(Submit your answers on a separate sheet if necessary.) 1. If some of your unknown sample failed to dissolve completely, would the value of the molecular weight you calculated be too high, too low, or unaffected? Explain fully. 2. What would be the effect on the experimentally determined molecular weight if your sample contained a soluble impurity of higher molecular weight than the pure sample? Explain. . What would be the effect on the observed molecular weight if your unknown sample contained : insoluble impurity of lower molecular weigh than the pure sample? Explain.

In extraction process, the solution contains mixture of benzoic acid and sodium chloride and was heated with tap water, chloroform was added in the separatory funnel. Why is it not possible to use alcohol instead of chloroform in this procedure?

1.) While performing the Dumas experiment, if the outside of the flask were not completely dry (Part I), how would this affect the calculated molar mass of the unknown volatile liquid? Would it be higher or lower? Explain.  2.) While determining the pressure during the Dumas experiment, if the barometric pressure reported were lower than the actual vapor pressure (Part I), how would this error affect the calculated molar mass of the unknown volatile liquid? Explain. 3.) While determining the volume during this experiment (Part II), if the total volume of the flask were incorrectly reported as 125 mL, how would this error affect the calculated molar mass of the unknown volatile liquid? Explain. 4.) Calculate the number of moles of Argon gas contained in a 4.00 dm3 container at 620. kPa and 25.0 oC. If the gas is Helium instead of Argon, will the answer change? Explain.  5.) In the Dumas method for determining the molar mass of an unknown volatile liquid, a sample of a volatile liquid…

A student forgot to add the mass of the unknown solute in trial 1 to the mass of the solute that was weighed for trial 2 and then added to the cyclohexane-solute solution used in trial 1. How would this omission affect the calculated molecular weight of the solute?

What would have been the effect on the formula weight you calculated for your unknown If the unknown was still bubbling when you filtered your product?

3 Draw a flow chart to shows the strategy for separation of three compounds: Phenanthrene and 4-Aminoacetophenone and 1,4-Dibromobenzen and dissolve mixture is Diethyl ether. add NaOH (1M) and (6M) to the aqueous layer and ether layer..

Briefly explain how you determined when the reaction was complete PROCEDURETo a six inch test tube was added thiamine hydrochloride (0.65 g), followed by water (2mL). The mixture was gently shaken until homogeneous, and then ethanol (7.5 mL)was added. Finally, sodium hydroxide (10%, 1.5 mL) was added and the mixture wasgently stirred to ensure complete mixing.Benzaldehyde (3.8 mL) was then added at room temperature in one portion with gentlestirring. The pH of the resulting reaction mixture was determined and adjusted to >10by dropwise addition of 10% sodium hydroxide. The reaction mixture was then partiallysubmerged in a 65 °C water bath2 and the progress of the reaction was periodicallymonitored by TLC analysis.Once TLC analysis indicated that the reaction was complete, the reaction mixture wascooled to approximately room temperature, and then chilled in an ice-water bath. Theresulting precipitate was collected by vacuum filtration and air-dried. The crude productwas purified by…

How would each of the following errors affect the experimental value of your molarity of acetic? Would your Molarity value be too high, too low, or unaffected? Explain your answer. if you titrated your acid sample to a bright pink rather than faint pink endpoint? if your "acetic acid" burette was still wet inside with deionized water when you filled it with acetic acid? if you recorded the final volume of NaOH as "39.88 mL" instead of "38.88 mL"?

Organic Chemistry, column questions

Please help me answer these question  4. Does the pooling of results in this experiment yield an average % Mg in MgO, which is closer to the accepted value than your class average? 5. Compare the precision obtained by your class to the precision obtained by the composite of all classes. Discuss.  6. What conclusion can you draw from the analysis of the data in assessing whether this laboratory procedure gives accurate results?