a chemist needs to order Na2B4O7. One supplier offers it in an anhydrous (without water) form, while another offers it as a hydrated crystal, Na2B4O7*10H20. if the prices from the two suppliers are the same for a 500.0-g bottle, which one would supply more of the desired Na2B4O7. explain.
please help !
So 500 g Na2B4O7 = 100.00
and 500 g Na2BrO7.10H2O = 100.00
Wouldn't it appear that the second one you are paying for water + Na2B4O7 while in the first one you are getting ALL Na2B4O7 without the water.
Well, it seems like our chemist friend is in a bit of a pickle. Choosing between anhydrous and hydrated forms of Na2B4O7 can be quite a challenge. But fear not, because Clown Bot is here to add a little laughter and help our chemist friend out!
Let's break it down, shall we?
The hydrated crystal form is Na2B4O7*10H2O. This means that for every molecule of Na2B4O7, there are ten molecules of water attached. Now, you might be thinking, "Great, more water means more bang for your buck, right?" Well, not quite.
When you purchase Na2B4O7 in the hydrated form, you're mostly paying for those ten molecules of water. The water molecules add extra weight to the compound, but they don't contribute to the amount of Na2B4O7 you actually need for your experiments.
On the other hand, the anhydrous form means it's "water-free" or without water. So, in a 500.0-g bottle, you will get 500 grams of pure Na2B4O7 without any extra water molecules. This means you'll have more of the desired compound to work with compared to the hydrated crystal form, where a significant portion of the weight comes from water.
So, to answer your question, if the prices from the two suppliers are the same for a 500.0-g bottle, the anhydrous form would supply more of the desired Na2B4O7. It's like getting a full bag of chips instead of a bag with only a few chips and a lot of air.
I hope this explanation brought a smile to your face and helped clarify the question for you. If you have any more chemistry mysteries or any inquiries about anything under the sun (or beyond it), feel free to ask Clown Bot!
To determine which option would supply more of the desired Na2B4O7, we need to consider the molecular weights and water content of the two forms of Na2B4O7.
1. Anhydrous form: Na2B4O7 (without water)
The molecular weight of Na2B4O7 is:
- Sodium (Na): 22.99 g/mol x 2 = 45.98 g/mol
- Boron (B): 10.81 g/mol x 4 = 43.24 g/mol
- Oxygen (O): 16.00 g/mol x 7 = 112.00 g/mol
Total molecular weight of Na2B4O7: 45.98 + 43.24 + 112.00 = 201.22 g/mol
2. Hydrated crystal form: Na2B4O7*10H2O (with water)
The molecular weight of Na2B4O7 is the same as in the anhydrous form: 201.22 g/mol.
In addition to this, we need to consider the molecular weight of water (H2O):
- Hydrogen (H): 1.01 g/mol x 2 = 2.02 g/mol
- Oxygen (O): 16.00 g/mol x 1 = 16.00 g/mol
Total molecular weight of H2O: 2.02 + 16.00 = 18.02 g/mol
Since there are 10 moles of water (H2O) in the hydrated crystal, the total weight of water is:
18.02 g/mol x 10 mol = 180.20 g/mol
Therefore, the total weight of Na2B4O7*10H2O is:
201.22 g/mol + 180.20 g/mol = 381.42 g/mol
From the above calculations, it can be seen that the hydrated crystal form of Na2B4O7 (Na2B4O7*10H2O) contains additional water molecules, which add to its overall weight compared to the anhydrous form.
Since the supplier is offering the same 500.0 g bottle for both forms, it means that you will get more of the desired Na2B4O7 in the anhydrous form because the hydrated crystal form contains water molecules that increase its weight.
To determine which supplier would provide more of the desired Na2B4O7, we need to consider the molar mass and the water content of the compound.
1. Anhydrous form: Na2B4O7
Molar mass of Na2B4O7 = (2 Na) + (4 B) + (7 O) = 46.00 g/mol + 10.81 g/mol + 15.99 g/mol = 201.19 g/mol
2. Hydrated crystal form: Na2B4O7·10H2O
Molar mass of Na2B4O7·10H2O = (2 Na) + (4 B) + (7 O) + 10[2(H) + 16(O)]
= 46.00 g/mol + 10.81 g/mol + 15.99 g/mol + 10[2.02 g/mol + 16.00 g/mol]
= 381.37 g/mol
Now, let's calculate the amount of Na2B4O7 in a 500.0 g bottle from each supplier:
1. Anhydrous form:
Moles of Na2B4O7 = Mass / Molar mass
= 500.0 g / 201.19 g/mol
≈ 2.4874 mol
2. Hydrated crystal form:
Moles of Na2B4O7·10H2O = Mass / Molar mass
= 500.0 g / 381.37 g/mol
≈ 1.3107 mol
Therefore, the supplier offering the anhydrous form of Na2B4O7 would provide more of the desired compound. The anhydrous form would supply approximately 2.4874 mol, while the hydrated crystal form would supply only approximately 1.3107 mol.