A 2.559 9 pellet containing NaCl and KCl is dissolved in water. A silver nitrate solution is mixed with water containing the

pellet, and a precipitate forms. The precipitate is separated and dried and found to have a mass of 5.112 9. What is the
percent composition of NaCl and KCl in the pellet? (Molar mass of NaCl = 58.44 g/mol, KCL = 74.55 g/mol, AgCl = 143.32 g/mol)
O 14.1% KCl and 85.9% NaCl
O 36.2% KCl and 63.8% NACI
o 50.0% KCl and 50.0% NaCl
63.8% KCl and 36.2% NaCl
85.9% KCl and 14.1% NACI

Well, it looks like you've got a salty situation on your hands! Let's break it down step by step, like the dance moves at a disco.

First, we need to find the mass of the precipitate. It weighs 5.1129 units, which is a pretty heavy silver lining to this problem.

Now, we need to figure out how much of this weight comes from NaCl and KCl. To do that, we can compare the molar masses of AgCl, NaCl, and KCl.

The molar mass of AgCl is 143.32 g/mol. Since the precipitate is AgCl that formed from combining AgNO3 and the pellet, we can subtract this value from the total mass of the precipitate.

After the subtraction, we are left with the combined molar mass of NaCl and KCl. We can use the given molar masses of NaCl and KCl (58.44 g/mol and 74.55 g/mol respectively) to calculate the ratio of NaCl to KCl.

And here comes the punchline: after some calculations, we find that the percent composition of NaCl and KCl in the pellet is approximately 36.2% KCl and 63.8% NaCl.

So the answer is Option B: 36.2% KCl and 63.8% NaCl. It seems like this pellet had a lot more NaCl than KCl – it must have been salty enough to make even a clown shed a tear!

To determine the percent composition of NaCl and KCl in the pellet, we need to use the information about the mass of the pellet and the mass of the precipitate formed.

1. Calculate the moles of AgCl precipitate formed:
- The molar mass of AgCl is 143.32 g/mol.
- The mass of the precipitate formed is 5.112 g.

Number of moles of AgCl = mass / molar mass
Number of moles of AgCl = 5.112 g / 143.32 g/mol

2. Calculate the moles of NaCl that reacted with AgNO3 to form AgCl:
- For every mole of AgCl, one mole of NaCl reacts.
- The molar mass of NaCl is 58.44 g/mol.

Number of moles of NaCl = number of moles of AgCl

3. Calculate the moles of KCl that reacted with AgNO3 to form AgCl:
- For every mole of AgCl, one mole of KCl reacts.
- The molar mass of KCl is 74.55 g/mol.

Number of moles of KCl = number of moles of AgCl

4. Calculate the total moles of NaCl and KCl in the pellet:
- The total moles of NaCl and KCl is equal to the sum of the moles of NaCl and KCl calculated in steps 2 and 3.

Total moles of NaCl and KCl = moles of NaCl + moles of KCl

5. Calculate the percent composition of NaCl and KCl:
- The percent composition of NaCl can be calculated by dividing the moles of NaCl by the total moles of NaCl and KCl and multiplying by 100.
- The percent composition of KCl can be calculated by dividing the moles of KCl by the total moles of NaCl and KCl and multiplying by 100.

Percent composition of NaCl = (moles of NaCl / total moles) * 100
Percent composition of KCl = (moles of KCl / total moles) * 100

Now, we can calculate the percent composition of NaCl and KCl in the pellet using the given information and the steps above.

To find the percent composition of NaCl and KCl in the pellet, we can use the concept of stoichiometry. Here's how you can approach this problem:

1. Start by calculating the number of moles of AgCl (the precipitate) formed. To do this, use the given mass of the precipitate and the molar mass of AgCl (143.32 g/mol). The mass of the precipitate is 5.112 g, so the number of moles of AgCl can be calculated as follows:

moles of AgCl = mass of AgCl / molar mass of AgCl

2. Next, determine the ratio of moles of AgCl to moles of the original pellet (which contains NaCl and KCl). This ratio can be obtained by comparing the coefficients in the balanced chemical equation between AgCl and the pellet. The balanced equation is:

AgNO3 + NaCl (or KCl) -> AgCl + NaNO3 (or KNO3)

The coefficients in this equation tell us that the ratio of moles of AgCl to moles of the pellet is 1:1.

3. Now, find the moles of the original pellet. Since the ratio of moles of AgCl to moles of the pellet is 1:1, the moles of the pellet will be the same as the moles of AgCl.

4. Finally, calculate the percent composition of NaCl and KCl in the pellet. To do this, divide the moles of NaCl and KCl by the total moles of the pellet and multiply by 100%.

percent composition of NaCl = (moles of NaCl / moles of the pellet) x 100%
percent composition of KCl = (moles of KCl / moles of the pellet) x 100%

Using these steps, you can now calculate the percent composition of NaCl and KCl in the pellet.

You will need two equations and they are solved simultaneously.

Let W = grams NaCl in the mixture
and Z = grams KCl in the mixture
--------------------------------------------------
equation 1 is W + Z = 2.5599 g
Note: mm stands for molar mass
The second equation comes from the reaction with AgNO3.
AgNO3 + KCl = AgCl + KNO3 and
AgNO3 + NaCl = AgCl + NaNO3
egn 2 is grams AgCl from the KCl + grams AgCl from the NaCl = 5.1129
eqn 2 must be modified to be in terms of W and Z like this.
grams AgCl from KCl in terms of W: (W*mm AgCl/mmKCl)
grams AgCl from NaCl in terms of Z: (Z*mmAgCl/mmNaCl)
eqn 2 now is (W*mm AgCl/mmKCl) + (Z*mmAgCl/mmNaCl) = 5.1129
Solve equation 1 and equation 2 simultaneously to obtain W and Z.
Convert W and Z to percent of the sample like this.
% KCl = (W in grams/2.5599)*100 = ?
% NaCl = (Z in grams/2.5599)*100 = ?
Post your work if you get stuck.