1.0000 g of hydrate of stannic chloride with unknown formula is heated to 100C (celsius) for 30 minutes. The remaining anhydrous salt weighted 0.7836g. What is the formula of this hydrate?

thanks

Stannic chloride is SnCl4 and the hydrate is SnCl4.xH2O

SnCl4.xH2O ==> SnCl4 + xH2O
1.000...........0.7836..0.2164

mols = grams/molar mass
Convert g to moles.
moles SnCl4 = 0.7836/molar mass
moles H2O = 0.2164/molar mass.

Then find the ratio of the two elements to each other with SnCl4 being 1.00. The easy to do that is to divide moles SnCl4 from above by itself (thereby assuring you get 1.00 for that value) then divide the moles H2O by the same number. Round the final value to a whole number and that will give you x. Post your work if you get stuck.

it shouldnt be the ratio of

SnCl4/ H2o....

and the ratio of

H2o/ H20 =1

??

C'mon. My directions aren't that bad.

moles SnCl4 = 0.7836/260.5 = 0.003008
moles H2O = 0.2164/18.015 = 0.01201

0.003008/0.003008 = 1.000
0.01201/0.003008 = 3.992 which rounds to 4.0 and the formula is
SnCl4.4H2O
Note: I consider this a freebie for you in which I have worked the entire problem for you. Your response to my instructions makes no sense at all and COULD be construed as being done on purpose to get an entire problem worked for you from scratch. Sorry if that sounds harsh and especially sorry if that isn't true; however, I will not be so accommodating in the future.

Well, well, well, we have a chemistry conundrum here! Let's put on our detective hats and solve this mystery, shall we?

So, we know that we have a hydrate of stannic chloride, with an unknown formula. When it's heated, the water vaporizes and leaves behind the anhydrous salt. Clever, clever.

Now, we're given the masses of the original hydrate (1.0000g) and the remaining anhydrous salt (0.7836g).

To find the formula, we need to determine the moles of the anhydrous salt and the water that was lost.

First, let's find the moles of the anhydrous salt:

Molar mass of the anhydrous salt = Unknown (we don't have the formula, after all!)

Moles = Mass / Molar mass

Moles of anhydrous salt = 0.7836g / Unknown molar mass

Now, we need to find the moles of water that was lost. Since the hydrate has lost water, the difference between the mass of the original hydrate and the anhydrous salt will give us the mass of water lost:

Mass of water lost = Mass of original hydrate - Mass of anhydrous salt

Now, let's convert the mass of water lost to moles:

Moles of water lost = Mass of water lost / Molar mass of water

Next, we need to determine the ratio between the moles of the anhydrous salt and the moles of water lost. This ratio will give us the formula of the hydrate.

Let's call this ratio "x:y," where x is the moles of the anhydrous salt and y is the moles of water lost.

Now, our task is to find the value of x and y.

But, alas, we don't have enough information! We need more clues, my friend. The molar mass of the anhydrous salt or the mole ratio between the stannic chloride and water molecules would help in solving this puzzle.

If you happen to find more information, I'll be here, ready to assist you with a chemistry comedy routine! Keep the laughs coming!

To determine the formula of the hydrate of stannic chloride, we need to first calculate the molar mass of the hydrated and anhydrous salts.

Step 1: Calculate the molar mass of the anhydrous salt (stannic chloride):
To do this, we need to find the molar mass of stannic chloride (SnCl4). The molar mass of tin (Sn) is approximately 118.71 g/mol, and the molar mass of chlorine (Cl) is approximately 35.45 g/mol.
So, the molar mass of SnCl4 is:
4(Cl) x 35.45 g/mol + 1(Sn) x 118.71 g/mol = 232.26 g/mol.

Step 2: Calculate the molar mass of water (H2O):
The molar mass of hydrogen (H) is approximately 1.01 g/mol, and the molar mass of oxygen (O) is approximately 16.00 g/mol.
So, the molar mass of H2O is:
2(H) x 1.01 g/mol + 1(O) x 16.00 g/mol = 18.02 g/mol.

Step 3: Calculate the molar mass of the water lost:
The mass of the anhydrous salt obtained is 0.7836 g, and the mass of the remaining water is 1.0000 g - 0.7836 g = 0.2164 g. Since the molar mass of water is 18.02 g/mol, we can calculate the moles of water lost:
0.2164 g / 18.02 g/mol = 0.012 mol.

Step 4: Calculate the moles of the anhydrous salt:
To calculate the moles of the anhydrous salt, we divide its mass (0.7836 g) by its molar mass (232.26 g/mol):
0.7836 g / 232.26 g/mol = 0.00337 mol.

Step 5: Determine the ratio of moles between the anhydrous salt and water:
By comparing the moles of water lost (0.012 mol) to the moles of the anhydrous salt (0.00337 mol), we find that the ratio is approximately 3:1.

Step 6: Write the formula of the hydrate:
Based on the 3:1 ratio, the formula of the hydrate is SnCl4 : 3H2O.

Therefore, the formula of the hydrate of stannic chloride is SnCl4 : 3H2O.