Calculate the concentration of grams of sodium stearate per milliliter of diluted solution. To do this, multiply the concentration of sodium stearate in the dishwashing liquid by the dilution of the solution (1.50 mL dishwashing liquid per 100 mL solution). Answer = 1.5 *10^-4 g/mL 4. Calculate the number of moles of sodium stearate in a single layer. To do this, first take the number of drops used to achieve the monolayer (1 drop) and convert it to mL using the calibrated number of drops per mL.
5 drops of water and 5 drops of the calcium nitrate solution were pipetted for each well. For the second part of the experiment, 5 drops of 0.1 M sodium hydroxide were added to wells 1 through 6. The well plate was left for 5 minutes allowing the precipitates to form. Using Table 2 given in the lab manual, the solubility product was calculated and the experiment results were compared to the accepted values. For the third part of the experiment, the process of part 1 was repeated using sodium hydroxide.
The number of drops to equal 1Ml of NaOH is 17 drops. To reach the pH the 7, 2.4mL of NaOH was added to the solution. The volume of NaOH required to break the buffer is 2mL, and the concentration of NaOH was , calculate and report the number of moles of NaOH consumed by the buffer was .02. This is the buffer capacity of the acetate buffer to consume NaOH reaches 7.0.
5Fe3+(aq) + Mn2+(aq) + 4H2O(l) The above equation shows that one mole of manganate(VII) ions reacts with 5 moles of iron(II) ions in acid solution. Using our average
* 25 mL of distilled water was stirred in to form the calcium chloride solution. * Stoichiometry was used to determine how much Na2CO3 was needed for a full reaction. 1.0g CaCl2·2H2O(1mol CaCl2·2H2O/147g CaCl2·2H2O)(1mol Na2CO3/1mol CaCl2·2H2O)(106g Na2CO3/1mol Na2CO3)=0.72g Na2CO3 * The 0.7g of Na2CO3 was weighed and put in a small cup. * 25ml of distilled water was stirred in to make a sodium carbonate solution. * The sodium carbonate solution was poured into the beaker with the calcium chloride solution.
Experiment 3 Title: Fluid Properties: Density and Viscosity Date: 20th October 2011 Abstract: Introduction: Experimental Procedure: Five liquids were tested for Density measurements. These liquids included Vegetable oil, corn syrup, shampoo and glycerol. For viscosity measurement only three liquids were tested such as shampoo, glycerol and vegetable oil. Part I – Density Measurement The density of the test fluid was found by weighing a known volume of the liquid using the graduated cylinder. The cylinder was weighed empty, and then graduated cylinder was filled to a certain volume according to the graduations on it and weighed again.
In addition, place iodine in the dropping tile in order to identify if starch is currently present. 5. Repeat each experiment 3 times. Equipment: 1. Dropping Tile 2.
Using 1 ml micropipette add 1.0 MR in each four 10 ml volumetric flasks. 3. Prepare following MR solution in four flasks: flask 1: add 5 mL pH 4 buffer (graduated cylinder) and fill to the mark with water flask 2: add 5 mL pH 5 buffer and fill to the mark with water flask 3: add 5 mL pH 7 buffer and fill to the mark with water flask 4: add 1 mL 0.01M NaOH and fill to the mark with water. 4. Record the spectrum for these four solutions in range 400-700 nm.
MATERIALS/APPARATUS: Beaker- 50cm3 Volumetric Flask-250cm3 Conical Flask- Burette-50cm3 Pipette-25cm3 Diammonium Iron (ii) Sulphate 0.1M Sulphuric Acid 0.01M Potassium Manganate (vii) Beaker Digital Balance - 3. d.p METHOD: 5g of Diammonium iron (ii) sulphate is weighed and dissolved into 100cm3 of 0.1M Sulphuric Acid. The solution was then poured into a 250cm3 volumetric flask including all the washings. The solution, was then made up to the 250cm3 mark with distilled water. RESULTS: Table 1 The table above shows the titer value when Iron solution was titrated against potassium Manganate (vii). Calculation: The Equation for the reaction is: 5Fe2+ + MnO4- +8H+ → 5Fe3+ + Mn2+ + 4H2O 1.
In this experiment we had one common clay dispersed into 5 test tubes. Different solutions were then added to the test tubes to see how they reacted. The solutions used were KCL, NaCL, CaCL2, ALCl3, and distilled water. The order of floculation seen was as follows; most being AlC3, 2nd most was CaCl2, next was NaCl, then KCL, and no