How would each of the following errors have affected the value of the molar mass? (For...
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How
would each of the following errors have affected the value of the
molar mass? (For...
1. A student performed a freezing point determination and calculated the molar mass of an unknown...
1. A student performed a freezing point determination and calculated the molar mass of an unknown like you did in this experiment. The only difference in procedure was that when determining the freezing point of the unknown-naphthalene mixture, they started with a clean empty test tube. If the following errors occurred, how would each affect the calculated molar mass of the solute (too high, too low, or no change)? Explain your answers. a. The thermometer used actually read 2.0 celcius...
7.How would the molar mass of the unknown acid be affected (higher, lower, or no change)...
7.How would the molar mass of the unknown acid be affected (higher, lower, or no change) if the follow-ing errors occurred? Briefly explain why in each case. a.The pH meter was incorrectly calibrated to read lower than the actual pH. b.During the titration, several drops of NaOH missed the reaction beaker and fell onto the bench top. c.In Part B of the procedure the acid was dissolved in 75 mL of distilled water rather than the 50 mL called for...
explain how would the calculated value of molar mass be affected if the temperature was assumed...
explain how would the calculated value of molar mass be
affected if the temperature was assumed to be 100 when it was
actually was only 90 Celcius
Experiment 8 Questions. 1. Explain how would the calculated value of the molar mass be affected (too high, too low, no effect) if: a) the flask had been left in the water bath for so long that after all the liquid vaporized, some of the vapor escaped and was replaced by air? less...
How would the calculated molar mass change (increase,decrease, no change) if the following experimental problems were...
How would the calculated molar mass change (increase,decrease, no change) if the following experimental problems were encountered? Explain the reason(s) for your answer. a) The unknown was impure and only part of the unknown dissolved in the lauric acid. b) Your unknown contained a substance which produced two ions per molecule of unknown when dissolved in the lauric acid. c) The unknown was insoluble in lauric acid. d) A very small amount of lauric acid was spilled after weighing, but...
Molecular Mass by Freezing point Depression (Preliminary Lab) The following errors occurred when the above experiment was carried out
Molecular Mass by Freezing point Depression (Preliminary Lab) The following errors occurred when the above experiment was carried out. How would each affect the calculated molecular mass of the solute (too high,too low, no effect)? Explain your answer. (a) The thermometer uses actually read 1.4C too high. (b) Some of the solvent was spilled before the solute was added.
Date Name Lab Section Partner(s) Determination of Molar Mass by Freezing Point Depression Data: Mass of...
Date Name Lab Section Partner(s) Determination of Molar Mass by Freezing Point Depression Data: Mass of empty test tube 2.2.6! Mass of test tube plus approximately 10.0 g of benzophenone 33.39 The difference is the mass of benzophenone (solvent) 8 kg Mass of unknown (-1.0 g) 1:09: 48.50°c 42.08. Freezing point of pure benzophenone Freezing point of benzophenone containing the unknown The difference is A fp CO Calculations: (Show set-up with cancellation of units) 1. molality of solution 2. moles...
For each of the following errors, tell whether your calculated molecular weight would be too high,...
For each of the following errors, tell whether your calculated molecular weight would be too high, too low, or unaffected. a) unawares, you inadvertently spilled some solute(so it didn't make it into the test tube) after it was weighed out. b) your thermometer is poorly calibrated and reads 0.3C lower than the actual temperature. c) while mixing the solution you spilled some over the sides of the test tube. Assume the solution was well mixed before the spill occurred.
7. For each of the following experimental or calculation errors, tell if the calculated value of...
7. For each of the following experimental or calculation errors, tell if the calculated value of R, in question 4, would be too high, too low or unchanged. Explain your answers. a. The temperature of the water was recorded too low. b. The mass of the magnesium was recorded too high. c. The magnesium was coated with magnesium oxide. d. Some air bubbles were introduced when the eudiometer was inverted. Some of the hydrogen gas dissolved in the water. (Hint:...
THE MOLAR MASS OF A VOLATILE LIQUID 1. A foil-covered flask was found to have a...
THE MOLAR MASS OF A VOLATILE LIQUID 1. A foil-covered flask was found to have a mass of 161.38 have a mass of 167.38 g. A volatile liquid was placed L00.0°C at a barometric pressure of 743.8 mm Hg. The foil-covered inside and heated to 100.0°C at a barometric press flask containing the vapor had a mass the molar mass of this volatile liquid. 's the vapor had a mass of 167.71 g and a volume of 147.0 mL. Calculate...
Indicate how each of the following would affect the value of the absorbance (too high, too low, or not effect) of the indicated solution
Indicate how each of the following would affect the value of the absorbance (too high, too low, or not effect) of the indicated solution. I really need help. I do not understand these questions! This is from a chemistry activity to determine the unknown concentration of an Erythrosin B solution by using a spectrophotometer. a. A student prepares solution A as instructed and pours it into a wet beaker. b. A student rinses the 10.00 mL pipet only with DI...
explain how would the calculated value of molar mass be
affected if the temperature was assumed to be 100 when it was
actually was only 90 Celcius
Experiment 8 Questions. 1. Explain how would the calculated value of the molar mass be affected (too high, too low, no effect) if: a) the flask had been left in the water bath for so long that after all the liquid vaporized, some of the vapor escaped and was replaced by air? less...
Date Name Lab Section Partner(s) Determination of Molar Mass by Freezing Point Depression Data: Mass of empty test tube 2.2.6! Mass of test tube plus approximately 10.0 g of benzophenone 33.39 The difference is the mass of benzophenone (solvent) 8 kg Mass of unknown (-1.0 g) 1:09: 48.50°c 42.08. Freezing point of pure benzophenone Freezing point of benzophenone containing the unknown The difference is A fp CO Calculations: (Show set-up with cancellation of units) 1. molality of solution 2. moles...
7. For each of the following experimental or calculation errors, tell if the calculated value of R, in question 4, would be too high, too low or unchanged. Explain your answers. a. The temperature of the water was recorded too low. b. The mass of the magnesium was recorded too high. c. The magnesium was coated with magnesium oxide. d. Some air bubbles were introduced when the eudiometer was inverted. Some of the hydrogen gas dissolved in the water. (Hint:...
THE MOLAR MASS OF A VOLATILE LIQUID 1. A foil-covered flask was found to have a mass of 161.38 have a mass of 167.38 g. A volatile liquid was placed L00.0°C at a barometric pressure of 743.8 mm Hg. The foil-covered inside and heated to 100.0°C at a barometric press flask containing the vapor had a mass the molar mass of this volatile liquid. 's the vapor had a mass of 167.71 g and a volume of 147.0 mL. Calculate...
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