A 15.0 g sample consisting of a mixture of silver nitrate and sodium nitrate is dissolved

in water. This aqueous mixture then reacts with aqueous potassium chloride to form
3.97 g of solid. Calculate the percent by mass of silver nitrate in the first mixture.

AgNO3 + KCl ==> AgCl + KNO3.

NaNO3 + KCl ==> no reaction.
So you obtained 3.97 g AgCl. Convert that to g AgNO3 this way.
3.97 x (molar mass AgNO3/molar mass AgCl) = ? g AgNO3.
%AgNO3 = (g AgNO3/mass sample)*100 = ?

To calculate the percent by mass of silver nitrate in the mixture, we need to determine the mass of silver nitrate in the mixture and divide it by the total mass of the mixture, then multiply by 100%.

Step 1: Calculate the number of moles of solid formed in the reaction.
To do this, we divide the mass of the solid formed (3.97 g) by its molar mass.

The molar mass of the solid can be calculated by adding the molar masses of silver chloride (AgCl) and sodium chloride (NaCl). The molar mass of AgCl is calculated as follows:

AgCl:
Ag (silver) = 107.87 g/mol
Cl (chlorine) = 35.45 g/mol

So, the molar mass of AgCl is 107.87 + 35.45 = 143.32 g/mol.

Now, to differentiate between the two chlorides, let's assign x to the molar mass of NaCl.

NaCl:
Na (sodium) = 22.99 g/mol
Cl (chlorine) = 35.45 g/mol

So, the molar mass of NaCl is 22.99 + 35.45 = 58.44 g/mol.

To find x, we know that the molar mass of the solid formed (AgCl + NaCl) is 143.32 + x. Since we have mentioned that the molar mass of the solid formed is 3.97 g/mol, we can write the following equation:

143.32 + x = 3.97

Now, solve for x:

x = 3.97 - 143.32

x = -139.35 g/mol

However, since we can't have a negative molar mass, it means an error has occurred in the problem statement. Please double-check the information provided.

If you have any other questions, feel free to ask.

To calculate the percent by mass of silver nitrate in the mixture, we need to analyze the given information and use stoichiometry to determine the amount of silver nitrate present.

Let's break down the problem step by step:

1. Determine the balanced chemical equation:
The reaction between silver nitrate (AgNO3) and potassium chloride (KCl) can be represented by the equation:
AgNO3 + KCl → AgCl + KNO3

2. Calculate the molar mass:
The molar masses of the compounds involved in the reaction are:
AgNO3 = 169.87 g/mol
AgCl = 143.32 g/mol

3. Calculate the amount of AgCl formed:
Given that 3.97 g of solid AgCl is formed, we need to convert this mass to moles using the molar mass of AgCl:
moles of AgCl = 3.97 g / 143.32 g/mol

4. Use stoichiometry to relate the amount of AgNO3 to AgCl:
From the balanced equation, we can see that 1 mole of AgNO3 reacts with 1 mole of AgCl. Therefore, the number of moles of AgNO3 is equal to the number of moles of AgCl:
moles of AgNO3 = moles of AgCl

5. Calculate the mass of AgNO3:
Using the molar mass of AgNO3, we can find the mass of AgNO3 in grams:
mass of AgNO3 = moles of AgNO3 * molar mass of AgNO3

6. Calculate the percent by mass of AgNO3:
Finally, we can calculate the percent by mass of AgNO3 by dividing the mass of AgNO3 by the total mass of the mixture and multiplying by 100:
percent by mass of AgNO3 = (mass of AgNO3 / total mass of mixture) * 100

By following these steps and substituting the given values, you can calculate the percent by mass of silver nitrate in the mixture.