One method for preparing baking soda is through reacting crystalline ammonium hydrogen carbonate with brine according to the following equation: NH4HCO3(s) + NaCl (aq) --> NaHCO3(aq) +NH4Cl(aq) Eq. 1 Brine contains sodium chloride, the compound needed to make baking soda, as well as potassium chloride, lithium chloride, and calcium chloride. Once the reaction has been completed, the solid baking soda is filtered off, but some contaminants may be present in the solid. The first step in determining the purity of the sample is to perform thermal gravimetric analysis (Experiment 7) on the baking soda sample to determine the percent composition of sodium bicarbonate in the sample. A sample of the baking soda will be heated until it decomposes to leave solid sodium carbonate according to the following equation: 2NaHCO3(s) --> Na2CO3(s) + CO2(g) + H2O(g) Eq.
Never push, pull or drag heavy items as you might suffer from a musculoskeletal injury. Where items are heavy, ask a colleague to help you lift them and, if it’s still too heavy, use a lifting device in addition to following basic health and safety guidelines on how to lift objects. * Cuts You need to take great care when using knives in the kitchen and also beware of glass objects. You need to follow safe procedures when using knives and other sharp kitchen utensils and when handling items made of glass as both can cause severe damage in the form of cuts. * Exposure to Hot and Harmful Substances Oil and other fluids such as water are commonplace in kitchens and it’s important that you take extreme care when working with or in close proximity to hot liquids.
Problem Which dissolves in water better, salt or baking soda? Hypothesis If salt and baking soda where put in water then baking soda will dissolve better than salt. Abstract The purpose of this project is to determine which material dissolves better in water between salt and baking soda. The hypothesis is If salt and baking soda where put in water then baking soda will dissolve better than salt. One teaspoon of salt and one teaspoon of baking soda were put in two separate transparent glasses of water and then the time of dissolving of each substance were calculated.
There are a couple different ways to determine the percent composition of baking soda. The most common ways to find this percent composition are through titrations and thermal gravimetric analysis. When and if the NaHCO3 sample is found to be pure, these chemists must have a way to determine which salts are present. The best way to determine what the sample contains is by emission analysis. The first way to find the percent sample of baking soda is titration.
The capsule will soften but not completely dissolve in the water, however will dissolve in the Hydrochloric Acid. The Tablet will slowly dissolve in water, however more rapidly in Hydrochloric Acid – however loosely comparable to the dissolving tablet. Equipment * Water * 2M Hydrochloric Acid * Test Tubes or Beakers * Stopwatch * 2 x Aspirin Enteric Coated Tablets * 2 x Aspirin Capsule * 2 x Regular Aspirin Tablets * 2 x Dissolving Aspirin Tablets * Safety Glasse * (Recommended) Gloves for handling Hydrochloric Acid Safety Precautions * 2M Hydrochloric Acid will burn both skin and clothing * Always wear eye protection while handling Hydrochloric Acid * Avoid contact with
Knowing the different boiling points of the two liquids was useful in this experiment so that the sand bath could be heated to different temperatures to evaporate the two solvents. Once the liquid was evaporated the vapor was collected and condensed in the condenser allowing the collection of said liquid. When simple distillation occurred the liquid only evaporated and condensed one time as opposed to the fractional distillation. Fractional distillation was more accurate due to the fractionated column allowing multiple vaporization and condensation reactions to take place. Raoult’s Law was used in this experiment because it describes the vapor pressure that takes place in the experiment.
The acid intermediate helps prevent co-precipitation. Such quick precipitation also causes silver chloride to form into very small particles, called a colloid. To make it into a more definite form, the precipitate has to be heated and stirred gently in the presence of nitric acid. Ag+(aq) + Cl-(aq) + heat → AgCl(s) The nitric acid prevents the precipitate from reverting back to a colloid state. If the sample was to re-colloid, it would easily wash right through the filter, causing the analytical results to be low.
Weather-hot weather could result in sun burn if protection such as sun block isn’t used. Cold weather could result in flu or catching a cold. 2 2 2x2=4 To avoid getting flu, we should ensure that we are fully equipped for whether the weather is warm or cold. In the shop We could be exposed to chemical liquids such as cleaning solvents. 4 4 4x4=16 The adults should avoid contact with chemicals and avoid the aisle which consists of chemical hazards.
h) A way to make hard water softer is to put an sodium nitrate and create a precipitate to mellow out the reaction. Another way of making it softer is by removing the calcium ions one way of doing that is by boiling the solution to take out some of the ions. Conclusion: Overall, we determined that sodium carbonate, Na2CO3, is the anion that can be used to precipitate the most metal cations. Also, we learned that the anion sodium chloride, NaCl, could be used to remove silver ions from solutions. The stuff that I found interesting was that how many colours you can get when you mix the cations and anions
Purification By Crystallization Experiment perf: 6/25/12 Report submitted: 7/2/2012 Abstract: In this crystallization experiment we were trying to separate a crystalline solid from a reaction mixture that had impurities. We accomplished this by dissolving our solution which was Acetanilide in a solvent. After the mixture was boiled, we then added decolorizing charcoal to help remove the colored impurities. Once this mixture was hot enough we transferred it into another beaker by using a funnel and then let it cool off. When our filtered solution started to cool off over time crystals started to form.