...Baking Soda & Baking Powder Baking Soda What Is Baking Soda? This household item has been around for thousands of years, it is very good for uses in and around the home, and has quite a number of different uses. It is well known and widely used, and can also be known by the names bread soda, cooking soda, and bicarbonate soda. The Chemical Name for Baking Soda Is Sodium Hydrogen Carbonate and the Chemical Formula Is NaHCO3 What Is It Used For It is commonly used as an antacid in cooking as it reacts with acidic ingredients such as buttermilk and yogurt. It can also neutralize both acids and bases and id often used to mop small chemical spills involving acidic or basic substances The Reaction with Vinegar Baking Soda reacts vigorously with vinegar to produce Carbon Dioxide (CO2). The chemical equation for this reaction is Sodium bicarbonate and vinegar => Sodium acetate and water and carbon dioxide NaHCO3 + CH3COOH => CH3COO-Na+ + H2O + CO2 Baking Powder Baking powder is a dry chemical leavening agent, a mixture of a weak alkali and a weak acid, and is used for increasing the volume and lightening the texture of baked goods. Baking powder works by releasing carbon dioxide gas into a batter or dough through an acid-base reaction, causing bubbles in the wet mixture to expand and thus leavening the mixture. It is used instead of yeast for end-products where fermentation flavours would be undesirable or where the batter lacks the elastic structure to hold...
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...percentage left behind. A deficiency in any of the minerals within ash would result in a wide range of health problems which is why it is a legal requirement to display the ash content on food packaging. This experiment is designed to recreate the process undergone by the pet food company to determine the ash content within the food. Method Weigh silica crucible and record weight prior to experiment. Grind over 5g of food sample in pestle and mortar and measure 5g of ground sample into the crucible. (W0) Place the dish in a baking oven for 24hrs to dry out the sample. Reweigh the sample in silica crucible, This is now the true weight of the sample (W1) Set up the bunsen burner on top of the heatproof mat with tripod and clay pipe triangle above to support the crucible. Ignite the bunsen burner and begin to heat the sample slowly ensuring the sample does not set on fire as this will result in a loss of material to the atmosphere in the form of particles. The sample should turn black. Once the sample reaches roughly 100°C continue to heat to 500°C until the sample turns white. Allow sample to cool to room temperature in a dessicator. Weigh the finished sample (W2) Calculate the ash content (X): (W2-W0)/(W1/W0)x100=X Materials: Silica dish Baking Oven Bunsen Burner Matches Tripod Clay pipe triangle Heat proof mat Measuring scales (accurate to 3 decimal points) Pestle and mortar 6g Food sample Results W0=13.134 W1=18.135 W2=13.595 (13.595-13.134)/(18...
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...| Experiment to find the amount of water in a hydrated compound | Calculating Reacting Quantities and Formulae | | Contents Aim 2 Introduction 2 Hypothesis 3 Apparatus 3 Method 3 Results 4 Calculation 4 Conclusion 5 Evaluation 5 Bibliography 6 Aim The aim of this experiment is to find the number of molecules of water of crystallisation combined with one molecule of magnesium sulphate and to ultimately find the formula of the hydrated salt. Introduction Within crystals of certain salts, there are a fixed number of water molecules, combined chemically in a fixed proportion. When a salt crystallises from a solution, it forms hydrated salts which contain water molecules that are loosely bonded together. The name for this is the water of crystallisation or water of hydration. Magnesium sulphate contains seven molecules of water (H2O) for each formula unit of MgSO4 and can be written like this: - MgSO4.7H2O The dot shows the weak salt/chemical bond in the formula. To determine the formula of a hydrated salt, it must be heated so that the water of crystallisation evaporates. When magnesium sulphate has been heated, the water is removed to form an anhydrous salt. This can be reversed by adding water to the anhydrous salt to make it hydrated which will cause the water to reattach itself to the salt. Other substances that act similarly to hydrates, but have distinct individual characteristics are:- * Hygroscopic – substances...
