Nickel as a mineral does not normally occur in water systems. The water effluents from the steel and allied alloys, electro platting, paints, ceramics and food industry are largely the source of this contamination. Nickel is used in metallurgy of alloys, magnets, protective coating, catalysts, and batteries. The toxicity of nickel to aquatic life varies widely and is influenced by nickel compounds, pH, synergetic effects, and other factors. The average abundance of Ni in the earth’s crust is 1.2 ppm; in soils it is 2.5 ppm; in streams it is 1μg/L, and in groundwater it is <0.1 mg/L. Nickel is obtained chiefly from pyrrhotite and garnierite. The common aqueous species is Ni2+. In reducing conditions insoluble sulphide can form, while in aerobic …show more content…
1.00 ml 10 g Ni
(iii) Hydrochloric acid (L.R. grade) 1.0 N : Dilute 100 ml concentrated hydrochloric acid to 1000 ml with grade I distilled water.
(iv) Bromine water : Saturate distilled water with bromine to prepare Bromine water.
(v) Heptoximereagent : Dissolve 0.1 g 1,2 –cycloheptanedionedioxime (heptoxime) in 100 ml 95 % ethyl alcohol.
(vi) Sodium tartrate solution : Dissolve 10g sodium tartrate (Na2C4H4O6.2 H2O) in 90 ml distilled water.
(vii) Cupferronsolution : Dissolve 1 g cupferron in 100 ml distilled water. Store in refrigerator or prepare fresh for each series of determinations.
(viii) Hydroxylamine – Hydrochloride solution : Dissolve10 g NH2OH.HCl in 90 ml distilled water. This has to be prepared fresh.
Procedure :
(a) Preparation of calibration curve :(i) Pippet portions of standard NiSO4 solution into 100 ml volumetric flask. Use a series from 50 to 250 µg Ni. (ii) Add 25 ml 1.0 N HCl in 5 ml bromine water. (iii) Cool with cold running tap water and add 10 ml concentrated Ammonium hydroxide. (iv) Immediately add 20 ml heptoxime reagent. (v) Add 20 ml ethyl alcohol. (vi) Dilute to volume with distilled water and mix. (vii) Measure absorbance at 445 nm, 20 min after adding reagent, using a reagent blank as
…show more content…
(ii) Acidify to methyl orange end point with concentrated H2SO4. (iii) Add 5 ml concentrated HNO3. (iv) Add 2 ml 30% H2O2 . (v) Evaporate on a hot plate to 15 to 20 ml.
(vi) Transfer the concentrate and any precipitate to a 250 ml conical flask using 5 ml concentrated HNO3. (vii) Add 10 ml concentrated H2SO4 and a few boiling chips or glass beads. Evaporate on a hot plate in a hood until dense white fumes of SO3 just appear. (viii) If solution does not clear, add another 10 ml concentrated HNO3 and repeat the evaporation to obtain fumes of SO3. Remove all HNO3 before continuing treatment. All HNO3 will be removed when the solution is clear and no brownish fumes are evident. Do not let the sample dry during this digestion.
(ix) Cool and dilute to about 50 ml with water. Heat to almost boiling to dissolve soluble salts slowly. Filter if
While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved.
This is what I will mix with the varying amounts of Strontium nitrate to form the precipitate. • Strontium Nitrate (enough to fill 8 boiling tubes with your varying amounts/36cm³) This is what I will mix with the sodium carbonate in order to form my precipitate. • Test Tube Rack
The serial 2-fold dilution were done with a volumetric pipette, its pump, and 10 mL volumetric flasks. Eight different solutions were produced, half of which came from Red 40 and the other half, from Blue 1. These different concentrated solutions were placed in a 10 mL volumetric flask, each labelled with either R for Red 40
The anion tests followed the cation tests. To test for the presence of the chloride (Cl-) anion, a small scoop of the unknown compound was mixed with 1 mL of water in a test tube to create a solution. Then, 1 mL of 6 M nitric acid (HNO3) and 1 mL of silver nitrate (Ag(NO3)2) solution were added to the test tube to see if a white precipitate formed. To test for the presence of the sulfate (SO42-) anion, a small scoop of the unknown compound was mixed with 1 mL of water in a test tube to create a solution. Then, 1 mL of 6 M hydrochloric acid (HCl) and 1 mL of barium chloride (BaCl2) solution were added to the test tube to see if a white precipitate formed.
