it can dissolve starches, silk, and cellulose (1). The compound is odorless, and a great conductor of electricity(1). It can dissolve cellulose, silk, and cornstarch (3). Other names for zinc chloride include zinc dichloride, and butter of zinc (4). It’s called butter of zinc based on its oily texture (3).
This compound has many uses due to its ability to corrode and dissolve. It is used to break down metal oxides, a process known as soldering (1). It can also fireproof and etch metals and stones. It also plays a key role in the production of dry cell batteries (4). Zinc chloride can be a great emulsifiers, breaking apart oil from water (4). The liquid form of it is used in paper and cement productions (4). It can preserve wood, protecting it from mold and rain (4). Lastly it’s a packer fluid for gas and oil (4).
Zinc chloride can be lethal. It’s a skin irritant, and can cause dermatitis if given direct contact (6). Secondhand contamination can be a serious problem in the lab area as well (6). If it gets on someone’s hands, it will get stuck in the cracks of their palms and their fingertips. Even if they wash their hands multiple times, it will remain (1). Eventually their hands would dry out and [painfully] crack (2). Then they can transmit it on to door knobs, beakers, and goggles. It could later be digested, after handling food, causing intestinal damage. Inhalation can lead to respiratory problems, most likely asthma (1). Eye contact can lead to destroyed corneas, and blindness (6). Severe overexposure can lead to death, from dissolving the cells of easy to reach orifices (eyes, mouth, lungs) (6). When handling this compound, one should always wear goggles, and gloves, as well as keeping nose, and mouth away from it (6).
Works Cited
(3) Mills, John S., and Raymond White. The Organic Chemistry of Museum Objects. Oxford [England: Butterworth-Heinemann, 1994. Academic OneFile. Web. 17 Feb. 2013.
(5) Nnama, Helen. "The Safety of Zinc Chloride?" Livestrong.com. LiveStrong Foundation, 17 Jan. 2011. Web. 01 Mar. 2013.
(4) Vogel, Arthur Israel., B. S. Furniss, and Arthur Israel. Vogel. Vogel's Textbook of Practical Organic Chemistry. London: Longman Scientific & Technical, 1989. Web. 17 Feb. 2013.
(2) Wells, A. F. Models in Structural Inorganic Chemistry. New York: Oxford UP, 1970. Gale Virtual Reference Library. Web. 17 Feb. 2013.
(1)"Zinc Chloride." Chemistry Daily. N.p., 4 Jan. 2007. Web. 17 Feb. 2013.
(6) "Zinc Chloride MSDS." Sciencelab.com. Science Lab, 9 June 2012. Web. 17 Feb. 2013
Materials:
· 2 50mL beakers
· 500 grams of granular zinc
· 1 mole of HCl
· 1 plastic spoon
· 1 triple beam balance
Chemical Equation: Zn (s.) + 2HCl (aq.) ZnCl2 (aq.) + H2 (g.)
Procedure
Put 50mL beaker on triple beam balance. Measure mass of 50mL beaker. Measure 10.5 grams of zinc by placing it inside of the 50mL beaker with the plastic spoon. Remove 50mL beaker from triple beam balance. In a separate beaker pour in 18 mL of HCl. Pour beaker of HCl into beaker of zinc. Record observations. After reaction has cooled, dispose of products accordingly.
Data Table
Zinc Chloride is synthesized from a single replacement reaction of hydrogen chloride mixed with granular zinc. The beginning features a hefty chemical analysis including uses and hazards. There is a specified procedure, materials list, calculations and data table as well as a citation for all information.
Introduction
Zinc chloride otherwise known as (ZnCl2) is a colorless or white compound of zinc and chlorine (1). Zinc chloride can be derived from a zinc hydrogen chloride reaction. (4). Zinc is a transition metal and has an oxidation number of +2, and chloride is a halogen with an oxidation number of +1(1). The compound has an overall oxidation number of two (1). They combine to create and ionic bond. Ionic compounds usually have a high melting point because they have such strong bonds (in comparison to molecular bonds) (1). But zinc chloride has an unusually low melting point of 275° Celsius or 527°Farnheit(2) and a boiling point of 756 °C or 1393 °F (2). It can even weigh up to 136.29 g/mol (1).
There are nine different reported structures with one being a liquid (1). Four structures are composed of crystals (4). Five are composed of hydrates (4). Hydrates are water infused crystals (4). Due to their high affinity for water, zinc chloride should be kept in water tight containers. Otherwise, one could end up with a lovely zinc chloride brick (1). It should also have all water, (including evaporated) removed from the surrounding air (1). Zinc chloride is aqueous meaning soluble in water. (2). It is soluble in acetone, ethanol, and diethyl ether (5). Once dissolved in water, it has a ph. of four (3).
Zinc chloride has a linear shape in its gas phase. There are no lone pairs on zinc, and a single bond to each chlorine atom (3). The most interesting property of zinc chloride is that it can dissolve starches, silk, and cellulose (1). The compound is odorless, and a great conductor of electricity(1). It can dissolve cellulose, silk, and cornstarch (3). Other names for zinc chloride include zinc dichloride, and butter of zinc (4). It’s called butter of zinc based on its oily texture (3).