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...which provides a measure of the total amount of minerals within a food.” It’s important for the correct amount of ash to be in a dog’s diet because as Professional Pet Foods (2013) explain, “excess ash will contribute excess minerals to the diet, potentially leading to health problems.” Method This method can be used for all types of food containing less than 50% fat, it allows for the determination of the mineral content of foodstuffs. In this process, the samples temperature is taken to 550°C to ensure all organic matter is burnt leaving only the mineral content of the food. The heating of the food sample is carried out in stages to prevent it setting on fire. Equipment: * Silica dish * Baking oven * Bunsen burner and apparatus * Food sample (crushed with pestle and mortar) * Measuring scales (accurate to at least 2 decimal places) Method: 1. Weigh the silica dish prior to the...
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...Properties of Substances and Their Structures (experiment B) Aim To investigate the empirical formula of a compound and to specify the empirical formula of a compound. Hypothesis I predict that the mass of copper sulfate will decrease if heated / burned, because the hydrogen inside it will vaporize and therefore the mass of CuSO4 after heated / burned decrease. Variables Independent : CuSO(Copper Sulfate) Dependent : Mass of curcible and magnesium; mass of curcible and magnesium oxide Control : Same mass of empty curcible, sama mass of magnesium before burned Materials Name of compound | Quantity | Hydrated cooper(II) sulfate (CuSO) | 1 | Bunsen Burner | 1 | Tripos stand | 1 | Pipeclay triangle | 1 | Crubicle | 1 | Pair of tongs | 1 | Electronic balencing | 1 | Sand paper | 3 | Procedures 1). Clean up the crucible until there’s nothing in it. 2). Weight an empty crucible. 3). Crush the CuSO until it become powder. 4). Measure the magnesium (CuSO) about 2 g. 5). Put it in the empty crucible. 6). Heat it until 5 minutes and another 5 minutes until the weight of crucible +magnesium after each minutes become constant. 7) Repeat step 3 – 6 for the second trial. Data Collection After Burned and the mass is constant. Trial | Mass of Crucible + Magnesium Oxide (g) | 1 | 55,19 g | 2 | 54,57 g | ∑Mass | 54,88 g | Trial | Mass of Crucible + Magnesium (g) | 1 | 54,19 g | 2 | 53,78 g | ∑Mass | 53...
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...Austin Neely August 31st, 2015 Experiment #01 The Determination of the Percent of Water in a Compound CHEM 1315‐ 025 Purpose of the Experiment & Techniques: The purpose of this experiment is to determine the percent of water in a hygroscopic compound. This will be done by boiling off the water only leaving the other element of the hygroscopic compound. When water molecules bond with the structure of solid substances this creates an ionic compound. By heating the compound, it is possible to release that water (known as water of hydration) and determine the amount of water the ionic compound is able to hold. By the law of conservation of mass when the compound is heated the water just doesn’t disappear which means...
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...WATER OF HYDRATION Experiment No. 5 I. Objectives 1. To be able to identify and know the different properties of hydrates. 2. To observe and test the reversibility of hydration reaction. 3. To test and compare substance for efflorescence and deliquescence. 4. To determine the percent water in a hydrate. II. Results and Discussions According to Hamak, Hydrates are ionic compounds (crystalline salts) that are bonded to water molecules thus having a definite amount of it as part of their structures. This “water of hydration” is released as vapor when the hydrate is heated in which it loses water and become dehydrated (anhydrous). The remaining solid is known as the anhydrous salt. The general reaction for heating a hydrate is: A. Identification of Hydrates Compounds of Nickel Chloride (NiCl2), Potassium Chloride (KCl), Sodium Tetraborate or Borax (Na2B4O7·10H2O), Sucrose (C12H22O11), Potassium dichromate (K2Cr2O7) and Barium Chloride (BaCl2) each in about 0.5 grams were heated on a Bunsen flame and their behavior was then observed specifically determining whether one is a hydrate. Refer to TABLE 1. Fig.1. Unheated Compounds TABLE 1. Summary and analysis of the results pertaining to the tested compounds ...
