how many kg of h20 must be added to 75.5g of Ca(NO3)2 to form a 0.500 m solution?

.92kg of water

molality=molessolute/kg sovent

kg water=gramssolute/(molmasssolute*molality)

Whoa, hold your horses! You want me to do some chemistry math? This clown's more into clowning around than crunching numbers. But hey, I'll give it a shot just for you!

To find out how many kg of H2O you need to add, we first need to determine the moles of Ca(NO3)2 present in the solution.

The molar mass of Ca(NO3)2 is 164.09 g/mol. So, we divide 75.5 g by 164.09 g/mol to find the moles of Ca(NO3)2.

Once you have the moles of Ca(NO3)2, you can use the formula Molarity (M) = moles of solute / liters of solution.

0.500 M is equal to 0.500 moles of Ca(NO3)2 per liter of solution. Now, we rearrange the equation to find how many liters of solution we have:

0.500 M = moles of Ca(NO3)2 / liters of solution.

Solving for liters of solution, we get:

Liters of solution = moles of Ca(NO3)2 / 0.500 M.

Now, subtract the volume of the Ca(NO3)2 solution from the total volume of the solution to get the volume of water needed. Convert this volume from liters to kilograms, and you'll have your answer.

Hope this circus act of mine was entertaining enough for you!

To determine the amount of water (H2O) needed to form a 0.500 molar (M) solution of Ca(NO3)2, we first need to calculate the amount of moles of Ca(NO3)2 present in 75.5 grams.

Step 1: Calculate the molar mass of Ca(NO3)2.
The molar mass of Ca(NO3)2 can be calculated by adding up the atomic masses of its constituent elements.
Ca: 40.08 g/mol
N: 14.01 g/mol
O: 16.00 g/mol (for each of the three oxygen atoms)

Molar mass of Ca(NO3)2 = (40.08 g/mol) + 2((14.01 g/mol) + 3(16.00 g/mol))
Molar mass of Ca(NO3)2 = 40.08 g/mol + 2(42.03 g/mol) + 3(48.00 g/mol)
Molar mass of Ca(NO3)2 = 40.08 g/mol + 84.06 g/mol + 144.00 g/mol
Molar mass of Ca(NO3)2 = 268.14 g/mol

Step 2: Convert the mass of Ca(NO3)2 to moles.
Using the molar mass of Ca(NO3)2, we can calculate the number of moles of Ca(NO3)2 in 75.5 grams.
Number of moles = mass / molar mass
Number of moles = 75.5 g / 268.14 g/mol

Step 3: Calculate the volume of the solution.
The volume of the solution can be calculated using the molarity and the number of moles of Ca(NO3)2.
Molarity (M) = moles of solute / volume of solution (in liters)
0.500 M = moles of Ca(NO3)2 / volume of solution (in liters)

Step 4: Calculate the amount of water required.
Since the water does not contribute to the molarity, we can assume that the volume of the solution (in liters) is equal to the volume of water added.
Volume of solution = volume of water added

We can now rearrange the equation for molarity to solve for the volume of water required.
Volume of water (in liters) = moles of Ca(NO3)2 / Molarity
Volume of water (in liters) = (75.5 g / 268.14 g/mol) / 0.500 M

Step 5: Convert the volume of water to kilograms.
To convert the volume of water from liters to kilograms, we need to know the density of water.
Density of water = 1 g/mL = 1 kg/L

Volume of water (in kilograms) = Volume of water (in liters) x Density of water
Volume of water (in kilograms) = (75.5 g / 268.14 g/mol) / 0.500 M x 1 kg/L

Now you can calculate the value for the volume of water in kilograms using the given values.

To determine how many kilograms (kg) of H2O must be added to 75.5g of Ca(NO3)2 to form a 0.500 m (mol/L) solution, we need to follow a step-by-step process.

Step 1: Calculate the moles of Ca(NO3)2
To do this, we divide the given mass of Ca(NO3)2 by its molar mass. The molar mass of Ca(NO3)2 is calculated by summing the atomic masses of each element in the compound.
Molar mass of Ca(NO3)2 = atomic mass of Ca + 2 x (atomic mass of N + 3 x atomic mass of O)
Molar mass of Ca(NO3)2 = 40.08 g/mol + 2 x (14.01 g/mol + 3 x 16.00 g/mol)
Molar mass of Ca(NO3)2 = 164.08 g/mol

Now, we can calculate the moles of Ca(NO3)2:
Moles of Ca(NO3)2 = mass of Ca(NO3)2 / molar mass of Ca(NO3)2
Moles of Ca(NO3)2 = 75.5 g / 164.08 g/mol

Step 2: Calculate the volume of the solution
We have a 0.500 m (mol/L) solution, which means we have 0.500 moles of Ca(NO3)2 in 1 liter (L) of solution.

Using the molarity formula (molarity = moles of solute / volume of solution in liters), we can rearrange it to find the volume of the solution:
Volume of solution (in L) = moles of solute / molarity
Volume of solution = 0.500 moles / 0.500 mol/L
Volume of solution = 1 L

Step 3: Calculate the mass of the final solution
Now that we know the volume of the solution is 1 liter, we can calculate the mass of the final solution by summing the mass of Ca(NO3)2 and the mass of water (H2O).

Mass of final solution = mass of Ca(NO3)2 + mass of water
Mass of water = Mass of final solution - mass of Ca(NO3)2
Mass of water = 1000 g (1 kg) - 75.5 g

Therefore, to form a 0.500 m solution, we need to add approximately 924.5 grams (kg) of H2O to 75.5 grams of Ca(NO3)2.