(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.
One of the reactions you observed resulted in this product: NaCl + H2O + CO2 (g)? What well did this reaction occur in? Describe how the observations for this reaction support your answer. B BoldI ItalicsU Underline Bulleted list Numbered list Superscript Subscript70 Words A reaction I observed in number 1.) Sodium Bicarbonate mixed with Hydrochloric acid.
Cool the filtrate to room temperature, add 1.5 g of sodium nitrite, and stir until reaction is complete. 5. Pour this mixture, while stirring, into a beaker containing 25 mL of ice water to which 5 mL of concentrated hydrochloric acid have been added. The diazonium salt of sulfanilic acid should soon separate as a finely divided white precipitate. Keep this suspension cooled in an ice bath until it is to be used.
7- Once finished turn the Bunsen burner to a safety flame and turn off the gas Materials- precipitates test In this experiment you will need: -Test tubes -Test rack -Unknown solution A -Unknown solution B -Silver Nitrate -Safety goggles -Barium chloride Method- precipitates test The method to this experiment is: 1- Gather your materials 2- Put on your safety goggles 3- Get unknown solution A and pour centimeter into a test tube 4- Add a centimeter of silver nitrate into unknown solution A 5- Observe the reaction and record your notes 6- Pour a centimeter of unknown solution B into another test tube 7- Add a centimeter of silver nitrate into unknown solution B 8- Observe the reaction and record your notes 9- Do the same with barium chloride and observe the reaction 10- Pour out the contents in the test tubes and wash them out 11- Pack up your materials Results-Flame test Cation Flame Test A= Calcium Vibrant orange color with a hint of yellow Calcium B=Copper Forest green color with a hint of orange Copper Results- Precipitate Test- Anion Halide Test (Silver Nitrate) Sulfate Test (Barium Chloride) Unknown A Turned cloud white color, has a quick reaction, sediment on the top Clear solution with a white stringy bits floating
Eventually using the NaOH and the acid’s consumed moles, the equivalent mass will be determined. Procedure: Part 2: Obtain 45mL of NaOH, and then weigh 0.3-0.4g of the unknown acid (KH2PO4). Dissolve the acid into 20.00mL water. Record the buret readings, and slowly titrate the NaOH into
0.5 grams of NaCl was added, stirred and filtered. The residue was washed with 2M HCl until the volume of the filtrate became 6mL. 1mL of the filtrate was tested with 2-3 drops of Mayer’s reagent, Wagner’s reagent and Draggendorrf’s reagent. The relative amount of precipitation was observed: (+ Slight turbidity), (++ Definite turbidity), (+++ Heavy turbidity). 3.2 Alkaloidal Analysis
During this period, reflux was observed, and the mixture appeared dark brown in color. To quench the reaction, the reaction mixture was transferred onto ice. NaOH was slowly added into the mixture, which resulted in acetic acid byproduct from the acetic anhydride reactant/solvent. This resulted in a clumpy and dark mixture. During
The compound’s empirical formula was determined to be FeK3(C2O4)3•3H2O. With the molecular formula and the balanced equation for the synthesis of potassium trioxalatoferrate (III) trihydrate, stoichiometry revealed potassium oxalate monohydrate was the limiting reactant. The theoretical yield of 6 grams of potassium oxalate monohydrate was
Sodium carbonate (molecular formula: Na2CO3), is the water soluble sodium salt of carbonate. The pure product appears as a while, odorless powder with a strong alkaline taste. It has high hygroscopicity. It can be easily dissolved in water to form an aqueous solution with moderate alkalinity Sodium bicarbonate (IUPAC name: sodium hydrogen carbonate) is chemical compound with the formula NaHCO3. It is a salt composed of sodium ions and bicarbonate ions.
The burette is attached to a laboratory stand with 2 clamps. The burette is first rinsed with 0.1M NaOH and then it is filled with it a bit above the 0.00 mL mark. NaOH is drained from the burette so that there are not bubbles in the tip and so that the NaOH reaches exactly the 0.00 mL level. Dispose of the waste NaOH solution that was drained. 50 mL of distilled water is added to the 250 mL beaker and 10 mL of HCl is pipetted into the beaker.