A 10g sample of an unknown ionic compound is dissolved, and the solution is treated with enough AgNO3 to precipitate all the chloride ion. If 30.1 g of AgCI are recovered, which of the following compound could be the unknown?

A. NaCI
B. NaNO3
C.BaCI2
D. Mg CI2
E.KCI
Pleas help me to solve this problem, I know the answer but I don't know the step how to solve it.

lol I know its late but for any other person that looks at this question in the future.

Using molar mass of AgCl you get roughly 24.74% Cl in the ionic compound.

Next, multiply that value in decimal form by 30.1 grams to find the grams of Cl. You should get about 7.44.

Then, you know the percent of Cl in the given 10 grams is .744 so you equate this to the grams of Chloride over grams of Chloride+x. NOTE: for the Magnesium instead of having 35.453 grams you will have 70.906 grams because there are two Cl.

Finally, solve for x and you should get 24.4g, which is fairly close to the molar mass of Magnesium.

of 30.1 g of AgCl, how many grams of Cl is that? ANS 30.1*35.4/(35.4+107.8)=7.44 grams. That leaves 2.56g for the metal

Now check moles: molesCl=7.44/35.4=.21moles

Now of the formulas, which metal has .21moles in 2.56g

Try NaCl: .21=2.56/23=not equal
Now, try KCl: .21=2.56/39=wont work.

Try MgCl2. In this, you want .21/2 moles Mg, .105=2.56/24.3=.105
amazing.

good

Well, well, well, it seems like you need help solving a chemistry problem! Don't worry, I've got your back.

To figure out which compound could be the unknown, we need to use some good old stoichiometry. Let's break it down, shall we?

The given problem tells us that 30.1 g of AgCl is recovered when reacting with the unknown compound. Now, we know that each chloride ion has a mass of 35.45 g/mol (taking the molar mass of Cl).

So, if we have 30.1 g of AgCl formed, it means that we had 30.1 g of chloride ions in the unknown compound. Keep up, we're just getting started!

Now, let's determine how many moles of chloride ions are present in the sample. We can do this by dividing the mass of chloride ions by their molar mass:

moles of chloride ions = mass of chloride ions / molar mass of chloride ions

moles of chloride ions = 30.1 g / 35.45 g/mol

Do the math, and you'll find out the number of moles. I believe in you!

Once you have the number of moles of chloride ions, you can use the balanced chemical equation to determine the ratio between chloride ions and the unknown compound.

For example, let's take compound A (NaCl). If it were the unknown compound, there would have to be 1 mole of NaCl for every mole of chloride ions. So, check if the number of moles of chloride ions you found earlier is equal to the number of moles of NaCl.

Repeat the same process for each of the given compounds (B, C, D, and E), and you'll find out which one matches the number of moles of chloride ions.

I hope this helps you solve the problem! Just remember to keep your chemistry hat on and use a little bit of math magic. Good luck!

To solve this problem, we need to use the principle of conservation of mass. First, we calculate the number of moles of AgCI that were recovered from the reaction.

The molar mass of AgCI can be calculated by adding the atomic masses of silver (Ag) and chlorine (CI). The atomic mass of Ag is 107.87 g/mol, and the atomic mass of CI is 35.45 g/mol.

Molar mass of AgCI = (1 × Ag) + (1 × CI) = 107.87 + 35.45 = 143.32 g/mol.

Next, we can calculate the number of moles of AgCI using the formula:

Moles of AgCI = Mass of AgCI / Molar mass of AgCI.

Given that 30.1 g of AgCI were recovered, we can substitute this value into the formula:

Moles of AgCI = 30.1 g / 143.32 g/mol.

Moles of AgCI ≈ 0.2099 mol.

Now, we need to determine the number of moles of chloride ions (Cl-) in the AgCI precipitate. Since AgCI is formed when a chloride ion is combined with a silver ion, the ratio between moles of AgCI and moles of chloride ions is 1:1.

Therefore, the number of moles of chloride ions is also approximately 0.2099 mol.

Next, we need to determine the number of moles of chloride ions in the original sample. Since the chloride ions came from the unknown compound, we can assume that all the chloride ions in the sample precipitated as AgCI. This means that the ratio between moles of chloride ions and moles of the unknown compound is also 1:1.

Therefore, the number of moles of chloride ions in the original sample is approximately 0.2099 mol.

Now, we can determine the mass of the unknown compound using its molar mass. Let's assume the unknown compound is represented by the formula MX, where M is the metal cation and X is the chloride ion.

We know that the molar mass of the unknown compound MX is equal to the sum of the molar masses of the metal cation and the chloride ion:

Molar mass of MX = Molar mass of M + Molar mass of X.

Since the unknown compound contains chloride ions, its molar mass can be calculated by adding the atomic masses of the metal cation and the chlorine ion.

Using the molar mass of chloride (35.45 g/mol) and the number of moles of chloride ions (0.2099 mol), we can substitute these values into the formula to find the mass of the unknown compound:

Mass of unknown compound = Moles of chloride ions × Molar mass of chloride ion.

Mass of unknown compound = 0.2099 mol × 35.45 g/mol.

Mass of unknown compound ≈ 7.441 g.

Here, notice that the mass of the unknown compound is less than the original mass of the sample (10g). This suggests that the unknown compound is a hydrate, meaning it contains water molecules in its structure.

Now, we can identify which compound could be the unknown based on its molar mass:

A. NaCI → Molar mass = 22.99 g/mol + 35.45 g/mol = 58.44 g/mol. Not a match.

B. NaNO3 → Molar mass = 22.99 g/mol + 14.01 g/mol + (3 × 16.00 g/mol) = 85.00 g/mol. Not a match.

C. BaCI2 → Molar mass = 137.33 g/mol + (2 × 35.45 g/mol) = 208.23 g/mol. Not a match.

D. MgCI2 → Molar mass = 24.31 g/mol + (2 × 35.45 g/mol) = 95.21 g/mol. Not a match.

E. KCI → Molar mass = 39.10 g/mol + 35.45 g/mol = 74.55 g/mol. Not a match.

Based on the molar mass calculations, the possible compound that could be the unknown is E. KCI.