up the experiment’s equipment as shown on figure 1. As you can see by figure 1‚ I have used the reaction between sodium thisoulphate solution and hydrochloric acid (HCL) to come up with results that will help me draw conclusions regarding the effects of the concentration of the acid. I decided to use this particular reaction due to the fact that the product of the reaction between sodium thisoulphate and hydrochloric acid (HCL) is precipitates of sulphur which tend to turn the solution cloudy. As a
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the acid. Rinse with the alkali. The labels fell off two bottles each containing a colourless solution‚ one of which was sodium carbonate solution and the other was sodium chloride solution. The addition of which solution to a sample from each bottle would most readily enable the bottles to be correctly relabelled? A B C D ammonia hydrochloric acid lead(II) nitrate sodium hydroxide © UCLES 2011 5070/11/O/N/11 3 3 Oxygen was prepared from hydrogen peroxide‚ with manganese(IV) oxide as
Free Oxygen Oxide Chlorine
associated with even small amounts of each of the following: a. concentrated hydrochloric acid‚ HCl HCL may be corrosive. It can cause burns to dosy tissue and can be deadly if inhaled or swallowed. b. sodium hydroxide‚ NaOH‚ solution NaOH is a very corrosive chemical and contact with it can cause burns to body tissue and possible eye damage. Can irriate the lungs and can cause permanent lung damage. also contact with water can generate enought heat
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Bag: LeChatelier’s Principle 1 E.D.T.A.‚ .15 M (Na2EDTA) - 2 mL in‚ Pipet 1 Hydrochloric Acid‚ 6 M - 2 mL in Pipet 1 Magnesium Chloride‚ 2 M - 3 mL in Pipet 1 Phenolphthalein Solution‚ 1% - 0.5 mL in Pipet 2 Pipet‚ Empty Short Stem 1 Sodium Bisulfate Crystals - 0.5 g in Vial 1 Sodium Bisulfate‚ 0.1 M - 4 mL in Pipet 1 Sodium Hydroxide‚ 1 M - 2 mL in Pipet 1 Sodium Sulfate‚ 1 M - 2 mL in Pipet 1 Thymol Blue Indicator‚ 0.04% - 0.5 mL in Pipet Experiment procedure: Part I: 1. Prepare an ice
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Calculate the [Fe3+] in a 0.25 M solution of Fe2(SO4)3? 9. Calculate the [Na+] in a 0.55 M solution of sodium acetate. (Write the proper formula for sodium acetate first). 10. Calculate the [Na+] in a 0.55 M solution of sodium carbonate. (Write the proper formula for sodium carbonate first.) 11. Calculate the [Na+] in a 0.55 M solution of sodium phosphate. (Write the proper formula for sodium carbonate first.) 12. 300 mL of 0.500 M NaCl is mixed with 400 mL of 0.200 M HCl. Calculate the final
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3.6.2. Hygroscopicity assessment of free films Free films were evaluated for hygroscopicity behavior to understand the contribution of lactose and sodium chloride on hygroscopicity‚ if any. It was found that HPMC SD and HPMC-LAC CP films were ‘moderately hygroscopic’ whereas HPMC-NaCl CP films were ‘very hygroscopic’. The percentage moisture content and classification of each sample as per Callahan et al. (Callahan et al.‚ 1982; Murikipudi et al.‚ 2013) has been listed in Table 5. 4. Discussion In
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mess and would take a long time to dry. A drying procedure is therefore necessary to remove all traces of water before the solvent is evaporated. This procedure consists of two steps: (1) thoroughly mixing the solution with saturated aqueous sodium chloride (saturated salt solution) and discarding the aqueous layer (this is a preliminary drying step that removes most of the water) and (2)‚ adding a solid inorganic drying agent (this strongly binds to the remaining traces of water dissolved in the
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from aqueous solutions of calcium chloride and sodium carbonate. These solutions will be prepared from 2.01 g of calcium chloride and 1.06 g of sodium carbonate . Materials: 3 beakers 100 mL graduated cylinder rubber policeman funnel filter paper Procedure: 1. Put on your safety goggles. 2. Obtain two clean beakers. Rinse the inside of the beakers with a small amount of distilled water. 3. Obtain the correct amounts of calcium chloride and sodium carbonate. Enter these masses in
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max expansion‚ covers more surface area‚ lays flatter on surfaceWater: did not form even circle‚ reached max expansion very quickly‚ formed more of a bubble on surfaceBOTH: Clear and shiny | e) Making iodine in water: potassium iodide (KI)‚ and sodium hypochlorite (bleach‚ NaClO). | KI- ClearNaOCl- ClearWhen combined they solution immediately turned a bright yellow. |
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Sodium Oxalate Sodium oxalate is the sodium or salt component of oxalic acid. Typically sodium oxalate is an odorless‚ white‚ and crystalline powder that decomposes at extremely high temperatures. Sodium oxalate is typically used as a reducing agent in most natural metabolic processes in plants and vegetables‚ and may also often be used as a primary standard for the standardization of potassium permanganate solutions. Like most other oxalates‚ sodium oxalates is highly toxic
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