Weight of the Rock Salt Sample: .343 (g)
Weight of the Rock Salt Solution: 9.910 (g)
Trial #1 Trial #2 Trial #3
Weight of Rock Salt Solution Delivered (g) : .89 1.17 .786
Weight of AgNO3 Solution Delivered (g) : 1.53 .548 .786
Concentration of AgNO3 : 4.70e-4 (moles of AgNO3/g of solution)
Calculate the number of moles of chloride in the sample of rock salt solution. (enter your answer for trial #1 in the first box, trial #2 in the second box, and trial #3 in the third box)
To calculate the number of moles of chloride in the sample of rock salt solution, we need to use the stoichiometry of the reaction between AgNO3 and chloride ions (Cl-) in the rock salt.
The balanced chemical equation for the reaction is:
AgNO3 + NaCl -> AgCl + NaNO3
From the balanced equation, we can see that 1 mole of AgNO3 reacts with 1 mole of NaCl to produce 1 mole of AgCl.
To find the number of moles of chloride in the rock salt solution, we can use the following steps for each trial:
Step 1: Calculate the number of moles of AgNO3 delivered:
Number of moles of AgNO3 = weight of AgNO3 delivered / molar mass of AgNO3
The molar mass of AgNO3 (silver nitrate) is 169.87 g/mol.
Step 2: Calculate the number of moles of AgCl formed (assuming all chloride reacts):
Number of moles of AgCl = number of moles of AgNO3
Step 3: Calculate the number of moles of chloride in the rock salt solution:
Number of moles of chloride = number of moles of AgCl
Let's calculate the number of moles of chloride for each trial:
Trial #1:
Number of moles of AgNO3 = 1.53 g / 169.87 g/mol = 0.00901 mol
Number of moles of chloride = 0.00901 mol
Trial #2:
Number of moles of AgNO3 = 0.548 g / 169.87 g/mol = 0.00323 mol
Number of moles of chloride = 0.00323 mol
Trial #3:
Number of moles of AgNO3 = 0.786 g / 169.87 g/mol = 0.00462 mol
Number of moles of chloride = 0.00462 mol
Therefore, the number of moles of chloride in the rock salt solution for trial #1 is 0.00901 mol, for trial #2 is 0.00323 mol, and for trial #3 is 0.00462 mol.