| | 1. (Points: 5.4) | | Solids have a __________ shape and are not appreciably __________. a. definite, compressible b. definite, incompressible c. indefinite, compressible d. indefinite, incompressible e. sharp, convertible | | Save Answer | | 2. (Points: 5.4) | | In the following list, only __________ is not an example of a chemical reaction. a. dissolution of a penny in nitric acid b. the condensation of water vapor c. a burning candle d. the formation of polyethylene from ethylene e. the explosive reaction of hydrogen with oxygen, which produces water, | | Save Answer | | 3.
Title : Reaction of Carboxylic Acids Objective : To Determine The Reaction of Carboxylic Acids Procedure : As referred to Lab manual. Results: A. Salt Formation |Compound |Solvent |Solubility | |Benzoic Acid |Cold Water |Partially soluble | |Benzoic Acid |10 % NaOH |Soluble | B. Salt Hydrolysis Sodium acetate solution changed the color of litmus from red to blue. C. Reaction With Sodium Carbonate Observation : A lot of gas bubbles was released.
When the solution is acidified during diazotization to form nitrous acid, the sulfanilic acid is precipitated out of solution as a finely divided solid, which is immediately diazotized. The finely divided diazonium salt is allowed to react immediately with dimethlaniline in the solution in which it was precipitated. Mechanism Diazotization: [pic] Diazo Coupling: Methyl orange is often used as an acid-base indicator. In solutions that are more basic than pH 4.4, methyl orange exists almost entirely as the yellow negative ion. In solutions that are more acidic than pH 3.2, it is protonated to form a red dipolar ion.
Determining the Chemical Formula of a Hydrate Purpose: Find the molecular formula of the hydrate of Copper (II) Sulfate. Materials: * 400 mL beaker * Tongs * Scoopula * Electronic Balance * Glass Rod * Hot Pad * 3 g hydrated copper(II) sulphate * Eye Protection Hypothesis: This lab will demonstrate a dehydration reaction. When the beaker containing hydrated copper (II) sulphate is heated, the water will evaporate, causing the color to change from blue to white, and the mass to decrease. Procedure: 1. Measure & record mass of beaker 2.
It is based on the manipulation of the solubility at various temperatures. To have an successful recrystallization of the solid, there has to be an ideal solvent meaning the liquid in which the solid or solute is infinitely insoluble at room temperature and infinitely soluble at high temperature. This experiment will determine if the Benzoic acid will truly be soluble in the polar solvent such as water. It will also show the efficiency of the recrystallization process by comparing the experimental and literature values of melting point of the pure benzoic acid. Experimental: The experiment started with measuring the melting point range of impure benzoic acid.
The Formula of Magnesium Oxide Aim:- To find the empirical formula of magnesium oxide by burning a weighted amount of magnesium ribbon in air. Data collection, processing and presentation:- Qualitative Data: Before the magnesium strip was put in the crucible to react with oxygen it was a silverly shiny solid. when the magnesium started reacting with oxygen it changed color, but all that was seen was a white flash. As the reaction continued a white solid powder started forming around the magnesium and was soon starting to spread out all over the crucible. The ending result was some left over magnesium, that at this point was white, and the white solid powder that covered the crucible on all sides.
What mass of MgCO3 is contained in a 2.750g solid sample consisting of only MgCO3 and MgO if heating to decompose all the MgCO3 according to the following equation leaves a solid residue weighing 2.160g? Magnesium oxide is unaffected by the heat. MgCO3(s) MgO (s) + Co2 (g) 2. a) Consider the reaction of question 2. Suppose a 3.250 g sample containing only MgCO3 and MgO is 42.6% MgO. How many grams of CO2 would be liberated by complete thermal decomposition of the MgCO3 in the sample?
Experiment 9 – Decomposition of Baking Soda Introduction The decomposition of any metal hydrogen carbonate will result in the formation of that metal carbonate, water vapor, and carbon dioxide. This lab will investigate the decomposition of sodium hydrogen carbonate, NaHCO3, commonly called baking soda. It is governed by the following chemical equation: 2 NaHCO3sNa2CO3s+ H2O g+ CO2 (g) In this lab, the NaHCO3 will be decomposed to form Na2CO3. The first half of the experiment will use a pure sample of NaHCO3, and the second part will use a mixture containing only some NaHCO3. Depending on how well the first half of the experiment is performed, the percent yield of this reaction should be 100%.
Experimental results: Reaction 1: Metallic Copper with Nitric Acid Cu(s) + 4HNO3(aq) Cu(NO3)2(aq) +2NO2(g) + 2H2O(l) Net ionic: Cu(s) + 4H+(aq) + 2NO3- (aq) 2NO2 (g) + Cu2+ (aq) + 2H2O(l) Type of Reaction: Redox Reaction: Copper loses electrons and is oxidized to copper (II) ion. Nitrogen gains electrons from the copper ion, and is reduced to nitrogen dioxide gas. Nitric acid is an oxidizing agent. Copper is the reducing agent. Observations: * Solution turns green and bubbles * Warm to the touch * Brown gas produced * Copper Dissolves Reaction 2: Copper (II) Nitrate with Sodium Hydroxide Cu(NO3)2(aq) + 2NaOH(aq) Cu(OH)2(s) + 2NaNO3(aq) Net ionic: Cu2+(aq) + 2OH-(aq) Cu(OH)2(s) Type of Reaction: Precipitate Reaction Observations: * With addition of water, the solution becomes blue, thick, and slime-like * When added to litmus paper, paper turns dark blue * Dark blue shows that the solution is basic Reaction 3: Heating Copper Cu(OH)2(s) CuO(s) + H2O(l) Net ionic: Cu(OH)2(s) CuO(s) + H2O(g) Type of Reaction: Redox Reaction: Cu is oxidized from 2- to 2+.
Experiment 3.1: Reduction of Benzophenone with Sodium Borohydride. Safety precaution: Sodium Borohydride Toxic & Irritant Wash spillages away with water Light Petroleum Highly Flammable Keep away from flames Ethyl Acetate Highly Flammable Keep away from flames. Residue to non-halogenated waste solvent. Ethanol Flammable Keep away from flames Residue to sink with lots of water. Benzophenone Harmful & Irritant Wash spillages away with water Hydrochloric acid Corrosive & Irritant wash spillages away with water.