5-Ten Test Tube Mystery

Formation

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Procedure ,[object Object],[object Object],[object Object],[object Object],[object Object]

Experiment Tips ,[object Object],[object Object],[object Object],[object Object],[object Object]

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Worksheet ,[object Object],[object Object],[object Object],[object Object]

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Recommandé

16 solubility

14 standardization&titration

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Rates of reaction

Acid base

TOPIC 5. RATE OF REACTION-LAB

projecteciencies

Rate of reaction temperature

Rate of Reaction

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16 solubility

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To Determine the Enthalpy of H2O2 Decomposition in Aqueous Solution

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Tendances

To Determine the Enthalpy of H2O2 Decomposition in Aqueous Solution

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Siti Alias

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janlee97

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lanceqwerty

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Lab 9: Chemical Reactions II Pre-lab Questions 1. What is a limiting reagent? 2. A student used 7.15 g of CaCl2 and 9.25 g of K2CO3 to make CaCO3. The actual yield was 6.15 g of CaCO3. Calculate the limiting reagent and the percent yield. Experiment: Synthesis of Garden Lime 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 ...

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Tendances (20)

To Determine the Enthalpy of H2O2 Decomposition in Aqueous Solution

Factors affecting rate of reaction (recovered)

Elly lee effect of temperature on reaction rate

Final Report

Heat of Reaction

Absolute isotopic scale for deuterium analysis of natural waters

Determination equilibrium constant

Chemical reactions p pt

Investigate the effect of temperature on amylase activity

Ch5 z5e gases

Borax

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Effect of variation in temperature & pH levels on the activity of salivary am...

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smile790243

phychem1phychem2 Lab 9: Chemical Reactions II Pre-lab Questions 1. What is a limiting reagent? 2. A student used 7.15 g of CaCl2 and 9.25 g of K2CO3 to make CaCO3. The actual yield was 6.15 g of CaCO3. Calculate the limiting reagent and the percent yield. Experiment: Synthesis of Garden Lime 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 t.

phychem1phychem2Lab 9 Chemical Reactions IIPre-lab Qu.docx

mattjtoni51554

Chemical Reactions 2

projecteciencies

Micro chemlab

Loren Copernicus

Titration is a method of volumetric analysis—the use of volume measurements to analyze the concentration of an unknown. The most common types of titrations are acid–base titrations, in which a solution of an acid, for example, is analyzed by measuring the amount of a standard base solution required to neutralize a known amount of the acid. A similar principle applies to redox titrations. If a solution contains a substance that can be oxidized, then the concentration of that substance can be analyzed by titrating it with a standard solution of a strong oxidizing agent.

Micro chem

Loren Copernicus

E q u i l i b r i u m : D e t e r m i n a t i o n o f a n E q u i l i b r i u m C o n s t a n t P u r p o s e To determine the equilibrium constant of a reaction. L e a r n i n g O b j e c t i v e s Take a reaction to equilibrium by setting up and monitoring a reaction in a reflux apparatus. Measure the amount of acid at equilibrium by carrying out an acid-base titration. Apply the information from a balanced chemical equation and data obtained in the laboratory to determine the concentrations of reactants and products at equilibrium. Calculate the value of the equilibrium constant using data obtained in the laboratory. L a b o r a t o r y S k i l l s To set up and monitor a reflux apparatus. To carry out an acid-base titration. E q u i p m e n t Two 50-mL graduated cylinders Two 125-mL Erlenmeyer flasks 1-mL pipet 25-mL buret Equipment necessary to assemble the reflux apparatus shown in Figure 1. C h e m i c a l s Anhydrous ethanol (ethyl alcohol) Anhydrous acetic acid Concentrated sulfuric acid I n t r o d u c t i o n From the beginning of this course, we have generally assumed that chemical reactions go to completion, that is, the reaction proceeds in the forward direction until one of the reactants is completely used up. However, many reactions do not go to completion and are able to move both in the forward and reverse directions simultaneously. Such a reaction is called a reversible reaction. A double arrow in the chemical equation designates a reversible reaction, as shown in Reaction 1: aA + bB −−−⇀↽−−− cC + dD (Reaction 1) 1 D e t e r m i n a t i o n o f a n E q u i l i b r i u m C o n s t a n t A reversible reaction has two reaction rates: a forward reaction rate, where the reactants A and B are consumed andtheproductsCandDareproduced,andareversereactionrate,wheretheproductsCandDareconsumedand thereactantsAandBareproduced. Allreversiblereactionseventuallyreachapointatwhichtheforwardreaction rate equals the reverse reaction rate. This point is called equilibrium. At equilibrium, the concentration of reactants and products do not change with time. It is important to remember that even though the concentration of reactants and products do not change with time, the reaction has not stopped. Equilibrium is a dynamic state. The state will persist as long as the reaction conditions remain constant. A reaction at equilibrium follows the law of mass action which gives the relationship between concentrations of the reactants and products at equilibrium. According to the law of mass action, the relationship between concentrations of reactants and products at equilibrium for the above reaction is given in Equation 1: 𝐾eq = [C]𝑐[D]𝑑 [A]𝑎[B]𝑏 (Equation 1) Thisrelationshipiscalledtheequilibrium-constantexpression. Theconstant, 𝐾eq, isapositivenumberwhose value depends on the reaction and temperature. In today’s experiment, students will be determining the equilibrium constant for the reac

