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From the moles of magnesium hydroxide, calculate the grams of magnesium hydroxide this corresponds to (the molar mass of magnesium hydroxide is 58.305 g/mol) and then convert this to milligrams. This is how many mg of Mg(OH)2 are in the initial mass of milk of magnesia that you used. From this ratio (mg of Mg(OH)2 in grams of milk of magnesia), calculate how many mg of Mg(OH)2 are in a standard 15 mL dose of the milk of magnesia. (The density of milk of magnesia is 1.06 g/mL, use that to convert "15 mL" to units of grams.) 1,105

From the moles of magnesium hydroxide, calculate the grams of magnesium hydroxide this corresponds to (the molar mass of magnesium hydroxide is 58.305 g/mol) and then convert this to milligrams. This is how many mg of Mg(OH)2 are in the initial mass of milk of magnesia that you used. From this ratio (mg of Mg(OH)2 in grams of milk of magnesia), calculate how many mg of Mg(OH)2 are in a standard 15 mL dose of the milk of magnesia. (The density of milk of magnesia is 1.06 g/mL, use that to convert "15 mL" to units of grams.) 1,105

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Number 9 plz!!! I think you need info from 7 and 8 thats what i included them.

Question 7 There is a youtube video of this experiment listed in reference 18 of the paper. Have a look at the video for how the experiment is done. He also demonstrates the math but I dislike how he does it because his calculations are just based on crossing out units and ignoring the chemistry going on. So we will break this calculation down into steps. In your experiment, you take 0.755 g of milk of magnesia and add some water and a drop of indicator dye. This is then neutralized with vinegar (which is a 5.0% acetic acid solution). It takes 2.25 mL of the vinegar to neutralize the milk of magnesia. To figure out the amount of Mg(OH)2 in the milk of magnesia (in that weird "how many mg of Mg(OH)2 are in 15 mL of milk of magnesia" unit.this unit is used because a standard dose of this medicine is 15 mL), work out the following: From the volume of vinegar you used, you can figure out how many moles of acetic acid you needed to neutralize the milk of magnesia. For this, you will need to use the density of the vinegar solution (1.02 g/mL), the concentration of acetic acid in the solution (it is 5.0% by mass, which means there are 5.0 g of acetic acid for every 100 g of vinegar solution), and the molar mass of acetic acid (which is 60.052 g/mol). How many moles of acetic acid did you need? 0.0019
Transcribed Image Text:Question 7 There is a youtube video of this experiment listed in reference 18 of the paper. Have a look at the video for how the experiment is done. He also demonstrates the math but I dislike how he does it because his calculations are just based on crossing out units and ignoring the chemistry going on. So we will break this calculation down into steps. In your experiment, you take 0.755 g of milk of magnesia and add some water and a drop of indicator dye. This is then neutralized with vinegar (which is a 5.0% acetic acid solution). It takes 2.25 mL of the vinegar to neutralize the milk of magnesia. To figure out the amount of Mg(OH)2 in the milk of magnesia (in that weird "how many mg of Mg(OH)2 are in 15 mL of milk of magnesia" unit.this unit is used because a standard dose of this medicine is 15 mL), work out the following: From the volume of vinegar you used, you can figure out how many moles of acetic acid you needed to neutralize the milk of magnesia. For this, you will need to use the density of the vinegar solution (1.02 g/mL), the concentration of acetic acid in the solution (it is 5.0% by mass, which means there are 5.0 g of acetic acid for every 100 g of vinegar solution), and the molar mass of acetic acid (which is 60.052 g/mol). How many moles of acetic acid did you need? 0.0019
Question 8 From the moles of acetic acid you used, how many moles of magnesium hydroxide were in the sample of milk of magnesia that you reacted? 0.0009 Incorrect Question 9 From the moles of magnesium hydroxide, calculate the grams of magnesium hydroxide this corresponds to (the molar mass of magnesium hydroxide is 58.305 g/mol) and then convert this to milligrams. This is how many mg of Mg(OH)2 are in the initial mass of milk of magnesia that you used. From this ratio (mg of Mg(OH)2 in grams of milk of magnesia), calculate how many mg of Mg(OH)2 are in a standard 15 mL dose of the milk of magnesia. (The density of milk of magnesia is 1.06 g/mL, use that to convert "15 mL" to units of grams.) 1,105
Transcribed Image Text:Question 8 From the moles of acetic acid you used, how many moles of magnesium hydroxide were in the sample of milk of magnesia that you reacted? 0.0009 Incorrect Question 9 From the moles of magnesium hydroxide, calculate the grams of magnesium hydroxide this corresponds to (the molar mass of magnesium hydroxide is 58.305 g/mol) and then convert this to milligrams. This is how many mg of Mg(OH)2 are in the initial mass of milk of magnesia that you used. From this ratio (mg of Mg(OH)2 in grams of milk of magnesia), calculate how many mg of Mg(OH)2 are in a standard 15 mL dose of the milk of magnesia. (The density of milk of magnesia is 1.06 g/mL, use that to convert "15 mL" to units of grams.) 1,105
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