1. The formation of water-insoluble chloride salts, especially silver(I) chloride, is useful for the analysis of compounds that contain chlorine. Consider the following unbalanced equation:
_____ BaCl2(aq) + _____ AgNO3(aq) --> _____ AgCl(s) + _____ Ba(NO3)2(aq)
a. Balance the equation.
BaCl2 + 2AgNO3 = 2AgCl + Ba(NO3)2
b. What mass of AgNO3, in grams, is required to react completely with 1.00 gram BaCl2?
c. What mass (in grams) of AgCl is produced in this process?
d. What mass (in grams) of Ba(NO3)2 is also produced in this process?
To answer part b, we need to determine the molar masses of BaCl2 and AgNO3:
- Molar mass of BaCl2 = (1 x 137.33 g/mol) + (2 x 35.45 g/mol) = 208.23 g/mol
- Molar mass of AgNO3 = (1 x 107.87 g/mol) + (1 x 14.01 g/mol) + (3 x 16.00 g/mol) = 169.87 g/mol
Next, we can use the stoichiometric coefficients from the balanced equation (1:2 ratio of BaCl2 to AgNO3) to calculate the number of moles of AgNO3 needed:
- Moles of BaCl2 = mass of BaCl2 / molar mass of BaCl2 = 1.00 g / 208.23 g/mol = 0.00480 mol
- Moles of AgNO3 = 2 x moles of BaCl2 = 2 x 0.00480 mol = 0.00960 mol
Finally, we can use the molar mass of AgNO3 to convert moles to grams:
- Mass of AgNO3 = moles of AgNO3 x molar mass of AgNO3 = 0.00960 mol x 169.87 g/mol = 1.63 g
Therefore, 1.63 grams of AgNO3 is required to react completely with 1.00 gram of BaCl2.
Moving on to part c, we can use the stoichiometric coefficients from the balanced equation (1:1 ratio of AgNO3 to AgCl) to calculate the moles of AgCl produced:
- Moles of AgCl = 0.00960 mol
Next, we can use the molar mass of AgCl to convert moles to grams:
- Molar mass of AgCl = (1 x 107.87 g/mol) + (1 x 35.45 g/mol) = 143.32 g/mol
- Mass of AgCl = moles of AgCl x molar mass of AgCl = 0.00960 mol x 143.32 g/mol = 1.38 g
Therefore, 1.38 grams of AgCl is produced in this process.
Finally, for part d, we can use the stoichiometric coefficients from the balanced equation (1:1 ratio of Ba(NO3)2 to AgCl) to calculate the moles of Ba(NO3)2 produced:
- Moles of Ba(NO3)2 = 0.00960 mol
Next, we can use the molar mass of Ba(NO3)2 to convert moles to grams:
- Molar mass of Ba(NO3)2 = (1 x 137.33 g/mol) + (2 x 14.01 g/mol) + (6 x 16.00 g/mol) = 261.34 g/mol
- Mass of Ba(NO3)2 = moles of Ba(NO3)2 x molar mass of Ba(NO3)2 = 0.00960 mol x 261.34 g/mol = 2.51 g
Therefore, 2.51 grams of Ba(NO3)2 is produced in this process.
To answer parts (b), (c), and (d) of the question, we need to use stoichiometry, which involves using the balanced equation to relate the quantities of reactants and products.
b. To determine the mass of AgNO3 required to react completely with 1.00 gram BaCl2, we need to convert the given mass of BaCl2 to moles and then use the stoichiometric ratio between BaCl2 and AgNO3 to find the corresponding amount of AgNO3.
1.00 gram BaCl2 * (1 mole BaCl2 / molar mass of BaCl2) * (2 moles AgNO3 / 1 mole BaCl2) * (molar mass of AgNO3 / 1 mole AgNO3) = mass of AgNO3 in grams
Note that we use the molar masses of BaCl2 (208.23 g/mol) and AgNO3 (169.87 g/mol) to convert between grams and moles.
c. Once we know the mass of AgNO3 required, we can use the stoichiometric ratio between AgNO3 and AgCl to find the corresponding mass of AgCl produced. The stoichiometric ratio is 2 moles AgCl for every 2 moles AgNO3.
mass of AgNO3 in grams * (2 moles AgCl / 2 moles AgNO3) * (molar mass of AgCl / 1 mole AgCl) = mass of AgCl in grams
d. Similarly, we use the stoichiometric ratio between AgNO3 and Ba(NO3)2 to find the corresponding mass of Ba(NO3)2 produced. The stoichiometric ratio is 1 mole Ba(NO3)2 for every 2 moles AgNO3.
mass of AgNO3 in grams * (1 mole Ba(NO3)2 / 2 moles AgNO3) * (molar mass of Ba(NO3)2 / 1 mole Ba(NO3)2) = mass of Ba(NO3)2 in grams
By substituting the values obtained from the calculations, you will find the mass of AgNO3, AgCl, and Ba(NO3)2 produced in the process.