This compound has many uses due to its ability to corrode and dissolve. It is used to break down metal oxides, a process known as soldering (1). It can also fireproof and etch metals and stones. It also plays a key role in the production of dry cell batteries (4). Zinc chloride can be a great emulsifiers, breaking apart oil from water (4). The liquid form of it is used in paper and cement productions (4). It can preserve wood, protecting it from mold and rain (4). Lastly it’s a packer fluid for gas and oil (4).
Zinc chloride can be lethal. It’s a skin irritant, and can cause dermatitis if given direct contact (6). Secondhand contamination can be a serious problem in the lab area as well (6). If it gets on someone’s hands, it will get stuck in the cracks of their palms and their fingertips. Even if they wash their hands multiple times, it will remain (1). Eventually their hands would dry out and [painfully] crack (2). Then they can transmit it on to door knobs, beakers, and goggles. It could later be digested, after handling food, causing intestinal damage. Inhalation can lead to respiratory problems, most likely asthma (1). Eye contact can lead to destroyed corneas, and blindness (6). Severe overexposure can lead to death, from dissolving the cells of easy to reach orifices (eyes, mouth, lungs) (6). When handling this compound, one should always wear goggles, and gloves, as well as keeping nose, and mouth away from it (6).
Works Cited
(3) Mills, John S., and Raymond White. The Organic Chemistry of Museum Objects. Oxford [England: Butterworth-Heinemann, 1994. Academic OneFile. Web. 17 Feb. 2013.
(5) Nnama, Helen. "The Safety of Zinc Chloride?" Livestrong.com. LiveStrong Foundation, 17 Jan. 2011. Web. 01 Mar. 2013.
(4) Vogel, Arthur Israel., B. S. Furniss, and Arthur Israel. Vogel. Vogel's Textbook of Practical Organic Chemistry. London: Longman Scientific & Technical, 1989. Web. 17 Feb. 2013.
(2) Wells, A. F. Models in Structural Inorganic Chemistry. New York: Oxford UP, 1970. Gale Virtual Reference Library. Web. 17 Feb. 2013.
(1)"Zinc Chloride." Chemistry Daily. N.p., 4 Jan. 2007. Web. 17 Feb. 2013.
(6) "Zinc Chloride MSDS." Sciencelab.com. Science Lab, 9 June 2012. Web. 17 Feb. 2013
Materials:
· 2 50mL beakers
· 500 grams of granular zinc
· 1 mole of HCl
· 1 plastic spoon
· 1 triple beam balance
Chemical Equation: Zn (s.) + 2HCl (aq.) ZnCl2 (aq.) + H2 (g.)
Procedure
Put 50mL beaker on triple beam balance. Measure mass of 50mL beaker. Measure 10.5 grams of zinc by placing it inside of the 50mL beaker with the plastic spoon. Remove 50mL beaker from triple beam balance. In a separate beaker pour in 18 mL of HCl. Pour beaker of HCl into beaker of zinc. Record observations. After reaction has cooled, dispose of products accordingly.
Data Table
Mass of beaker
Mass of beaker and zinc Volume of HCl |
18.9 grams
30,4 grams 18 milliliters |
Calculations
a) To obtain mass of zinc
Mass of beaker and zinc - mass of beaker = mass of zinc
30.4g. -18.9g. = 10.5g.
b) Estimated mass of zinc chloride
a) To obtain mass of zinc
Mass of beaker and zinc - mass of beaker = mass of zinc
30.4g. -18.9g. = 10.5g.
b) Estimated mass of zinc chloride
10.5 g Zn
|
1 mole Zn
65.3 g Zn |
1 mole ZnCl
1 mole Zn |
100.8 g ZnCl
1 mole ZnCl |
= 16.2 g of Zinc Chloride
Observations
There was a single significant reaction of hydrogen chloride mixing with zinc. Tiny gas bubbles were emitted, and projected upwards.
Conclusion
Hydrogen gas was emitted in tiny gas bubbles during the reaction, proving that the reaction did occur. There were a few sources of error. Due to class time/other experimenters waiting, the experimenter didn’t get to watch the full reaction. She was also hurried in measuring, causing her measurement of the mass of zinc to be less than accurate. The time table of experiment was undeterminable, due to lack of information on the concentration of the hydrogen chloride. The beakers may have not been the clean, because of residue from previous experiments.
Observations
There was a single significant reaction of hydrogen chloride mixing with zinc. Tiny gas bubbles were emitted, and projected upwards.
Conclusion
Hydrogen gas was emitted in tiny gas bubbles during the reaction, proving that the reaction did occur. There were a few sources of error. Due to class time/other experimenters waiting, the experimenter didn’t get to watch the full reaction. She was also hurried in measuring, causing her measurement of the mass of zinc to be less than accurate. The time table of experiment was undeterminable, due to lack of information on the concentration of the hydrogen chloride. The beakers may have not been the clean, because of residue from previous experiments.