The active ingredient in some antiperspirants is aluminum chlorohydrate, Al2(OH)5Cl. Analysis of a 2.000-g sample of antiperspirant yields 0.334 g of aluminum. What percent (by mass) of aluminum chlorohydrate is present in the antiperspirant? (Assume that there are no other compounds containing aluminum in the antiperspirant.)
No. Anonymous has given the % Al in the compound.
g Al2(OH)5Cl = 0.334g Al x (molar mass Al2(OH)5Cl/atomic mass Al) = ?
Then % Al2(OH)5Cl = [g Al2(OH)5Cl/2.000)]*100 = ? and it is to 3 s.f. based on the 0.334 g Al.
To find the percent (by mass) of aluminum chlorohydrate in the antiperspirant, we need to calculate the mass of aluminum chlorohydrate from the given mass of aluminum and then calculate the percentage.
Step 1: Calculate the molar mass of aluminum chlorohydrate (Al2(OH)5Cl).
The molar mass of Al = 26.98 g/mol
The molar mass of O = 16.00 g/mol
The molar mass of H = 1.01 g/mol
The molar mass of Cl = 35.45 g/mol
Molar mass of Al2(OH)5Cl = (2 * Al) + (5 * H) + O + Cl
= (2 * 26.98 g/mol) + (5 * 1.01 g/mol) + 16.00 g/mol + 35.45 g/mol
= 133.97 g/mol
Step 2: Calculate the mass of aluminum chlorohydrate in the antiperspirant.
Given: Mass of aluminum = 0.334 g
To find the mass of aluminum chlorohydrate, we need to use the ratio of the molar mass of aluminum to the molar mass of aluminum chlorohydrate.
Mass of aluminum chlorohydrate = (Mass of aluminum / molar mass of Al) * molar mass of Al2(OH)5Cl
= (0.334 g / 26.98 g/mol) * 133.97 g/mol
= 1.652 g
Step 3: Calculate the percentage.
Now we can calculate the percentage of aluminum chlorohydrate in the antiperspirant.
Percent (by mass) of aluminum chlorohydrate = (Mass of aluminum chlorohydrate / mass of antiperspirant) * 100
= (1.652 g / 2.000 g) * 100
= 82.6% (rounded to one decimal place)
Therefore, the percent (by mass) of aluminum chlorohydrate present in the antiperspirant is approximately 82.6%.
To find the percent (by mass) of aluminum chlorohydrate in the antiperspirant, you can calculate the mass percent by using the formula:
Percent mass = (mass of aluminum chlorohydrate / mass of antiperspirant) x 100
First, we need to determine the mass of aluminum chlorohydrate in the antiperspirant. We are given that a 2.000 g sample of antiperspirant yields 0.334 g of aluminum.
Using the molar mass of aluminum (Al) and the molar mass of aluminum chlorohydrate (Al2(OH)5Cl), we can calculate the mass of aluminum chlorohydrate in the 0.334 g of aluminum obtained.
The molar mass of Al is 26.98 g/mol, and the molar mass of Al2(OH)5Cl is:
(2 x 26.98 g/mol) + (5 x 1.01 g/mol) + (1 x 35.45 g/mol) = 210.45 g/mol.
Now, we can calculate the mass of aluminum chlorohydrate:
Mass of aluminum chlorohydrate = (0.334 g Al) x (210.45 g/mol Al2(OH)5Cl) / (26.98 g/mol Al)
= 2.61 g.
Finally, we can calculate the percent mass of aluminum chlorohydrate in the antiperspirant:
Percent mass = (2.61 g / 2.000 g) x 100 = 130.5%.
Therefore, approximately 130.5% (by mass) of aluminum chlorohydrate is present in the antiperspirant.
Note that the result is greater than 100% because it represents the percent composition of aluminum chlorohydrate in the antiperspirant, not the overall composition of the antiperspirant.
(0.334g/2.000g)*100= ???
4-significant figures.