Producing Chloride Using Nitrate and Sodium Chloride Purpose of activity The purpose of the activity was to produce the insoluble salt silver chloride using the soluble salts silver nitrate and sodium chloride which I prepared in unit 1 activity 2a AB + CD = AD + CB ================= silver nitrate + sodium chloride = silver chloride + sodium nitrate Portfolio Evidence – (Lukas Chamberlain) Activity 3.1-3c: Precipitation Safety Points Sodium Chloride · Wear safety goggles · Do not eat · Use smallest amounts possible on a watch glass to prevent contamination of the bottle · Test for sodium last as the nichrome wire is difficult to clean afterwards · Wear suitable protective clothing · If splashed in eyes: In case of contact with eyes, rinse immediately with cold water and seek medical advice · If spilt on floor: Scoop up and clean surface · If spilt on skin or clothing: Wash off · Irritant Silver Nitrate · Wear safety goggles · Wear goggles · Use lowest mole and lowest volume needed · Wear suitable clothing · If splashed in eye: Rinse eye for ten minutes · If spilt on floor: scoop up and wash surface · If spilt on skin: wash thoroughly · Corrosive · Irritant · Oxidising · Danger to environment Silver Chloride None listed Sodium Nitrate None listed Portfolio Evidence – (Lukas Chamberlain) Activity 3.1-3c: Precipitation Method and material 1. I carefully measured out 10 cm3 silver nitrate using a 10cm3 measuring cylinder for accuracy. I did this over a sink, and then I poured the... ... middle of paper ... ...d also mean that the safety points are probably larger because there is a risk of more being spilt so it would cause more damage. The silver nitrate is also produced to a higher level of accuracy as less is wasted and that means more profit. Portfolio Evidence – (Lukas Chamberlain) Activity 3.1-3c: Precipitation Observations during procedure I observed that the washings that I collected after I filter out the precipitate was cloudy showing that it still had particles of silver nitrate as that is a insoluble salt and does not dissolve in water. Portfolio Evidence – (Lukas Chamberlain) Activity 3.1-3c: Precipitation Summary This experiment prepared silver chloride by a precipitation reaction between silver nitrate and sodium chloride. The silver chloride was filtered and the yield calculated.
The purpose for this lab was to use aluminum from a soda can to form a chemical compound known as hydrated potassium aluminum sulfate. In the lab aluminum waste were dissolved in KOH or potassium sulfide to form a complex alum. The solution was then filtered through gravity filtration to remove any solid material. 25 mLs of sulfuric acid was then added while gently boiling the solution resulting in crystals forming after cooling in an ice bath. The product was then collected and filter through vacuum filtration. Lastly, crystals were collected and weighed on a scale.
2-ethyl-1,3-hexanediol. The molecular weight of this compound is 146.2g/mol. It is converted into 2-ethyl-1-hydroxyhexan-3-one. This compounds molecular weight is 144.2g/mol. This gives a theoretical yield of .63 grams. My actual yield was .42 grams. Therefore, my percent yield was 67%. This was one of my highest yields yet. I felt that this was a good yield because part of this experiment is an equilibrium reaction. Hypochlorite must be used in excess to push the reaction to the right. Also, there were better ways to do this experiment where higher yields could have been produced. For example PCC could have been used. However, because of its toxic properties, its use is restricted. The purpose of this experiment was to determine which of the 3 compounds was formed from the starting material. The third compound was the oxidation of both alcohols. This could not have been my product because of the results of my IR. I had a broad large absorption is the range of 3200 to 3500 wavenumbers. This indicates the presence of an alcohol. If my compound had been fully oxidized then there would be no such alcohol present. Also, because of my IR, I know that my compound was one of the other 2 compounds because of the strong sharp absorption at 1705 wavenumbers. This indicates the presence of a carbonyl. Also, my 2,4-DNP test was positive. Therefore I had to prove which of the two compounds my final product was. The first was the oxidation of the primary alcohol, forming an aldehyde and a secondary alcohol. This could not have been my product because the Tollen’s test. My test was negative indicating no such aldehyde. Also, the textbook states that aldehydes show 2 characteristic absorption’s in the range of 2720-2820 wavenumbers. No such absorption’s were present in my sample. Therefore my final product was the oxidation of the secondary alcohol. My final product had a primary alcohol and a secondary ketone
Firstly, an amount of 40.90 g of NaCl was weighed using electronic balance (Adventurer™, Ohaus) and later was placed in a 500 ml beaker. Then, 6.05 g of Tris base, followed by 10.00 g of CTAB and 3.70 g of EDTA were added into the beaker. After that, 400 ml of sterilized distilled water, sdH2O was poured into the beaker to dissolve the substances. Then, the solution was stirred using the magnetic stirrer until the solution become crystal clear for about 3 hours on a hotplate stirrer (Lab Tech® LMS-1003). After the solution become clear, it was cool down to room temperature. Later, the solution was poured into 500 ml sterilized bottle. The bottle then was fully wrapped with aluminium foil to avoid from light. Next, 1 mL of 2-mercaptoethanol-β-mercapto was added into fully covered bottle. Lastly, the volume of the solution in the bottle was added with sdH2O until it reaches 500 ml. The bottle was labelled accordingly and was stored on chemical working bench.
