a 6.54 g sample consisting of a mixture of silver nitrate and sodium nitrate is dissolved in water. this mixture then reacts with barium chloride to for 3.50 g of silver chloride. calculate the percent by mass of silver nitrate in the first mixture

2AgNO3 + BaCl2 ==> 2AgCl + Ba(NO3)2

How many moles AgCl were formed? That is g/molar mass = moles = 3.50/143.32 = 0.0244 moles.

Since 1 mole AgCl = 1 mole AgNO3, we must have had 0.0244 moles AgNO3 in the original sample and we convert to grams by g = moles x molar mass.

Then percent AgNO3 = (mass AgNO3/mass sample)*100 = ??

%AgNO3 is 10.38%

Well, well, well, looks like we have a chemistry question here. Don't worry, I've got the perfect clownish solution for you!

Okay, let's get down to business. First, we need to calculate the moles of silver chloride formed. With a molar mass of silver chloride of 143.32 g/mol, we can divide the mass of silver chloride (3.50 g) by its molar mass to get the moles.

Moles of silver chloride = 3.50 g / 143.32 g/mol = 0.0244 mol

Since every mole of silver chloride comes from one mole of silver nitrate, we know that the moles of silver nitrate in the mixture is also 0.0244 mol.

Now, let's calculate the mass of silver nitrate. With a molar mass of silver nitrate of 169.87 g/mol, we can multiply the moles of silver nitrate by its molar mass.

Mass of silver nitrate = 0.0244 mol * 169.87 g/mol = 4.10 g

Now we can calculate the percent by mass of silver nitrate in the mixture.

% by mass = (mass of silver nitrate / mass of mixture) * 100

% by mass = (4.10 g / 6.54 g) * 100 = 62.61%

So, the percent by mass of silver nitrate in the first mixture is approximately 62.61%. Ta-da!

To calculate the percent by mass of silver nitrate in the first mixture, we need to use stoichiometry and convert the mass of silver chloride formed into the mass of silver nitrate originally present.

First, we need to find the number of moles of silver chloride formed. We can use the molar mass of silver chloride to convert the mass of silver chloride to moles:
Molar mass of AgCl = Atomic mass of Ag + Atomic mass of Cl = 107.87 g/mol + 35.45 g/mol = 143.32 g/mol

Number of moles of AgCl formed = Mass of AgCl / Molar mass of AgCl
Number of moles of AgCl formed = 3.50 g / 143.32 g/mol

Next, we need to use the balanced equation between silver chloride and silver nitrate to find the ratio of moles between them. The balanced equation is as follows:
2 AgNO3 + BaCl2 -> 2 AgCl + Ba(NO3)2

From this equation, we see that 2 moles of AgNO3 react to form 2 moles of AgCl. Therefore, the ratio of moles of AgNO3 to moles of AgCl is 2:2, or 1:1.

Now we can calculate the number of moles of AgNO3 originally present, using the number of moles of AgCl formed as a reference (since they have a 1:1 ratio):
Number of moles of AgNO3 = Number of moles of AgCl formed

Now we have the moles of AgNO3. To find the mass of AgNO3, we can use the molar mass of AgNO3:
Molar mass of AgNO3 = Atomic mass of Ag + Atomic mass of N + (3 x Atomic mass of O)
Molar mass of AgNO3 = 107.87 g/mol + 14.01 g/mol + (3 x 16.00 g/mol) = 169.87 g/mol

Mass of AgNO3 = Number of moles of AgNO3 x Molar mass of AgNO3
Mass of AgNO3 = (3.50 g / 143.32 g/mol) x 169.87 g/mol

Finally, we can calculate the percent by mass of AgNO3 in the mixture:
Percent by mass of AgNO3 = (Mass of AgNO3 / Mass of initial mixture) x 100
Percent by mass of AgNO3 = (3.50 g / 6.54 g) x 100

Now you can perform the calculations to find the final answer.

To calculate the percent by mass of silver nitrate in the initial mixture, you'll need to determine the mass of silver nitrate present in the sample and then divide it by the total mass of the mixture. Here's how you can do it step by step:

Step 1: Calculate the mass of silver chloride formed.
Given that the mass of silver chloride formed is 3.50 g, this represents the mass of silver that was originally present in the silver nitrate. Since the molar mass of silver chloride (AgCl) is 143.32 g/mol, we can calculate the number of moles of silver chloride formed as follows:

Number of moles of AgCl = mass of AgCl / molar mass of AgCl
Number of moles of AgCl = 3.50 g / 143.32 g/mol

Step 2: Determine the number of moles of silver nitrate that reacted.
Since each mole of silver nitrate (AgNO3) reacts with one mole of silver chloride to form one mole of silver chloride, the number of moles of silver chloride formed is equal to the number of moles of silver nitrate that reacted. Therefore:

Number of moles of AgNO3 = Number of moles of AgCl

Step 3: Calculate the mass of silver nitrate using its molar mass.
Using the molar mass of silver nitrate (AgNO3), which is 169.87 g/mol, we can calculate the mass of silver nitrate present in the sample as follows:

Mass of AgNO3 = Number of moles of AgNO3 × molar mass of AgNO3

Step 4: Calculate the percent by mass of silver nitrate in the mixture.
Finally, we can determine the percent by mass of silver nitrate in the mixture using the following formula:

Percent by mass of AgNO3 = (Mass of AgNO3 / Initial mass of mixture) × 100

Just substitute the values calculated in the previous steps into this formula to get the final result.