Sodium bicarbonate and dilute sulfuric Experiment 5 ionic reactions Pour about 2mL of aqueous sodium bicarbonate into an evaporating dish, not a test tube.
Determine if any of the new compounds are insoluble using the solubility rules: Add about 2mL of each of the two reagents. Which anions generally do not form precipitates?
Write the formulae and names for the possible new compounds: Note any temperature changes by touching the test tube. Such reactions can be classified into other reaction types as well. Also, following this section, is a set of solubility rules which will enable you to identify any insoluble solid precipitate formed during a reaction.
Record the well numbers of the precipitates you chose for your equations. Place 2 drops of sodium bicarbonate solution into five vertical wells under 5. A white precipitate appears and the solution gets warm when solutions of barium hydroxide and phosphoric acid are mixed.
Gas-forming Reactions A reaction in which a gas is produced, bubbles form in the solution, is called a gas forming reaction.
Sodium bicarbonate and barium chloride 8. When a salt dissolves in water, it separates into its constituent cations and anions. Place 2 drops of sodium chloride solution into five vertical wells under 4. This is the precipitate. Stir with a glass rod.
Switch the partners of the original salts Be sure each cation is paired with a new anion: Note the rate of evolution of bubbles of oxygen. Although I feel this experiment was interesting, I believe directions could have been more clear and detailed for better results.
In this experiment the only bases used will be those containing the hydroxide ion OH. This is an aqueous solution and will be denoted with aq. The final form of the equation would be: Gas Forming Reactions Some reactions can be classified as more than one of the reaction types listed above, and also may be called single-replacement or double-replacement reactions.
Write the results of the tests with litmus paper into your laboratory notebook. Sodium hydroxide and dilute sulfuric acid Obtain 2mL of aqueous sodium hydroxide in a small test tube.
The proper technique is to dip a clean stirring rod into the solution and then touch the stirring rod to the litmus paper. Write careful observations into your laboratory notebook. Hydrogen peroxide decomposes to form liquid water and oxygen gas. The purpose of this experiment is to work with solutions of ionic substances.
Do not perform reactions at the main dispensing hood. Obtain 2mL of dilute sulfuric acid in another test tube. The focus of this experiment is on precipitates. If the precipitates are allowed to dry they are much harder to remove.
Set up a Bunsen burner, ring stand and ring, and a clay triangle. Copper II sulfate and sodium chloride After you have run each reaction, write down all observations including colors of original reagent solutions, amount of precipitate formed and colors of precipitates.
Sodium phosphate solution will react with calcium chloride solution to form a white precipitate. Just by looking at the solubility rules, my results were what I expected them to be.
Determine the formulae of the reactants: Do not measure these volumes, use 40 drops or approximately 2mL as shown by your instructor. In a neutral solution, litmus paper is lavender In a basic solution, litmus paper is blue.
Silver nitrate and potassium bromide 5. Gently stir the ash with a glass rod and describe the appearance of the ash in your laboratory notebook. Consider the ions that are formed when the salts dissolve:EXPERIMENT 9: Double Replacement Reactions PURPOSE a) To identify the ions present in various aqueous solutions.
b) To systematically combine solutions and identify the reactions that form precipitates and gases. 5 This leaves the net ionic equation, Ag+ (aq). The goal of this experiment is to study the nature of ionic reactions, write balanced equations, and to write net ionic equations for precipitation reactions.
Based on the solubility rules my results proved accurate.
PURPOSE EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS To perform and observe simple chemical reactions. To identify the products of chemical reactions and write balanced equations for those reactions.
Experiment 1 Chemical Reactions and Net Ionic Equations. Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict.
Ionic Reactions Lab. Chem Lab 5: Ionic Reactions Submitted by Abstract: The purpose of this experiment is to work with aqueous solutions of ionic substances. Aqueous solutions are those solutions in which water is the solvent.
When ionic substances are dissolved in water, the ions separate and become surrounded by water molecules. The focus of this experiment is on precipitates.
Experiment 6 Chemical Reactions OUTCOMES After completing this experiment, the student should be able to: write balanced chemical equations and net ionic equations.
identify the species being oxidized and reduced in oxidation-reduction reactions. DISCUSSION. Purpose The purpose of this experiment is to study ionic reactions, to be able to write balanced equations, and to be able to write net ionic equations for precipitation reactions. Procedure First, all reactions will be completed in the well plate.Download