1. How many grams of pure, solid NaOH are required to make 400 mL of 0.1M...

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1. How many grams of pure, solid NaOH are required to make 400 mL of 0.1M NaOH solution? 2. How many grams of a solution that is 50% by weight NaOH is required to make 400 mL of 0.1M NaOH solution? 3. The density of a 50% solution of NaOH is 1.525 g/mL. What volume of a solution that is 50% by weight NaOH is required to make 300 mL of 0.1M NaOH solution? 4. Why does weighing by difference eliminate systematic balance errors? 5. For each of your 3 acceptable trials (not the cursory one) in standardizing your NaOH against KHP, what are the mass in grams of KHP for each of the three samples to one thousandth of a gram, e.g. 0.507g? 6. What is the volume in mL of NaOH required to reach the endpoint for each of the KHP samples and enter the volume to a hundredth of a mL, e.g. 15.24 mL? 7. Calculate the values for each of your three trials for the molarity of your NaOH solution. Place your molarity entries in the order corresponding with the masses of KHP and the volumes of NaOH required for the trials. 8. Calculate the value for the average of the three trials determining the molarity of your NaOH solution. 9. Calculate the value for the standard deviation of the average molarity. 10. Calculate the value for the 90% confidence limits for the molarity of your NaOH solution. 11. Why does it not matter how much water you added when dissolving the acid or when carrying out the titration? 12. What was the brand name of your sample commercial vinegar solution? 13. What volume in mL did you use for each of the three acceptable trial samples of your vinegar analysis? 14. What was the volume of standardized NaOH solution that was required for each trial determining the amount of acetic acid in your commercial vinegar sample? 1. How many grams of pure, solid NaOH are required to make 400 mL of 0.1M NaOH solution? 2. How many grams of a solution that is 50% by weight NaOH is required to make 400 mL of 0.1M NaOH solution? 3. The density of a 50% solution of NaOH is 1.525 g/mL. What volume of a solution that is 50% by weight NaOH is required to make 300 mL of 0.1M NaOH solution? 4. Why does weighing by difference eliminate systematic balance errors? 5. For each of your 3 acceptable trials (not the cursory one) in standardizing your NaOH against KHP, what are the mass in grams of KHP for each of the three samples to one thousandth of a gram, e.g. 0.507g? 6. What is the volume in mL of NaOH required to reach the endpoint for each of the KHP samples and enter the volume to a hundredth of a mL, e.g. 15.24 mL? 7. Calculate the values for each of your three trials for the molarity of your NaOH solution. Place your molarity entries in the order corresponding with the masses of KHP and the volumes of NaOH required for the trials. 8. Calculate the value for the average of the three trials determining the molarity of your NaOH solution. 9. Calculate the value for the standard deviation of the average molarity. 10. Calculate the value for the 90% confidence limits for the molarity of your NaOH solution. 11. Why does it not matter how much water you added when dissolving the acid or when carrying out the titration? 12. What was the brand name of your sample commercial vinegar solution? 13. What volume in mL did you use for each of the three acceptable trial samples of your vinegar analysis? 14. What was the volume of standardized NaOH solution that was required for each trial determining the amount of acetic acid in your commercial vinegar sample?

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The detailed answer for the above question is provided below Answer 1 400 g 2 800 g 3 2000 mL 4 Weighing by difference eliminates systematic balance errors by taking into account the weight of the con... View the full answer