If NaCl has a solubility of 36.0 g in 100 g of H2O at 20 °C, how many moles of water are needed to prepare a saturated solution containing 0.263 mol of NaCl at 20 °C?

A solubility of 36.0 g NaCl/100 g H2O is 36.0/58.44 = 0.616 mol NaCl.

100 g H2O is 100/18 = about 5.55 mols H2O so the solubility in terms of mols/mols is 0.616 mols NaCl/5.55 mols H2O.

5.55 mols H2O x (0.263/0.616) = ? mols H2O to prepare a saturated solution.

Well, let's tackle this problem like a clown tackling a unicycle, with a mixture of precision and comedy!

To find the number of moles of water needed, we first need to convert the grams of NaCl to moles. So, given that the solubility of NaCl is 36.0 g in 100 g of H2O, we can say that 36.0 g of NaCl is equivalent to 0.263 mol of NaCl.

Now, to find the number of moles of water, we can use the fact that the ratio of NaCl to H2O is 1:1. This means that for every 1 mole of NaCl, we need 1 mole of H2O.

Since we have 0.263 mol of NaCl, we also need 0.263 mol of H2O. So voila, there you have it!

To prepare a saturated solution containing 0.263 mol of NaCl at 20 °C, you will need 0.263 mol of water. Just remember, when it comes to moles, always keep your clown shoes on and your calculations precise!

To determine the moles of water needed to prepare a saturated solution containing 0.263 mol of NaCl at 20 °C, we can use the molar mass of water and the given solubility of NaCl. Here are the steps:

1. Find the molar mass of water (H2O). The molar mass of hydrogen (H) is 1.008 g/mol, and the molar mass of oxygen (O) is 16.00 g/mol. Adding these together, we get:
Molar mass of H2O = (2 * molar mass of H) + molar mass of O
= (2 * 1.008 g/mol) + 16.00 g/mol
= 18.015 g/mol

2. Calculate the mass of NaCl needed to form a saturated solution. The solubility of NaCl is 36.0 g in 100 g of water, so the mass of NaCl needed to form a saturated solution can be calculated using the formula:
Mass of NaCl = (Mass of water / 100) * Solubility of NaCl
= (100 g / 100) * 36.0 g
= 36.0 g

3. Determine the mass of water needed to dissolve 0.263 mol of NaCl. To do this, divide the moles of NaCl by the molar mass of NaCl and then multiply by the molar mass of water:
Mass of water = (Moles of NaCl / Molar mass of NaCl) * Molar mass of water
= (0.263 mol / 58.44 g/mol) * 18.015 g/mol
= 0.0873 * 18.015 g
≈ 1.573 g

4. Convert the mass of water to moles. Divide the mass of water by the molar mass of water:
Moles of water = Mass of water / Molar mass of water
= 1.573 g / 18.015 g/mol
≈ 0.0873 mol

Therefore, approximately 0.0873 moles of water are needed to prepare a saturated solution containing 0.263 mol of NaCl at 20 °C.

To find the number of moles of water needed to prepare a saturated solution containing 0.263 mol of NaCl, we need to use the mole ratio between NaCl and water.

The molar mass of NaCl is 58.44 g/mol.

First, let's calculate the mass of NaCl needed to prepare a saturated solution containing 0.263 mol of NaCl:
Mass of NaCl = Number of moles of NaCl × Molar mass of NaCl
Mass of NaCl = 0.263 mol × 58.44 g/mol
Mass of NaCl = 15.337 g (approx)

Next, let's calculate the mass of water needed to dissolve this amount of NaCl:
Mass of water = Total mass of solution - Mass of NaCl
Mass of water = 100 g - 15.337 g
Mass of water = 84.663 g (approx)

Now, we can calculate the number of moles of water needed:
Number of moles of water = Mass of water ÷ Molar mass of water

The molar mass of water (H2O) is 18.02 g/mol.

Number of moles of water = 84.663 g ÷ 18.02 g/mol
Number of moles of water = 4.698 mol (approx)

Therefore, you would need approximately 4.698 moles of water to prepare a saturated solution containing 0.263 mol of NaCl at 20 °C.