When you mix copper‚ silver‚ and nitrate together‚ you will end up with silver nitrate solution will turn blue (it has become copper nitrate). On the piece of copper‚ there would be a coating of solid silver. If a chemical reaction is going to be observed when chemicals are mixed‚ heated or any other means of altering the substance‚ then we will be able to predict the products formed. If it is observed that in the original versus the changed substance no new substances are formed‚ the change is reversible
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One of the chemicals provided differed slightly from chemical description in the lab manual. The lab manual called for the chemical NH3 which is Ammonia. The chemical provided was an Aqueous Ammonia solution of NH4OH. When holding up the solution of AgNO3 and NH4OH to a light source for 5 minutes it was observed that no reactions took place despite the information contained in the lab manual. Also while testing the household chemical Brite‚ It was observed that the Bromthymol Blue changed to a green color that was not
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reactions of the chemicals that undergoes SN1 or SN2 reaction. Nine different compounds were given to be examined with two reagents - NaI in acetone and AgNO3 in ethanol. The SN1 reaction happens in AgNO3 in ethanol reagents‚ and SN2 reaction is in NaI in acetone. Procedure: Following the lab manual. Results: compound NaI /acetone (SN2) AgNO3/ethanol (SN1) Bromobenzene NR NR Bromocyclopentane X 2 sec Bromocyclohexane NR 4 sec 2-bromobutane 5 min 2 sec 2-chlorobutane
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98.) Consider the unbalanced redox reaction: Cr2O72- (aq ) + Cu(s ) → Cr3+ (aq ) + Cu2+ Balance the equation in acidic solution and determine how much of a 0.850 M K2Cr2O7 solution is required to completely dissolve 5.25 g of Cu. Nitric acid is usually purchased in concentrated form with a 70.3% HNO3 concentration by mass and a density of 1.41 g/mL. How much of the concentrated stock solution in milliliters should you use to make 2.5 L of 0.500 M HNO3? Mass %= Mass Solute/ Mass Solvent + Mass
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observable reaction (or lack thereof). Exceptions included part C where one drop of BTB (bromthymol blue) was used and part E where an additional drop of HCI (hydrochloric acid) was added to blue dye and NaOCI (sodium hypochlorite). In part K‚ the AgNO3 (silver nitrate) and NaOH (sodium hydroxide) mixture was saturated into a paper towel and exposed to a bright light. The resulting mixtures were then observed against two different backgrounds‚ one white and one black‚ by slipping a white piece of
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UTAR FHSC1134 Inorganic Chemistry Trimester 3 Experiment 1 ________________________________________________________________________ Title: Investigating the Properties of Period 3 Oxides Aim: To examine the oxides of Period 3 elements and describe their structure and bonding. Introduction: Generally‚ there are oxides of metals and non-metals. Metals burn in oxygen to form basic oxides while non-metals form acidic oxides. Structurally‚ they are covalent or ionic compounds. You are to
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Once it has been dissolved from the other two cations‚ it is centrifuged and the liquid is decanted into another test tube. Once in the other test tube‚ a drop of 6.0 M acetic acid and two drops of 1.0 M K2CrO4 is added to the saved liquid. If the lead (II) cation is present‚ a yellow precipitate forms and ensures the presence of that cation. When testing my unknown solution‚ the lead (II) ion was not present in my solution. To further separate the cations
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Gerona‚ Evelyn Chemical Reactions Experiment No. 7 Date Performed: Feb. 17‚ 2014 Date Submitted: Feb. 24‚ 2014 Mrs. Vitancol I. Theoretical Framework A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Classically‚ chemical reactions encompass changes that only involve the positions of electrons in the forming and breaking of chemical bonds between atoms‚ with no change to the nuclei (no change to the elements present)‚ and can often
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Oxidation Lab Part 1: Purpose: You are going to investigate the ease with which different metals undergo oxidation and reduction. Materials: | 4 samples of each of: lead‚ zinc‚ iron‚ copper | spot plates steel wool/sand paper | | | | Solutions of: | copper(II) sulfate Ferric nitrate Silver nitrate Lead (II) nitrate | | Procedure: 1. Obtain 4 samples of each metal and clean with steel wool or sand paper. Wash your hands after cleaning the metals so you are not exposed to lead
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reagents are added into the tubes 2 M NaOH 2 M NH4OH 0.5 M K4Fe(CN)6. - Record your observations. 2. REACTIONS OF SILVER HALIDES - Prepare 3 test tubes‚ 10 drops of 0.5 M KCl‚ 0.5 M KBr‚ and 0.5 M KI are added into each one- Add 10 drops of 0.1 M AgNO3 to each salt solution. Record your observations. - Each test tubes are divided into 2 test tubes and labeled 1-3 A and 1-3 B - Test tubes 1-3 A 5 drops of 2 M NH4OH are added to each of test tubes. Observe the change. - Test tubes 1-3 B 5 drops
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