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...glassware use a liquid detergent in place of the scouring powder. Occasionally, specific chemical deposits are completely unaffected by these general cleaning methods, but if the chemical nature of the deposit is known, a specific reagent may be selected for cleaning; ask your instructor for advice in this circumstance. Drying Operations Glassware must frequently be dry as well as clean. This is best done by putting the glassware into a drying oven, preferably one with circulating air that will quickly remove the water vapor. Hot glassware with parallel sides, such as beakers and bottles, is most conveniently handled with beaker tongs as shown in Fig. 2. It is unwise to dry Pyrex and Kimax equipment by direct heating with a Bunsen burner; it is usually fatal (to the glassware) to treat soft glass equipment this way. Alternatives to the drying oven are wiping with clean toweling (but cloth and paper lint are often a problem), or rinsing with volatile acetone followed by drawing clean air through the container; however, acetone is rather expensive and highly flammable. A common requirement, especially in quantitative analysis, is a very dry sample or product. These materials are usually dried in the drying oven at a specified temperature for a specified length of time, followed by immediate transfer to a...
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...B): Making the Iron Sulphide: As soon as the sulphur and iron was placed over the Bunsen burner in the crucible, the sulphur started dissolving and producing bubbles (effervescence) and soon there was a liquid looking substance surrounding the iron. After the mixture had been taken off the Bunsen burner there was a blue flame being sustained over the mixture for about 30 seconds. After being off the Bunsen burner for approximately 5 minutes the combination of iron and sulphur had turned into a grainy black powder (iron sulphide). Examining new Substance: In the foil there was a gold-brown sand like substance and a blue grainy substance. The iron sulphide was the blue and the gold-brown were the extra iron filings that weren’t dissolved into the new substance. The iron sulphide had no distinct small and had a slight magnetic pull when a magnet was put up against the side of the foil. The spikes were once again directed away from the...
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...Purpose How do we determine the reaction type and write a balanced equation for chemical reactions? Background Discussion There are many kinds of chemical reactions and several ways of classifying them. One popular and useful method is to classify reactions into five major types. These are: (1) synthesis, (2) decomposition, (3) single replacement, (4) double replacement, and (5) combustion. Most reactions can be put into one of these categories. In a synthesis reaction, two or more substances (elements or compounds) combine to form a more complex substance. A decomposition reaction is exactly the opposite of a synthesis reaction. In a decomposition reaction, a compound breaks down into two or more simpler substances (elements or simpler compounds.) In a single replacement reaction, one element in a compound is replaced by a more active element. In a double replacement reaction, the positive ions of two different ionic compounds can be thought of as “replacing each other.” Most replacement reactions (both single and double) take place in aqueous solutions containing free ions. In a double replacement reaction, one of the products must be removed from the solution as a precipitate, water, or an insoluble gas. A precipitate is a solid that is produced as a result of a chemical reaction in solution. As the precipitate separates from the solution, the solution appears cloudy. In a combustion reaction a substance combines with oxygen, releasing a large amount...
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...Conclusion: This experiment aimed to find out the empirical formula of magnesium oxide. In order to determine the percentage composition and empirical formula of magnesium oxide, a 10cm piece of magnesium strip was placed inside a crucible and heated strongly with a bunsen burner, to react it with the oxygen in the air. The masses were measured before and after the reaction. Balanced equation for magnesium oxide: 2Mg + O2 2MgO (“Types of Reaction”) According to “Burning Magnesium”, after magnesium is heated and reacted with the oxygen in the air, it is suppose to form a white powder of MgO, which is exactly what is shown in table 1. The reason why this white powder was formed is because when heated magnesium gives up 2 electrons to O2 atoms. This reaction is an exothermic, gives off heat. In table 1, the observations were that it took a while till the crucible was touchable, and not as hot as it was before. Overall, Metal oxides are bases and they react with acids to neutralize them and this is why magnesium oxide is found in most ingredients for treating acid reflux. (“Types of Reaction”) As said in table 1, magnesium turns red and then lights up and catches fire,...