E q u i l i b r i u m D e t e r m i n a t i o n o f a n E

AlyciaGold776

Water Testing Lab Background Information: Chemists can detect and identify ions in water solution in several different ways. In this lab you will use some chemical tests to check for the presence of certain ions in aqueous solution. Positively charged ions are called cations; negatively charged ions are called anions. The tests you will perform are confirming tests. If the test is positive, it confirms that the ion in question is present. In each confirming test you will look for a change in solution color, or the appearance of an insoluble material called a precipitate. A negative test (no color change or precipitate) doesn’t necessarily mean the ion in question is not present. The ion may simply be present in such a small amount that the color or precipitate cannot be seen. Purpose: § To use chemical tests to determine the presence of ions in three different water samples. Objectives: § To test for the presence of cations iron (III) Fe3+, calcium Ca2+, copper Cu+, as well as the anions chloride Cl-, phosphate PO43-, and sulfate SO42-. § To perform each of the following confirming tests on three different samples: 1. A reference solution (known to contain the ion of interest) 2. Tap water (which may or may not contain the ion) 3. A control (distilled water, known not to contain the ion) § Test for water hardness using ion-testing strips. § Complete a confirmative ion-testing using a complete ion-testing strip. Materials: § 10 test tubes § Test tube rack § 10 mL graduated cylinder § Test reagent solutions in dropper bottles o Potassium thiocyanate (KSCN) o Potassium oxalate (K2C2O4) o Acetic acid (HC2H3O2) o Silver nitrate (AgNO3) o Barium Chloride (BaCl2) § Reference ion solutions o Iron (III) Nitrate - Fe(NO3)3 o Calcium Chloride – CaCl2 o Iron (II) Sulfate – FeSO4 Procedures: PART ONE 1. Safety goggles should be worn at ALL times during this lab exercise. If you spill any of the reagents on your hands, wash them immediately. 2. Clean five test tubes with water and dry all glassware before starting the experiment. 3. In this lab, you are testing water samples for the presence of four different ions: Ca2+, Fe3+, Cl-, and SO42-. For EACH of the test procedures you will test a reference solution (known to contain the ion), a control (distilled water-known not to contain the ion), and your water samples brought from home. Follow the diagram below and be sure to keep track of your water samples: 4. Measure 1 pipette full (about 2 mL) of reference solution, control, and the three water samples into five clean test tubes. Label the three test tubes Reference (R), Control (C), and Water Sample #1, 2, & 3. 5. Follow the table below to test for each ion: 6. As you perform each test, record your observations in the data table below. 7. When you have completed an ion test, wash your test tubes with water and dry them thoroughly before moving on to the next ion test. P.

Water Testing Lab Background Information Chemists can .docx

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Acid/Base Chemistry Portland Community College Staff* Version 42-0137-00-01 Lab Report Assistant This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ writing of lab reports by providing this information in an editable file which can be sent to an instructor. Observations In columns 3 and 4, record the color and intensity seen. In columns 5 and 6, determine if the substance is an acid or a base, and if the substance is ionic. For the last column, determine which chemical species is acting as an acid or base. Data Table 1: Acids and Bases Acting in Water Well Substance 1drop BTB Plus 1 drop of substance Acid or base (Q1) Ionic? Y/N (Q2) Species acting as acid or base (Q3) 1 NaHCO3 2 CH3COOH 3 HCL 4 Na2CO3 5 H2SO4 6 CH3COONa 7 NaOH 8 HNO3 9 NaHSO4 10 NH3 11 H3PO4 12 NaH2PO4 13 Na2HPO4 14 Na3PO4 15 NaHSO3 Data Table 2: Following Acid/Base neutralization reactions Well # 1 Drop of Each Observation +2 Drops Acid Observation +2 Drops Base Observation 1 BPB + NaOH HCl NaOH 2 BPB + NaOH H2SO4 NaOH 3 BPB + NaOH CH3COOH NaOH 4 BPB + NaOH H3PO4 NaOH 5 BPB + Ca(OH)2 HCl Ca(OH)2 6 BPB + Ca(OH)2 H2SO4 Ca(OH)2 7 BPB + Ca(OH)2 CH3COOH Ca(OH)2 8 BPB + Ca(OH)2 H3PO4 Ca(OH)2 9 BPB + NH3 HCl NH3 10 BPB + NH3 H2SO4 NH3 11 BPB + NH3 CH3COOH NH3 12 BPB + NH3 H3PO4 NH3 Please note here if any of the other starting materials is other than a clear, colorless solution. Data Table 3: Investigating Odor as a Means of Indicating Neutralization. Substance(s) Odor 2 Drops of HCl in Well #1 1 Drop of Ammonia on Swab Swab with Ammonia & HCl Data Table 4: Investigating Evaporation as a Means of Indicating a Neutralization Reaction. Reaction Mixture Observation (When Wet) Observation (When Dry) HCl + NaOH CH3COOH + NH3 HNO3 + NaOH PART 5: Mini-Experiments 1. Use BTB to classify four household products as acidic or basic. Possible substances to test include home cleaning products, glass cleaner, liquid detergent, bleach, soft drinks, liquid from food items, etc. Remember to: a. Hypothesis (What you think will happen and why) or purpose: b. Method used to test your hypothesis: c. Data and Observations Put your data and observations in the space below. You can include pictures that you “draw.” d. Conclusions 2. Find one common, highly colored substance that can be used as an acid-base indicator. Possible substances include fruit/vegetable juice or products, inks, food coloring, flower petals, etc. If using fresh fruit, veggies, or flo.

AcidBase ChemistryPortland Community College StaffVersio.docx

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Jean-Claude Bradley presents at the American Chemical Society meeting on August 20, 2012. Examples are first presented to demonstrate how access to Open Notebooks can provide critical information not usually shared in the traditional publication process. The use of Google App Scripts to look up chemical properties allows for the use of Google Spreadsheets as a self-contained dashboard to plan and analyze chemical reactions. The concept of the Open Chemical Property Matrix (OCPM) is introduced and a smartphone app to suggest recrystallization solvents is then presented.

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