From the moles of magnesium hydroxide (see attached), 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.) From the moles of acetic acid you used, how many moles of magnesium hydroxidewere in the sample of milk of magnesia that you reacted?0.001 In your experiment, you take 0.755 g of milk of magnesia and add some water and adrop of indicator dye. This is then neutralized with vinegar (which is a 5.0% aceticacid solution). It takes 2.25 mL of the vinegar to neutralize the milk of magnesia. Tofigure out the amount of Mg(OH)2 in the milk of magnesia (in that weird "how manymg of Mg(OH), are in 15 ml of milk of magnesia" unit.this unit is used because astandard 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 aceticacid you needed to neutralize the milk of magnesia. For this, you will need to use thedensity of the vinegar solution (1.02 g/mL), the concentration of acetic acid in thesolution (it is 5.0% by mass, which means there are 5.0 g of acetic acid for every 100 gof vinegar solution), and the molar mass of acetic acid (which is 60.052 g/mol). Howmany moles of acetic acid did you need?0.0019

Given, Moles of magnesium hydroxide = 0.001 mol Molar mass of magnesium hydroxide = 58.305 g/mol As…

Answered: calculate the grams of magnesium…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 93QRT: A soft drink contains an unknown mass of citric acid, C3H5O(COOH)3. It requires 6.42 mL of 9.580 ×...

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From the moles of magnesium hydroxide (see attached), 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.)

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?
0.001

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), 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

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