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...and chemical properties, were understood to have defined chemical change. The experimental procedures were divided into five phases: Magnesium and Oxygen, Zinc and Copper(II) Sulfate, Metals and HCl, Reactions of Ionic Compounds, and the Sodium Carbonate and HCl. Different Reactions were noted for each respective phase. When necessary, a numerical coefficient would be added before the name of the formula on either the reactant's or product's side to achieve a balanced chemical equation. Introduction Explosion of fireworks, pharmaceutical drugs(medicine), and fuel, what do they have in common? A chemical reaction! Most of these chemical reactions naturally occur without us having the slightest idea on that they exist. The focus of this experiment is to differentiate and classify different types of chemical reactions, and be aware of the significance and importance of these chemical reactions in our lives. One of the primary methods to classifying a synthesized chemical reaction is determining if it came from a : Combination, Single Replacement, Double Replacement, Decomposition, or a Combustion Reaction. Physical and Chemical Properties of the unaltered substances were noted and recorded as it was believed to have influenced the outcome or result of the reaction. Pre-cautionary measures and safety hazards would strictly be maintained especially when heating the Mg ribbon (looking directly at the light may possibly cause blindness), and dealing with the highly-reactive Hydrochloric...
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...Dadiangas University Discussion of Variables (Independent and Dependent) This research study was designed to investigate the effectives of laboratory equipment and facilities towards the performance of Health Sciences students. The variables under consideration are the laboratory equipment and facilities as our Independent variable and the student’s performance as our dependent variable. A laboratory (informally, lab) is a facility that provides controlled conditions in which scientific or technological research, experiments, and measurement may be performed. Labs used for scientific research take many forms because of the differing requirements of specialists in the various fields of science and engineering. Despite the great differences among laboratories, some features are common. Laboratory equipment refers to the various tools and equipment used by scientists working in a laboratory. Laboratory equipment is generally used to either perform an experiment or to take measurements and gather data. Larger or more sophisticated equipment is generally called a scientific instrument. However, in this study, we will be focusing on Health Sciences laboratories. Scientific laboratories can be...
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...Electrolytes and Electrical Conductivity Summary of Principles: In this experiment it will define the difference between strong electrolytes, weak electrolytes, and non electrolytes by measuring and comparing the conductivities of the various solutions that are made from these substances. And also predict whether a reaction occurs and to write net ionic equations. Substances such as NaCl and K2SO4 are called electrolytes. The other substances such as sucrose which doesn’t produce ions in aqueous solutions are called non electrolytes. Electrolytes can be further divided into two groups: strong electrolytes and weak electrolytes. Strong electrolytes dissociate to a large extent into ions when dissolved in water and weak electrolytes that are partially ionized. Equations and Mechanisms: Net Ionic Equations: AB+XY AY+XB The Ohms law : G(S)= 1/R=I(A)/V(V) Apparatus and Supplies: Balance, two crucibles and lids, Bunsen burner , cobalt(II) chloride hexahydrate (CoCl2x6H20), an unknown hydrate. Chemicals: Outline of experimental procedure: Part 1 A know hydrate CoCl2x6h20: * Obtain 20mL for each of the solutions list in the data and report sheet. * Obtain a calibrate a conductivity meter. * Rinse the electrode in deionized water and use a paper towel to dry it. * Dip the electrode into the solution. * When the display is stabilizes record the conductance reading. Mark SE-strong electrolytes, WE- weak electrolytes, NE-non electrolytes. * Wash the...
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...document/publication should be sent to us at enquiries@educationscotland.gov.uk. This document is also available from our website at www.educationscotland.gov.uk. Contents Introduction 5 Chemical analysis 6 Qualitative and quantitative analysis 6 Volumetric analysis 6 Gravimetric analysis 14 Colorimetric analysis 17 Organic techniques 22 Introduction 22 Preparation 22 Isolation 24 Purification 29 Identification 33 Percentage yield 37 Errors 39 Accuracy and precision 39 Repeatability and reproducibility 41 Quantifying errors 41 Absolute uncertainties and percentage uncertainties 42 Combining uncertainties 43 Some ‘forgotten’ uncertainties 46 Experiments 53 Experiment 1A: Preparation of a standard solution of 0.1 mol l–1 oxalic acid 53 Experiment 1B: Standardisation of approximately 0.1 mol l–1 sodium hydroxide 55 Experiment 1C: Determination of the ethanoic acid...
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