Some compounds have very distinctive colors when burned, such as Potassium, which is a white/purple, and sodium, which is a deep red hue. The first step for a flame test is to gather the needed materials. These include beakers, distilled water, the unknown substance, a Bunsen burner, matches, a nichrome wire, tubing to connect the gas line to the Bunsen burner, goggles, and known compounds to compare with. The first step is to make aqueous solutions of all the substances to be tested. This is done by adding .5
Using two test tubes, label one “s” for substrate and the other “e” for enzyme. The substrate tube should contain 7 mL of distilled water, 0.3 mL of hydrogen peroxide, and 0.2 mL guaiacol and the enzyme tube should contain 6 mL of distilled water and 1.5 mL of peroxidase. Combine the materials of the substrate and enzyme tubes, mix the two using a clean transfer pipette, transfer a portion into a cuvette so that the cuvette is about half-full then cover the top of the cuvette with Parafilm and then place it in the spectrophotometer and record absorbance. Remove the cuvette and repeat recording absorbance at 1, 2, 3, and 4 minutes. Be sure to mix the cuvette and clean its surface with Kimwipes before each reading.
In the round-bottom flask (100 mL), we placed p-aminobenzoic acid (1.2 g) and ethanol (12 mL). We swirled the mixture until the solid dissolved completely. We used Pasteur pipet to add concentrated sulfuric acid (1.0 mL) to the flask. We added boiling stone and assembled the reflux. Then, we did reflux for 75 minutes.
Chemical compounds that are available to determine are CaCO3, CaCl2, Ca(NO3)2, mgCl2, MgSO4, KCl, HCl, HC2H3O2, KNO3, K2SO4, NaC2H3O2, Na2CO3, NaCl, Na2SO4, HNO3, H2SO4, HNO3, H2SO4, NH4Cl, (NH4)2SO4, K2CO3, 0.1 M AgNO3, 0.2 M BaCl, Mg(s), NaOH, and KOH. To start this experiment, start with the flame test by gathering a Bunsen burner and a Nichrome wire. Connect the Bunsen burner with a rubber tube to a laboratory gas. To prepare solutions for the flame test, weigh out 0.205 gram of Unknown Compound using an analytical balance and mixed it into a 140 mL beaker filled with 20 mL ionized water. Ensure that solid is completely dissolved using a stirring rod.
Move 10 ml of the fourth well to the fifth well. FIll the fifth well with 90 ml of dh20 to reach 100ml. Start with 1% solution for Fluoride 100 ml and move 10ml of the first well into the next. Fill the well with 90ml dh20 to reach 100ml. move 10 ml of the second well to the third well.
Pat McGurrin October 24, 2015 Period #1 Honors Biology Mr. Dinunzio Murder and Meal Lab Analysis Procedure: 1.) Gather all materials: Safety goggles, 250ml beaker, water, hot-plate, test-tubes, paper bag tear, stomach contents, pipette, Biruet solution, Benedict’s solution, and Iodine solution. 2.) Put on safety glasses.
Next, a 100 mL graduated cylinder was used to measure 60 mL of distilled water. The water was added to the compound and stirred with a glass-stirring rod until dissolved. Next, The flame test required the solution made during the solubility test. The experiment needed a metal wire that was dipped into the solution
After (NH4)2CO3 was added to the basic solution, heat is applied to the test tube. It was then centrifuged and the liquid was discarded into a waste beaker. The precipitate was then washed with deionized water and centrifuged once again. Acetic acid was then added to the solid precipitate to dissolve it, resulting in a clear solution. Potassium chromate (K2CrO4) was added in step 12 because the chromate (CrO42-) ion and the unknown cation.
Acids are proton donors in chemical reactions which increase the number of hydrogen ions in a solution while bases are proton acceptors in reactions which reduce the number of hydrogen ions in a solution. Therefore, an acidic solution has more hydrogen ions than a basic solution; and basic solution has more hydroxide ions than an acidic solution. Acid substances taste sour. They have a pH lower than 7 and turns blue litmus paper into red. Meanwhile, bases are slippery and taste bitter.
Once dissolved, fill the rest of the volumetric flask up to the line on the neck of the flask. Again mix the solution. Use four, 10mL volumetric flask, and label them from 1-4. Add approximately 2mL of copper sulfate pentahydrate into flask 1, 4mL to flask 2,