It is emphasized in the procedure that the water bath should be continuously stirred while heating and cooling the sample. What will happen if the water bath was not stirred? Identify its effect to the related derived data
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- 5.Provide two reasons that the observed boiling point of a pure liquid isolated during a fractionaldistillation may be lower than the literature value.Be specific.The density of the first fraction collected would be expected to be close to a value of ______. 1.00 g./mL 0.895 g/mL 0.789 mL 0.950 g.mLA student doing this experiment had some problems with the procedure, as described below. Explain what effect each problem would have had on the magnitude of the results calculated. b) The student neglected to open the pinch clamp on the plastic tubing between the filter flask and the beaker when the Mg came in contact with the HCl solution. After the stopper popped out of the Erlenmeyer flask, the student quickly replaced the stopper, opened the clamp, and proceeded with the experiment. c) The student began titrating the unreacted HCl with standard NaOH solution and realized that there was a large air bubble in the buret tip. The bubble came out as the first few milliliters of titrant were added. d) The student forgot to add indicator to the titration mixture until 12.50 mL of titrant had been added. When the indicator was finally added, the solution was colorless.
- Acetone and isopropyl alcohol are generally not suitable for use in extraction, but are frequently used as recrystallization solvents. ExplainA student doing this experiment had some problems with the procedure, as described below. Explain what effect each problem would have had on the magnitude of the results calculated. a) The vial containing the Mg tipped over when the student first placed it in the Erlenmeyer flask. The student was able to return it to an upright position almost immediately, and the student continued the experiment. b) The student neglected to open the pinch clamp on the plastic tubing between the filter flask and the beaker when the Mg came in contact with the HCl solution. After the stopper popped out of the Erlenmeyer flask, the student quickly replaced the stopper, opened the clamp, and proceeded with the experiment. c) The student began titrating the unreacted HCl with standard NaOH solution and realized that there was a large air bubble in the buret tip. The bubble came out as the first few milliliters of titrant were added. d) The student forgot to add indicator to the titration mixture until…During heating, some solution of NaCl splattered out of the evaporating dish. How would this affect the calculated percentage of mixture recovered upon separation?
- What could have gone wrong in the separation and purification process to result in the disparity from the observed and expected yields? Select all that apply A) Both the benzoic acid and sand may have been wet before the student recorded the masses, hence the increase in expected masses. B) The student may have filtered the benzoic acid while cold. Hence the sand could have been contaminated with benzoic acid and resulted in a higher mass for sand. C) The sand may have dissolved in the hot water along with the benzoic acid, hence, the recorded mass for benzoic acid was more. D)The benzoic acid may have been cooled down too quickly on ice thereby allowing other soluble impurities to crystallize with benzoic acid causing the increase in the expected massDetermination of melting point can also be done by heating melting point capillary to the thermometer using “Thiele tube”. Draw a complete Thiele tube melting point apparatus. What effect would poor circulation of the melting point bath liquid have on the observed melting point?1. The entire mercury bulb of the thermometer must be below the level of the side arm in order to obtain an accurate reading of the distillation temperature. Why is this so?2. Why is cold water circulated through the condenser from the bottom rather than from the top?4. In most distillations, the total volume of liquid obtained (distillate + residue) is not equal to the volume of the mixture introduced into the flask. What are the possible sources of loss in this procedure?
- The entire mercury bulb of the thermometer must be below the level of the side – arm in order to obtain an accurate reading of the distillation temperature. Why is this so?If insoluble impurities eg. dust, tissues, filter paper etc were mixed with the sample how will these affect the measured melting pointDraw the structure of benzoic acid and look up for its literature melting point? Please answer very soon will give rating surely