Name: ___________________________________ Date: ______________ Practice Test #3 ____ 1. When a precipitation reaction occurs, the ions that do not form the precipitate A) evaporate B) are cations only C) form a second insoluble compound in the solution D) are left dissolved in the solution E) none of these 2. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) ____ 3.
Name: 6.03: Calorimetry Data and Observations: Part I: Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations that you made over the course of part I. (4 points) I observed that when the metal is placed inside the calorimeter, it transfers heat to the water making the water increase temperature while the metal will decrease temperature. I also noticed that the system was the metal and the surroundings is the water, this is because the water is taking in the heat from the metal making the water warm. Metal Name Mass of Metal Volume of water Initial temp.
Oil hypothesis accept/reject = Accept, the final result had very little oil in it. b. Vinegar hypothesis accept/reject = Accept, the final result had very little vinegar in it. c. Laundry detergent hypothesis accept/reject = Accept, the final result had a great amount of laundry detergent in it. 3. What affects did each of the contaminants have on the water in the experiment?
First of all, a pharmaceutical product can be made from seaweed by heating seaweed in water. This causes the product to be extracted from the seaweed. After that, filtration is needed to extract the seaweed from the water. Finally, by evaporating the product can be extracted from the water. 2.
When water is added to a mixture of salt and sand, the salt dissolves, but the sand does not. The mixture can then be separated by a simple filtration. The salt leaves with the water and the sand is trapped on the filter. Neither the salt nor the sand has been chemically changed. In this laboratory, we used physical and chemical properties to separate the components of a ternary (three substances) mixture.
CHEMISTRY September 25, 2010 Experiment #5: Percentage of water in a Hydrate Summary of Principles In this lab, students will calculate the amount of water in an unknown hydrate. A hydrate is a compound with a specific number of water molecules associated with the ions of that compound. A hydrate may form when an anhydrous compound is exposed to atmospheric water or when the ionic compound is crystallized from an aqueous solution. An anhydrous compound is a substance without water. There are two parts to this lab.
A reporting entity may begin the second statement with net income. Although Zumiez states the total amount of comprehensive income, they fail to break out the components of their total anywhere in their financial statements. SFAS No. 130 requires the disclosure of comprehensive income and discusses how to report and disclose comprehensive income and its components, including net income. However, it does not specify when to recognize or how to measure the items that make up comprehensive income.
Lesson written by Carolina Sylvestri Experiment: Reaction Between Ions in Aqueous Solutions The Monster Mash Background: Ionic solids dissolve in water to form aqueous solutions which conduct electricity. These solutions contain both positive and negative ions in such numbers that their net electric charge is zero. In this experiment, you will mix various ionic solutions, two at a time, to determine which combinations form precipitates. Knowing which ions are present makes it possible to deduce which of the possible ion combinations are responsible for the precipitates. From your data table, it will then be possible to generate a solubility table.
Purpose: The purpose of this lab is to investigate whether mass is gained or lost during a chemical reaction. Hypothesis: It will be found out that the mass is neither gained nor lost during a chemical reaction but transferred. Materials: * Safety goggles * Erlenmeyer flask * Balance * Graduated Cylinder * Beaker * Iron (III) chloride solution * Copper (II) sulphate solution * Sodium bicarbonate * Test tubes (small, and large) * Rubber Stopper * Tweezers * Paper towel * Scoopula * Sodium hydroxide solution * Hydrochloric acid Procedure: 1. 5ml of iron (III) chloride was measured and placed in the Erlenmeyer flask. 2.
Discussion: Analyze and discuss your results. Did your results support your hypothesis? What there a significant difference between the experimental and control subjects? Can any conclusions be drawn? How much confidence do you place in your results?