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Experimental Lab on Chemical Reactions resulting in Precipitates, Lab Reports of Chemistry

Arizona State University (ASU) - TempeChemistry

An experiment involving the combination of given reagents to form four different precipitates. The lab includes procedures for each reaction, observations, and results in the form of molecular, ionic, and net ionic equations. The experiment aims to produce useful solids for the chemical waste disposal company, with three out of the four chemical reactions resulting in a precipitate.

Typology: Lab Reports

Pre 2010

Uploaded on 09/02/2009

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Introduction
The main objective of this lab was to take the given reagents and combine them to
form four different precipitates. A precipitate, by definition is “an insoluble solid formed
by a reaction in solution.”1 The first chemical reaction, Sulfuric Acid (H2SO4) and
Sodium Carbonate (Na2CO3), will not produce a precipitate. Both the Sulfuric Acid and
the Sodium Carbonate do not form a precipitate, due to both compounds being soluble.
The solubility of a substance is by definition “the amount of that substance that can be
dissolved in a given quantity of solvent”2. However, the remaining three reactions, Silver
Nitrate (AgNO3) & Barium Chloride (BaCl2), Manganese (II) Nitrate (Mn(NO3)2) &
Sodium Hydroxide (NaOH), and Zinc (II) Nitrate (Zn(NO3)2) & Sodium Hydroxide, will
result in precipitates. To fulfill the goals of the lab, three out of the four chemical
reactions must result in a precipitate. The standard equation for this lab was a double
displacement reaction Ax+By Ay+Bx.
Experimentation
The first experiment was set up with a two test tubes. The first procedure was to
pour 1 mL of Sulfuric Acid into a test tube. The next step was to pour 1 mL of Sodium
Carbonate into a different test tube. Then pour the two in one test tube to observe the
reaction and record the results. Since the solution didn’t produce a precipitate a Bunsen
burner was used to burn out the water which was still contained inside the test tube.
The second procedure was to pour 1 mL of Silver Nitrate into a test tube. The
next step was to pour 1 mL of Barium Chloride into a different test tube. Then pour the
two in one test tube to observe the reaction and record the results. A centrifuge was used;
1 Brown, Theodore L, Lemay, H. Eugene, Jr., Bursten, Bruce E., Burdge, Julia R. Chemistry The Central
Science. New Jersey: Prentice Hall, 2003.
2 Chemistry the Central Science.
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Introduction The main objective of this lab was to take the given reagents and combine them to form four different precipitates. A precipitate, by definition is “an insoluble solid formed by a reaction in solution.”^1 The first chemical reaction, Sulfuric Acid (H 2 SO 4 ) and Sodium Carbonate (Na 2 CO 3 ), will not produce a precipitate. Both the Sulfuric Acid and the Sodium Carbonate do not form a precipitate, due to both compounds being soluble. The solubility of a substance is by definition “the amount of that substance that can be dissolved in a given quantity of solvent”^2. However, the remaining three reactions, Silver Nitrate (AgNO 3 ) & Barium Chloride (BaCl 2 ), Manganese (II) Nitrate (Mn(NO 3 ) 2 ) & Sodium Hydroxide (NaOH), and Zinc (II) Nitrate (Zn(NO 3 ) 2 ) & Sodium Hydroxide, will result in precipitates. To fulfill the goals of the lab, three out of the four chemical reactions must result in a precipitate. The standard equation for this lab was a double displacement reaction Ax+By  Ay+Bx. Experimentation The first experiment was set up with a two test tubes. The first procedure was to pour 1 mL of Sulfuric Acid into a test tube. The next step was to pour 1 mL of Sodium Carbonate into a different test tube. Then pour the two in one test tube to observe the reaction and record the results. Since the solution didn’t produce a precipitate a Bunsen burner was used to burn out the water which was still contained inside the test tube. The second procedure was to pour 1 mL of Silver Nitrate into a test tube. The next step was to pour 1 mL of Barium Chloride into a different test tube. Then pour the two in one test tube to observe the reaction and record the results. A centrifuge was used; (^1) Brown, Theodore L, Lemay, H. Eugene, Jr., Bursten, Bruce E., Burdge, Julia R. Chemistry The Central Science. New Jersey: Prentice Hall, 2003. (^2) Chemistry the Central Science.