A precipitation reaction can occur when two ionic compounds react and produce an insoluble solid. A precipitate is the result of this reaction. This experiment demonstrates how different compounds, react with each other; specifically relating to the solubility of the compounds involved. The independent variable, will be the changing of the various chemical solutions that were mixed in order to produce different results. Conversely the dependent variable will be the result of the independent variable, these include the precipitates formed, and the changes that can be observed after the experiment has been conducted. The controlled variable will be the measurement of ten droplets per test tube.
I knew that my non-metallic ion was Nitrate (NO3). I found this out after doing the precipitate test. I tested each known compound with silver nitrate as well as my unknown compound and found that it reacted by turning foggy, just like Sodium Nitrate. I saw in that formula that Nitrate was the non-metal since it was stated last, so I didn’t include Sodium.
Hydrochloric Acid, Sodium Thiosulphate Reaction. Research: What is the difference between Hydrochloric acid is a strong colourless acid formed when hydrogen chloride gas dissociates in water, used in industrial and laboratory. processes. The.
Salt is made up of sodium and chlorine and it is a natural occurrence on our planet, it can be found and harvested mainly from the seas, oceans or salt lakes. However salt can also be mined from within the earth from dried up underground seas, normally it’s only used as road salt (maldonsalt). The product salt has multiple functions, Salt is used to preserve foods and also to flavor foods, salt can also be used as a stabilizer in water and rock salt is used to melt ice during the winter (Freeman, 2007).
Electrical conductivity refers to a substances ability to carry moving electrons (conduct electricity). In order to do so, there must be a supply of delocalised electrons. While in a solid state, ionic substances can not conduct electricity as there are no delocalised electrons or free/mobile ions to act as charge carriers. In an aqueous ionic solution, the H2O molecules break apart the crystal lattice structure of the ionic substance into individual ions, surrounding each ion in a jacket of hydration. Below is the equation that describes the dissociation of NaCl when in H2O solvent.
The purpose of this lab to find if some certain compounds are made up of ionic or covalent bonds and to determine the properties of these compounds. This lab relates to the things we have been learning in class because compounds are part of our everyday life, so it’s nice to know some of the characteristics about it. In this lab we poured a small amount of the sample to a piece of labeled filter paper. To test the hardness, we separated a small amount of the sample and tried to crush it with the spatula. Next, we tested the conductivity of the sample by pouring each beaker with 30 mL of water. Then, Replace a paper clips on the edge of the beaker and if they were secure and partially under water. We then connected the wires to a battery and
2. Clean the surface of a 20 cm strip of magnesium ribbon using steel wool
Silver chloride is an ionic chemical compound with the chemical formula, AgCl. Silver chloride has a electronegativity of 1.4 and is known be rather, extremely low with regards to water solubility. It has a density if 5.56 gm/cm3, a melting point of 455 degrees and a boiling point of 1,547 degrees and the state of this compound is solid in room temperature. When heated, AgCl converts to silver and chlorine, which is evident by the greyish or purplish prominence of the compound.
2nd step heat the mixture: Make sure the agarose dissolves. Wait until it boils and when you are going to transfer the mixture, wear gloves to avoid getting burnt. Transfer the mixture into a removable gel tray.
In short, we can recall that the hypothesis is sodium chloride increases the swimming behavior of the Paramecium tertaurelia. Our |t-calculated|, as shown in Table 2, is less than the t-critical value from the table, therefore our averages for both the experimental group and control group are not significantly different enough, statistically speaking. As a result, our hypothesis is not supported. In this case, we accept the null hypothesis, which states that the sodium chloride has no effect on the swimming speed of the Paramecia tetraurelia and it is thus, supported. According to the results for the t-test, our t-calculated is less than the t-critical; therefore, we are less than 95% confident that the swimming speed increases. These results
1. The labels have fallen off of three bottles thought to contain hydrochloric acid, or sodium chloride solution, or sodium hydroxide solution. Describe a simple experiment which would allow you to determine which bottle contains which solution.
6. I then rinsed out the beaker and glass rod into the flask to make