One of the most popular pool disinfectants is the element chlorine, in the form of the chemical compound calcium hypochlorite (an ionic solid). Which would dissolve more calcium nypochlorite: a hot swimming pool or a cold swimming pool? Justify your answer "More calcium hypochlorite will dissolve in the (hot or cold) swimming pool because 11

One of the most popular pool disinfectants is the element chlorine, in the form of the chemical compound calcium hypochlorite (an ionic solid). Which would dissolve more calcium nypochlorite: a hot swimming pool or a cold swimming pool? Justify your answer "More calcium hypochlorite will dissolve in the (hot or cold) swimming pool because 11

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter14: Chromatography

Section: Chapter Questions

Problem 9P

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A stock solution of 75% v/v ethanol was diluted with distilled water to prepare 1L of 42% v/v ethanol. (Density of ethanol = 0.789 g/mL; MW of ethanol = 46 g/mol). Determine the initial volume (in mL) of 75% v/v ethanol used in the preparation. Final answer should NOT contain any unit. Type the VALUE only. Please observe 0 decimal places.
The mass of a beaker is 5.333g. After 5.00mL of a concentrated hydrochloric acid solution is pipetted into the beaker, the combined mass of the beaker and the hydrochloric acid sample is 11.229g. From the data, what is the measured density of the hydrochloric acid solution?
Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.
50 mg of granular salt is briefly stirred into a glass container of 1/5 liter volume filled with water. After briefly mixing, some salt is still seen at the bottom of the class. The visible salt is filtered from the water, weighed and determined to have a mass of 20 mg. What is the dissolved phase concentration of salt remaining in the water? Provide your answer to the nearest whole number in units of mg/l.
The %purity of a powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. a. How many moles of CO2 were collected? b. What is the percent purity of the sample? Round off to the nearest whole number
The %purity of a powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. What CASE does this experiment satisfy?
What is the molarity of a concentrated solution of sulfuric acid with a specific gravity of 1.84 and 95.0% by weight sulfuric acid? specific gravity = density of substance at certain temp/density of water at 4 degrees C the density of water is 0.999973 g/mL at 4 degrees celsius. Describe how to prepare 3.0 L of 0.100M. I will pipet ______ and add this to 200mL water. The solution will be stirred and diluted to 3L with water.
How would you prepare 75 mL of an H2SO4 solution at 20% in weight (density=1.1394 g/mL, richness=227.9 g/L) starting from the commercial H2SO4 solution (98%, density=1.8361 g/mL, richness=1799 g/L)? Please choose among the most appropriate procedure which better describes the preparation of the previous diluted H2SO4 solution: Select one or more: a. Take the required volume of commercial H2SO4 solution with an adequate pipette, pour it into a graduated flask and add water up to the final volume (75 mL in this case). Homogenize the flask by stirring it gently. b. Take a beaker and put about 40 mL of distilled water. Then take the required volume of commercial H2SO4 solution with an adequate pipette and pour them over the beaker. Let the solution be warm and pour the mixture into a graduated flask and add water up to the final volume (75 mL in this case). Homogenize the flask by stirring it gently. c. Take a beaker and put about 40 mL of distilled water. Then take the required volume…
A powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr.What is the %purity of the sample to the nearest whole number?
There's 1 drink (and you are asked to determine the glucose concentration in the drink in the units of g/100mL. (Why these units? Well, once you have the concentrations in g/100mL you will be able to compare your values with the nutritional values given on the drink bottles’ labels). The sample of the drink was diluted 1/100 (i.e. by a factor of 100). This was an essential step in the method because, without it, the machine used to analyse the glucose concentration (spectrophotometer) would have given an error as the concentration would have been too high for accurate detection. What this means for you is that the dilution factor will need to be taken into consideration in your calculations (remember the aim is to calculate the concentration in the original drink and not in the diluted drink). You measured the concentration of their diluted drink using the spectrophotometer and their results were provided to them in the units mM (millimolar). Glucose Concentration in mM of drink =…
There's 1 drink (and you are asked to determine the glucose concentration in the drink in the units of g/100mL. (Why these units? Well, once you have the concentrations in g/100mL you will be able to compare your values with the nutritional values given on the drink bottles’ labels). The sample of the drink was diluted 1/100 (i.e. by a factor of 100). This was an essential step in the method because, without it, the machine used to analyse the glucose concentration (spectrophotometer) would have given an error as the concentration would have been too high for accurate detection. What this means for you is that the dilution factor will need to be taken into consideration in your calculations (remember the aim is to calculate the concentration in the original drink and not in the diluted drink). You measured the concentration of their diluted drink using the spectrophotometer and their results were provided to them in the units mM (millimolar). Glucose Concentration in mM of drink =…