Precipitation react 1
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This document describes a lab experiment on precipitation reactions. Students will observe precipitation reactions by mixing aqueous solutions of cations and anions in test tubes. They will identify which two cations form the most precipitates. The materials needed are listed. The procedure involves placing solutions in test tubes and observing any color changes or precipitate formation. Examples of double displacement reactions that form precipitates are provided, such as the reaction of Pb(NO3)2 and NaCl forming an insoluble PbCl2 precipitate. Safety precautions are emphasized.
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This document discusses different types of chemical reactions including decomposition, synthesis, combustion, double replacement, and single replacement reactions. It provides examples of each type of reaction and explains the key features that define them. Double replacement reactions are highlighted, where a metal replaces a metal in a compound and a nonmetal replaces a nonmetal, forming a precipitate if one of the products is insoluble. Guidelines are provided for writing molecular, total ionic, and net ionic equations for double replacement reactions.
Precipitation react2
This document summarizes an experiment on double displacement precipitation reactions. Various metal nitrates and chlorides were reacted and precipitates were observed and recorded. Silver nitrate produced precipitates with potassium iodide (silver iodide, yellow), sodium chloride (silver chloride, white), sodium hydroxide (silver hydroxide, brown), iron(III) chloride (silver chloride, light yellow), sodium carbonate (silver carbonate, light green), and copper(II) sulfate (silver sulfate, very light blue). Lead(II) nitrate also produced precipitates with the same reactants. The conclusion is that silver and lead ions form the most precipitates in these double displacement reactions.
QUALITATIVE ANALYSIS (CONFIRMATORY TEST FOR CATIONS)
CHAPTER 6 ACID, BASE AND SALT
6.11 Qualitative Analysis for Salts
Confirmatory test for cations (Ammonium ion, NH4+; iron(II) ion, Fe2+, iron(III) ion, Fe3+ and lead(II) ion, Pb2+) using
1. Nessler's Reagent (for ammonium ion, NH4+)
2. Potassium hexacyanoferrate(III) and potassium thiocyanate (for iron(II) ion, Fe2+ and iron(III) ion, Fe3+)
3. Potassium iodide (for lead(II) ion, Pb2+)
Lab 9 Chemical Reactions IIPre-lab Questions1. What is a limi.docx
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 ...
ABSTRACT WEIGHT Contains an INTRODUCTORY statement (2-3 Sent.docx
ABSTRACT WEIGHT
Contains an INTRODUCTORY statement (2-3 Sentences) A B C D F /2
States the purpose of the experiment accurately
Clearly links chemical relationships to observing chemical change
Defines single and double displacement reactions,
explains evidence of chemical change, and use of stoichiometry
A B C D F /3
A B C D F /2
A B C D F /3
Explains how results were evaluated (compare observations with
solubility tables, knowledge of gas forming rxns, qualitative analysis)
A B C D F /2
/20
REACTION SHEET WEIGHT
Accurately describes fundamental steps or lessons learned that are
essential to conducting the experiment (equipment used, major
procedural steps, big picture reasons for doing what you did, any
important information you learned from conducting the experiment )
* Excludes non-essential details that can be assumed to be known
A B C D F /10
A B C D F /10
Comments:
/20
Name:______________________ WINTER 2017
Lab Abstract Rubric – CH 204
Experiment #6 – OBSERVING AND WRITING CHEMICAL REACTIONS Total Points to Date and %:_____ /2
Contains a description of the METHODS used (2-3 Sentences)
Accurately explains significance of observations and/or results of
the experiment, interprets all important tends and data
comparisons, connects experimental work to theories and/or
principles that explain the work. Relate back to the introductory
statement and your specific results/observations.
A B C D F /2Contains a CONCLUDING statement (3-5 Sentences)
Contains a description of the most interesting RESULTS/
OBSERVATIONS (3-4 Sentences)
/3A B C D F
A B C D F /3
Comments:
Contains each (8-10) balanced reactions with correct physical states,
proper chemical formulas, and accurate stoichiometry:
NaCl (aq) + AgNO3 (aq) → AgCl (s) + NaNO3 (aq)
Contains, in sentence form, the description of the reaction:
Aqueous sodium chloride reacted with aqueous silver nitrate to
form solid silver chloride and aqueous sodium nitrate.
LABORATORY NOTEBOOK WEIGHT
Includes carbon copy of completed & on-time pre-lab A B C D F /2
Includes a complete record of properly constructed lab notes
which include the date, data, calculations, notes to self, ect. A B C D F /3
Demonstrates legible and comprehensible organization of
observations and data
A B C D F /3
Comments:
/8
Abdullah Alfifi
CH 204
7/11/2016
Experiment 6: Observing Chemical Reactions/Writing Chemical Equations
Introduction
Chemical reactions occur when atoms of same or different elements exchange electrons to form new products. The exchange of electrons or atoms is usually invisible and can be seen in form or chemical changes. The changes represents evidence of a chemical reaction. Such cha.
phychem1phychem2Lab 9 Chemical Reactions IIPre-lab Qu.docx
This document provides the procedure for a chemistry lab experiment involving chemical reactions. The experiment involves synthesizing calcium carbonate and determining the limiting reagent and percent yield. Students will carry out two trials of the reaction of calcium chloride and potassium carbonate solutions to produce calcium carbonate precipitate. They will calculate the theoretical and actual yields, identify the limiting reagent, and calculate the percent yield for each trial. The procedure provides detailed steps for setting up the reaction, filtering and drying the product, collecting data, and performing calculations to analyze the results.
