to create a 0.25 M Potassium Chloride solution. Your mass is 5.00 grams of Potassium Chloride. How many liters of water is needed?

how many moles of KCl in 5g? 5/74.55 = 0.067 moles

x/0.067moles = 1000mL/0.25moles
x = 268 mL

Ah, the recipe for a 0.25 M Potassium Chloride solution! Let me put on my clown hat and calculate this for you.

To determine how many liters of water you need, we first need to convert the mass of Potassium Chloride to moles. The molar mass of KCl is 74.55 g/mol (since potassium has a molar mass of approximately 39.10 g/mol and chloride has a molar mass of approximately 35.45 g/mol).

So, dividing the mass of Potassium Chloride (5.00 grams) by its molar mass (74.55 g/mol) will give us the number of moles.

5.00 g / 74.55 g/mol = 0.067 moles of KCl

Now, since we want a 0.25 M solution (which means 0.25 moles of KCl per liter of solution), we can use the following equation to find the volume of water needed:

moles of solute (KCl) = molarity (M) x volume (L)

0.067 moles = 0.25 M x volume

Solving for the volume:

volume = 0.067 moles / 0.25 M

volume = 0.268 L

Therefore, you will need approximately 0.268 liters or 268 milliliters of water. Cheers to a perfectly diluted solution!

To determine the number of liters of water needed to create a 0.25 M Potassium Chloride solution with 5.00 grams of Potassium Chloride, you need to know the molar mass of Potassium Chloride.

Step 1: Find the molar mass of Potassium Chloride (KCl)
The atomic mass of potassium (K) is approximately 39.10 grams per mole.
The atomic mass of chlorine (Cl) is approximately 35.45 grams per mole.
So, the molar mass of Potassium Chloride is (39.10 + 35.45) grams per mole = 74.55 grams per mole.

Step 2: Calculate the number of moles of Potassium Chloride (KCl)
Number of moles = mass / molar mass
Number of moles = 5.00 grams / 74.55 grams per mole ≈ 0.067 moles

Step 3: Calculate the volume of water needed to make a 0.25 M solution
Molarity (M) = moles of solute / volume of solution in liters
0.25 M = 0.067 moles / volume in liters

Rearrange the equation to solve for volume:
Volume in liters = moles of solute / Molarity

Volume in liters = 0.067 moles / 0.25 M = 0.268 liters

Therefore, approximately 0.268 liters (or 268 mL) of water is needed to create a 0.25 M Potassium Chloride solution using 5.00 grams of Potassium Chloride.

To determine the volume of water needed to create a 0.25 M Potassium Chloride (KCl) solution, we need to use the formula:

Molarity (M) = moles of solute / volume of solvent (in liters)

Firstly, we need to calculate the moles of Potassium Chloride using its mass and molar mass. The molar mass of KCl is 74.55 g/mol (39.10 g/mol for potassium + 35.45 g/mol for chlorine).

Moles = Mass / Molar mass
Moles = 5.00 g / 74.55 g/mol
Moles ≈ 0.067 mol

Next, we can rearrange the formula to solve for the volume of solvent:

Volume of solvent (in liters) = moles of solute / Molarity

Volume of solvent = 0.067 mol / 0.25 M
Volume of solvent ≈ 0.27 L

Therefore, approximately 0.27 liters (or 270 milliliters) of water is needed to make a 0.25 M Potassium Chloride solution using 5.00 grams of Potassium Chloride.