also occur. Anhydrous CuSO4 is white‚ but upon exposure to air‚ the anhydrous salt absorbs water. This reaction produces blue CuSO4·5 H2O. In some cases‚ compounds can actually dissolve in their water of hydration. Salts such as calcium chloride (CaCl2)‚ calcium sulfate (CaSO4)‚ and magnesium sulfate (MgSO4)‚ can absorb so much water that they form solutions. These salts are said to be deliquescent. We often use anhydrous salts of this type as drying agents. Some hydrated salts such as Na2SO4·10
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Chemistry Stage 3 Standards Guide Exemplification of Standards through the 2010 WACE Examination Chemistry: Stage 3 Standards Guide 1 2010/33606 Copyright © Curriculum Council‚ 2011 This document—apart from any third party copyright material contained in it—may be freely copied‚ or communicated on an intranet‚ for noncommercial purposes by educational institutions‚ provided that it is not changed in any way and that the Curriculum Council is acknowledged as the copyright owner. Copying
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Discussion Questions 1. Why do different metals have different characteristic flame test colours? The photons emitted during the test precisely match the quantum energy difference between the excited state and the ground state. For different elements the spacing between the ground state and the higher energy levels is different. So different elements have different flame test colours. 2. Most salts contain a metal and a non-metal. Look at the compounds we tested and determine whether it is
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1 a The diagram shows the parts of a hydrogen atom. [pic] Use words from the list to label the diagram. electron group nucleus symbol (2) b Hydrogen can be used as a clean fuel for cars. i When hydrogen burns in air‚ it reacts with another element. Complete the word equation for this reaction. hydrogen + ................... → water (1) ii Suggest one reason why hydrogen is called a clean fuel. (1)
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Isolation: * 1 Cup Wheat Flour * Cheese Cloth * Iodine Solution * Water Qualitative Color Reaction Tests: * Isolated Gluten * 2.5 M‚ 3 M‚& 6 M NaOH * 10% & 20% NaOH * Conc. NaOH solution * 5% NaNO2 * 10% Na2CO3 * 2% Nitroprusside solution * 0.02% Naphthol solution * 1% Sulfanilic acid * 0.1% Ninhydrin solution * Conc. HNO3 * Conc. H2SO4 * Hopkins-Cole
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Introduction to Chemistry Laboratory: A Lesson on Tools‚ Techniques and Measurements PURPOSE: The purpose of this set of experiments (3 total) is to become familiar with the common types of laboratory glassware and equipment‚ and how to obtain and analyze data from these items. LEARNING OBJECTIVES: By the end of this experiment‚ the student should be able to demonstrate the following proficiencies: 1. Know which glassware (beakers‚ burettes‚ pipettes‚ graduated cylinders‚ flasks‚ etc) should
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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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Unit 2 learning Aim C - How fast is your reaction? – Part 3 Safety Wear eye protection while doing the practical work and keep it on when clearing up and washing things out in the sink. Avoid skin contact with all the solutions used and wash off any splashes on your skin with cold running water. Apparatus required eye protection timer 2 measuring cylinders (100 cm3) pipette paper with a black cross on it Chemicals required sodium thiosulfate solution (15 g/dm3) cobalt(II) chloride solution
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Ionic Reactions Abstract This experiment is designed to study the nature of ionic reactions‚ and write net ionic equations for precipitation reactions‚ as well as to identify spectator ions‚ perception reactions and solubility of different compounds. Experiment and Observations In this experiment I was using a 96-well plate to add two drops of the following solutions into seven wells in rows A through E: cobalt (II) nitrate‚ copper (II) nitrate‚ iron (III) nitrate‚ barium
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help remove and purify a particular substance in that case was 1-bromobutane‚ from other components in the reaction flask. Separation was carried out because there was a high probability of other components in the distillate. And finally we used CaCl2 as a very good drying agent for a variety of solvents. So for instance‚ 1-butanol is the limiting reagent‚ theoretically 29.95g of 1-bromobutane. Our percent yield was 15.8% as showed in the calculations. Our volume was 1.247 g/mL. And as finally
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