one test tube of water was placed on one side, and the solution on the other. The centrifuge ran for eight minutes, then the test tubes were removed and the liquid was poured out (decanting). Deionized water was poured in; the centrifuge was turned on again to clean the solution out of the solid. This procedure was repeated two more times. The third procedure was to pour 1 mL of Manganese (II) Nitrate into a test tube. The next step was to pour 1 mL of Sodium Hydroxide into a different test tube. Then pour the two in one test tube to observe the reaction and record the results. A centrifuge was used; one test tube of water was placed on one side, and the solution on the other. The centrifuge ran for eight minutes, then the test tubes were removed and the liquid was poured out (decanting). Deionized water was poured in; the centrifuge was turned on again to clean the solution out of the solid. This procedure was repeated two more times. The fourth procedure was to pour 1 mL of Zinc (II) Nitrate into a test tube. The next step was to pour 1 mL of Sodium Hydroxide into a different test tube. Then pour the two in one test tube to observe the reaction and record the results. A centrifuge was used; one test tube of water was placed on one side, and the solution on the other. The centrifuge ran for eight minutes, then the test tubes were removed and the liquid was poured out (decanting). Deionized water was poured in; the centrifuge was turned on again to clean the solution out of the solid. This procedure was repeated two more times. Results Equations: Molecular Equation 1 H 2 SO4(aq) + Na 2 CO3(aq)  H 2 CO3(aq) + Na 2 SO4(aq) Ionic Equation 1 H 2 +(aq) + SO 4 2-(aq) + Na 2 +(aq) + CO 3 2-(aq)  H 2 +(aq) + CO 3 2-(aq) + Na 2 +(aq) + SO 4 2-(aq)

Table 2 Chemical Reaction Products Solution Combinations Solid Formed H 2 SO 4 & Na 2 CO 3 No solid was formed AgNO 3 & BaCl 2 AgCl Mn(NO 3 ) 2 & NaOH Mn(OH) 2 Zn(NO 3 ) 2 & NaOH Zn(OH) 2 The only chemical reaction that did not produce a precipitate was that of the Sulfuric Acid and Sodium Carbonate combination. The other three combinations, Silver Nitrate and Barium Chloride, Manganese (II) Nitrate and Sodium Hydroxide, and Zinc (II) Nitrate and Sodium Hydroxide did form a precipitate. The Silver Nitrate and Barium Chloride formed a white solid powder-like substance that settled at the bottom of the test tube. This powder-like substance is Silver (I) Chloride (AgCl). The Manganese (II) Nitrate and Sodium Hydroxide, combination turned the solution an apple-juice color. This same combination also produced a light white gel-like substance that floated in the solution. This light white gel-like substance is Manganese (II) Hydroxide (Mn(OH) 2 ). The last solution that created a precipitated was the Zinc (II) Nitrate and Sodium Hydroxide combination. This combination’s solution did not change color, it remained clear, however this solution did produce a light white gel-like substance that remained suspended in the clear solution. This gel-like substance is Zinc (II) Hydroxide (Zn(OH) 2 ). Discussion The Sulfuric Acid and Sodium Carbonate combination did not form a precipitate due to the two new compounds formed being soluble. The two compounds that were formed were Carbonic Acid (H 2 CO 3 ) and Sodium Sulfate (Na 2 SO 4 ). The Carbonic Acid

contains carbonate (CO 3 2-) which is usually insoluble, except when it is in a compound that contains an alkali metal cation. Carbonic Acid also contains hydrogen which is an alkali metal cation, making the compound soluble.^3 Sulfuric Acid is also soluble, thus it also broke down. The final solution contained all of the following ions: H 2 +, CO 3 2-, Na 2 +, SO 4 2-. These ions did not come together to form a compound that would result in a precipitate. These ions did not form a precipitate due to all of the listed ions being soluble. By definition ions must be insoluble in order for them to form a precipitate. The next combination, Silver Nitrate and Barium Chloride, formed two compounds, Silver Chloride and Barium Nitrate (Ba(NO 3 ) 2 ). Silver Chloride is insoluble, however Barium Nitrate is soluble. The Silver Chloride is insoluble due to it containing silver, which is insoluble. Since Silver Chloride is insoluble it formed a precipitate. Since barium nitrate is soluble, it broke down into Ba2+^ and (NO 3 ) 2 -. The Manganese (II) Nitrate and the Sodium Hydroxide formed two compounds, Manganese (II) Hydroxide and Sodium Nitrate. The Manganese (II) Hydroxide proved to be insoluble due to it containing hydroxide (OH-). The hydroxide is insoluble, therefore making the compound form a precipitate. The Sodium Nitrate is soluble; therefore it broke down into Na+^ and NO 3 -^ ions. The Zinc (II) Nitrate and the Sodium Hydroxide chemical reaction was the last to form a precipitate. The two solutions formed two compounds, Zinc (II) Hydroxide and Sodium Nitrate. The Zinc (II) Hydroxide proved to be insoluble due to it containing hydroxide. The hydroxide is insoluble, therefore making the compound form a precipitate. The Sodium Nitrate is soluble; therefore it broke down into Na+^ and NO 3 - ions. (^3) Chemistry the Central Science.