White precipitate shows the presence of chloride (Cl-). Chloride anion equation: HCl(aq) + AgNO3 (aq) → HNO3 (aq) + AgCl(s). The nitrate anion test involves cooling a mixture containing 1 mL of test solution and 3mL 18M H2SO4. 2mL is poured down the inner test tube side and the presence of a brown ring shows nitrate (NO3-) to be present. The carbonate anion test mixes 1 mL of test solution and drops of 6M HCl.
Allow the mixture to cool for a few minutes then filter it, using either gravity or vacuum filtration. (We shall be using vacuum filtration.) Wash the residue in the funnel once with a little water and collect all the filtrate. 4. Pour all the filtrate and washings into a 250cm3 volumetric flask.
Gracen Seiler April 7th, 2015 Section- 109 Investigating Stoichiometry with Sodium Salts of Carbonic Acid Introduction- This experiment is intended to help find a better understanding of chemical stoichiometry through titrations of NaHCO3 and NA2CO3 with HCl. A chemical reaction is a process that involves rearrangement of the molecular or ionic structure of a substance, as opposed to a change in physical form in a nuclear reaction. Titration is when a measured amount of solution of unknown volume is added to a known volume of a second solution until the reaction between them is complete. The objective of this experiment is reacting sodium bicarbonate (NaHCO3) and sodium carbonate (NaCO3) with hydrochloric acid (HCl) to produce sodium chloride (NaCl), water (H20) and carbon dioxide (CO2). -Use the titrations of the following chemical reactions: NaHCO3 + HCl (aq) NaCl (aq) + H2O (l) + CO2 (g) 2HCl (aq) + Na2CO3 (s) 2NaCl (aq) + H2O (l) + CO2 (g) Experimental procedure- Two Erlenmeyer flask must be labeled “unknown 1 and unknown 2”.
For example, the reaction |BaCl2•2H2O ( BaCl2 + 2H2O |(2) | is reversible, and if water is added to the anhydrous salt BaCl2, formation of BaCl2•2H2O takes place: |BaCl2 + 2H2O ( BaCl2•2H2O |(3) | The reaction of dehydration of hydrated ferrous sulfate |FeSO4•7H2O ( FeSO4 + 7H2O |(4)
NaHCO3 (sodium bicarbonate - baking soda) and HCl (hydrochloric acid). The bubbles formed are carbon dioxide. HCl (hydrochloric acid) and BTB (bromothymol blue). Bromothymol blue is one of many acid-base indicators. What color do you observe?
17. Repeat Steps 12 through 16 above for well #2 and well #3 and record your data under the Trial 1 column in the Data Table 1. 18. Wash the well plate immediately with liquid soap and dry the well plate thoroughly with paper towel and cotton swabs to remove any precipitate from the bottom of
Experiment F: Dehydration of Cyclohexanol to Cyclohexene March 18, 2013 OBJECTIVES * Gain familiarity of dehydration mechanism and refractive index * Synthesize cyclohexene through dehydration of cyclohexanol by using phosphoric acid as catalyst * Grow in familiarity in reading IR spectra and data BALACED CHEMICAL EQUATION FOR THE DEHYDRATION C6H12O + H3O4P C6H10 + H2O TABLE OF PROPERTIES AND EQUIVALENTS NameCASChemical FormulaStructure | FW (g/mole) | BP/MP (° C) | Density (g/mL) | Refractive index | Molar amounts added (mol/L) | Limiting reagent | Hazards | Cyclohexanol108-93-0C6H12O | 100.16 | 161.125.15 | 0.96 | n20/D 1.465 | | Yes | Results in skin, respiratory tract and eye irritation; hazardous if swallowed |
Procedure 1. Begin to prepare an EDTA solution. Weigh out 3.62-3.64 g of NaH2EDTA and record exact mass. Add the weighed amount to a 250 ml volumetric funnel carefully using a funnel Wash the funnel with water to ensure all of the solid is delivered to the flask Add 100-200 ml of water and mix. Enough water should be added so that the flask is full to the 250 ml mark Tightly wrap the top of the flask with a Parafilm when finished 2.