Science 10th Class
This document provides information on stoichiometry, which involves using mole ratios from balanced chemical equations to calculate mass relationships between substances in a chemical reaction. It outlines the steps to solve stoichiometry problems, which include writing a balanced equation, identifying known and unknown quantities, setting up mole ratio conversion factors between moles of reactants and products, and checking the answer. Key concepts discussed include the mole ratio from coefficients in a balanced equation, molar mass to convert between moles and grams, and the molar volume used to calculate liters of gas at standard temperature and pressure.
Types of Reactions PPT.pdf_١١٢٢٠٠٠٤.pptx
There are five main types of chemical reactions: synthesis, decomposition, single replacement, double replacement, and combustion. A chemical reaction occurs when atoms bond together to form new compounds or when compounds separate to form other compounds. Chemical reactions can be identified by certain characteristics like gas produced, light produced, temperature change, color change, or precipitate formed.
introduction to puckers.pptx
1) The document discusses various types of evidence that indicate a chemical reaction has occurred, including temperature change, gas formation, color change, and precipitate formation.
2) It describes word equations, skeleton equations, and how to translate between the two. Balancing equations requires using coefficients to satisfy the law of conservation of mass.
3) Key characteristics of the main types of chemical reactions - synthesis, decomposition, single replacement, double replacement, and combustion - are outlined.
Tang 07 equilibrium and solubility 2
This document discusses solubility equilibria and the formation of precipitates. It defines key terms like solubility product constant (Ksp), explains how to calculate Ksp values from molar solubility and vice versa, and shows examples of using Ksp to determine whether precipitates will form when solutions are mixed. The key points are that solubility is dependent on equilibrium, saturated solutions have concentrations where Ksp = Q, and precipitates form when mixing produces Q > Ksp (supersaturation).
Chemistry - Types of Reactions Lab
This document describes a chemistry experiment involving 6 chemical reactions using common reagents like magnesium, zinc, copper sulfate, sodium chloride, silver nitrate, lead nitrate, and potassium iodide. Balanced chemical equations are provided for each reaction along with observations and safety precautions. Questions at the end assess understanding of precipitation reactions, gas tests, and identifying reaction types.
Types of Chemical Reactions.ppt
Decomposition reaction
Combination reaction
Combustion reaction
Neutralization reaction
Single displacement reaction
Double displacement reaction
Precipitation reaction
Redox reaction
Planning and Designing Lab
This experiment aims to identify alkanes and alkenes by their reactions with different substances and determine their properties. Cyclohexane and cyclohexene are used as representative alkanes and alkenes, respectively. A series of tests are conducted including bromine, potassium permanganate, sulfuric acid and sodium hydroxide tests. The results show that cyclohexene is more reactive than cyclohexane due to the presence of a carbon-carbon double bond, undergoing addition reactions, while cyclohexane only undergoes substitution reactions. This supports the hypothesis that alkenes are much more reactive than alkanes.
Solubility intro
This document discusses how to write ionic equations for dissolution and precipitation reactions. It explains that dissolution reactions involve a solid salt breaking into its constituent ions in aqueous solution. Precipitation reactions involve mixing ions that form an insoluble solid product. The document provides examples of writing balanced equations for calcium chloride dissolving, potassium nitrate dissolving with nitrate staying together as a polyatomic ion, and silver and chloride ions forming an insoluble silver chloride precipitate.
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Precipitation react 1
- 1. CHEMISTRY Bryan Terán & Andrea Alonso
- 2. Precipitationin DoubleDisplacementReactions In this lab activitywe have to observe precipitation reactions by mixing aqueous solutions of cations and anions. We have to Indicate which 2 cations form the most precipitates.
- 3. Materialsfor the practise Pb(NO3)2 KI NaOH Na2CO3 AgNO3 KNO3 CaCl2 NaCl FeCl3 CuSO4 Test tubes Test tubes rack
- 4. Procedure 1- Place 21 clean test tubes in a test tube rack 2- Add 6 drops of the solution indicated at the worksheet to 7 clean test tubes 3- Add 6 drops of AgNO3, Pb(NO3)2and CaCl2solution to everytest tube
- 5. EXEMPLES 4- Observe and record information and color of precipitates formed For example … Pb ( NO 3)2 reaction with NaCl to form PbCl2 and Na(NO3)
- 6. But one of the new compounds are not soluble and precipitates are formed The Cl- ions aren’t soluble with Pb++. Pb(NO3)2 + NaCl PbCl2 + NaNO3 white
- 7. More exemples… This reaction between AgNO3 and KI, forms AgI and KNO3. The Ion I- isn’t soluble with Ag and forms precipitates.
- 8. At the end… After mixing all the compounds and balance the reactions… …5- We must tidy and clean all the materials
- 9. REMEMBER! We must not make any reaction without the supervision of our teacher FELISA PINILLA.
- 10. VERY IMPORTANT!! And even more important, -not to ingest any material…