you mix 60.0 mL of 1.0 M silver nitrate with 25.0 mL of .80 M sodium chloride. what mass of silver chloride should you form?
Well, isn't that a silver-tongued question! Let's calculate the molar ratio of silver chloride formed from the reaction between silver nitrate and sodium chloride.
According to the balanced chemical equation:
AgNO₃ + NaCl → AgCl + NaNO₃
The molar ratio of AgNO₃ to AgCl is 1:1, meaning one mole of AgNO₃ reacts with one mole of AgCl. Similarly, the molar ratio of NaCl to AgCl is also 1:1.
To find the moles of AgNO₃, we can use the equation: moles = molarity × volume (in liters).
Moles of AgNO₃ = 1.0 M × 0.060 L = 0.06 moles
Moles of NaCl = 0.80 M × 0.025 L = 0.020 moles
Since the molar ratio of AgNO₃ to AgCl is 1:1, the moles of AgCl formed would be 0.06 moles.
The molar mass of AgCl is approximately 143.32 g/mol. To find the mass, we'll multiply the number of moles by the molar mass:
Mass of AgCl = 0.06 moles × 143.32 g/mol = 8.60 grams
So, you should form approximately 8.60 grams of silver chloride. Just remember, this answer is not tarnished with seriousness, it's all about the silver lining!
To determine the mass of silver chloride formed, we need to use the balanced chemical equation and calculate the moles of reactants. Then, we can use stoichiometry to find the moles of silver chloride produced, and finally convert moles to mass using the molar mass of silver chloride.
1. Write the balanced chemical equation for the reaction between silver nitrate (AgNO3) and sodium chloride (NaCl):
AgNO3 + NaCl -> AgCl + NaNO3
2. Calculate the moles of silver nitrate (AgNO3):
Moles of AgNO3 = volume (L) x molarity (mol/L)
Moles of AgNO3 = 0.060 L x 1.0 mol/L
Moles of AgNO3 = 0.060 mol
3. Calculate the moles of sodium chloride (NaCl):
Moles of NaCl = volume (L) x molarity (mol/L)
Moles of NaCl = 0.025 L x 0.80 mol/L
Moles of NaCl = 0.020 mol
4. Determine the limiting reactant:
Since the stoichiometric ratio of AgNO3 to AgCl is 1:1, the reactant that produces the fewer moles of product will be the limiting reactant. In this case, sodium chloride (NaCl) produces fewer moles of AgCl.
5. Calculate the moles of AgCl formed:
Moles of AgCl = Moles of limiting reactant (NaCl)
Moles of AgCl = 0.020 mol
6. Convert moles of AgCl to mass using the molar mass of AgCl:
Molar mass of AgCl = atomic mass of Ag + atomic mass of Cl
Molar mass of AgCl = 107.87 g/mol + 35.45 g/mol
Molar mass of AgCl = 143.32 g/mol
Mass of AgCl = Moles of AgCl x Molar mass of AgCl
Mass of AgCl = 0.020 mol x 143.32 g/mol
Mass of AgCl = 2.87 grams
Therefore, you should form 2.87 grams of silver chloride.
To find the mass of silver chloride formed, we need to use the concept of stoichiometry.
The balanced chemical equation for the reaction between silver nitrate (AgNO3) and sodium chloride (NaCl) is:
AgNO3 + NaCl -> AgCl + NaNO3
From the equation, we can see that 1 mole of AgNO3 reacts with 1 mole of NaCl to produce 1 mole of AgCl.
First, let's calculate the number of moles of silver nitrate (AgNO3):
Moles of AgNO3 = (volume in liters) x (concentration in mol/L)
= (60.0 mL / 1000 mL/L) x (1.0 mol/L)
= 0.060 L x 1.0 mol/L
= 0.060 mol
Next, let's calculate the number of moles of sodium chloride (NaCl):
Moles of NaCl = (volume in liters) x (concentration in mol/L)
= (25.0 mL / 1000 mL/L) x (0.80 mol/L)
= 0.025 L x 0.80 mol/L
= 0.020 mol
Since the stoichiometry of the balanced equation tells us that both reactants have a 1:1 ratio to the product, the limiting reactant will be the one that produces the smallest number of moles. In this case, NaCl is the limiting reactant because it produces fewer moles than AgNO3.
Now we need to calculate the moles of AgCl formed using the limiting reactant (NaCl):
Moles of AgCl = Moles of NaCl = 0.020 mol
Finally, let's calculate the mass of silver chloride (AgCl) formed using its molar mass:
Mass of AgCl = Moles of AgCl x Molar mass of AgCl
The molar mass of AgCl is the sum of the atomic masses of silver (Ag) and chlorine (Cl):
Molar mass of AgCl = (atomic mass of Ag) + (atomic mass of Cl)
= 107.87 g/mol + 35.45 g/mol
= 143.32 g/mol
Now, we can calculate the mass of silver chloride (AgCl):
Mass of AgCl = 0.020 mol x 143.32 g/mol
= 2.87 g
Therefore, you should form 2.87 grams of silver chloride.
1.0 M x 0.060 L = moles AgNO3.
0.80 M x 0.0250 L = moles NaCl.
AgNO3 + NaCl ==> NaNO3 + AgCl.
This should help.