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19 Nov 2019
Please help with these lab calculations I am so confused what to do.
Calculations: 1. The NaOH solution you used was made by diluting 8.000 g of Using the calculated results from your 3 flasks 7. Calculate an average weight percent of H3CCOOH in vinegar. 8. Calculate a standard deviation for the weight percent of 50 wt% NaOH to a final volume of 1.00 L. Calculate the molarity of this NaOH solution (MNaoH). Make sure the molar mass of NaOH that you use in your calculation has 5 significant figures. (Hint: 50 wt% NaOH means that half of the solution is NaOH and the other half is water.) H3CCOOH in vinegar. 9. Create a Results Table summarizing the calculated weight percent of H3CCOOH in vinegar for each of the 3 flasks, the average value and the standard deviation. Add a title to your Results Table (it can't be "Results") Discussion: Begin your discussion with a brief summary of the experiment. Present your calculated weight percent of acetic acid (H3CCOOH) in vinegar. Compare your results to the stated weight percent of H3 2. Calculate the number of moles of NaOH used in the titration: moles NaOH = VNaOH x MNaOH 3. Calculate the number of moles of HaCCOOH present in 2.00 mL of vinegar: moles HsCCOOH = moles NaOH used in titration 4. Convert the moles of H3CCOOH to a mass of H3CCOOH. Figure 9.1 Photo of a Vinegar Bottle Distiieu vvIte 5. Recall that you used 2.00 mL of vinegar. Calculate the mass of 2.00 mL of vinegar. Use a vinegar density of 1.000 g/mL. Vinegar mass vinegar = V/vinegar à 1.000 g/mL ALL NATURAL 5% ACIDITY 6. Calculate the weight percent of HsCCOOH in vinegar: weight 90 HsCCOOH-mass HsCCOOH/mass vinegar à 100%
Please help with these lab calculations I am so confused what to do.
Calculations: 1. The NaOH solution you used was made by diluting 8.000 g of Using the calculated results from your 3 flasks 7. Calculate an average weight percent of H3CCOOH in vinegar. 8. Calculate a standard deviation for the weight percent of 50 wt% NaOH to a final volume of 1.00 L. Calculate the molarity of this NaOH solution (MNaoH). Make sure the molar mass of NaOH that you use in your calculation has 5 significant figures. (Hint: 50 wt% NaOH means that half of the solution is NaOH and the other half is water.) H3CCOOH in vinegar. 9. Create a Results Table summarizing the calculated weight percent of H3CCOOH in vinegar for each of the 3 flasks, the average value and the standard deviation. Add a title to your Results Table (it can't be "Results") Discussion: Begin your discussion with a brief summary of the experiment. Present your calculated weight percent of acetic acid (H3CCOOH) in vinegar. Compare your results to the stated weight percent of H3 2. Calculate the number of moles of NaOH used in the titration: moles NaOH = VNaOH x MNaOH 3. Calculate the number of moles of HaCCOOH present in 2.00 mL of vinegar: moles HsCCOOH = moles NaOH used in titration 4. Convert the moles of H3CCOOH to a mass of H3CCOOH. Figure 9.1 Photo of a Vinegar Bottle Distiieu vvIte 5. Recall that you used 2.00 mL of vinegar. Calculate the mass of 2.00 mL of vinegar. Use a vinegar density of 1.000 g/mL. Vinegar mass vinegar = V/vinegar à 1.000 g/mL ALL NATURAL 5% ACIDITY 6. Calculate the weight percent of HsCCOOH in vinegar: weight 90 HsCCOOH-mass HsCCOOH/mass vinegar à 100%
Collen VonLv2
4 Nov 2019