1.)
a. After using the solution viewer in the virtual lab, I found the following masses:
- Na+: 0.39g
- Cl-: 0.61g
Together, they add up to NaCl's mass of 1.00g.
b. After adding 100mL of water to the 1.00g AgNO3 solution and using the solution viewer:
- Ag+: 0.61g
- NO3-: 0.39g
c. After adding the solid AgNO3 to the 1.00g NaCl solution the mass of each species is as follows:
Table 1: Mass of each species after reaction
Species Mass (g)
Na+ 0.39
Cl- 0
NO3- 0.39
Ag+ 0
AgCl(s) 1.22
2.)
a. To calculate the grams of Silver Nitrate needed to completely react with Sodium Chloride:
First, we must find the moles of Sodium Chloride: 2.00g / (58.44g/mol) = 0.034 moles
The reaction follows a 1:1 ratio, therefore, we need 0.034 moles of Silver Nitrate.
To find the mass of AgNO3 needed: 0.034 moles * (169.88g/mol) = 5.77g
b. We add 5.77g of Silver Nitrate to the solution in the virtual lab. After the reaction, the amounts of Ag+ and Cl- in the solution are both less than 0.01g, confirming the reaction was complete.
3.) To calculate the grams of AgCl formed when excess NaCl is added to the 3.00g AgNO3 solution:
First, find the moles of AgNO3: 3.00g / (169.88g/mol) = 0.0176 moles
The reaction follows a 1:1 ratio, so 0.0176 moles of AgCl will be formed.
To find the mass of AgCl: 0.0176 moles * (143.32g/mol) = 2.52g
So, 2.52g of AgCl(s) will be formed.
4.) To check the answer in 3(a) using the virtual lab:
- Add excess NaCl to the 3.00g AgNO3 solution.
- Allow the reaction to complete.
- Use the solution viewer to measure the mass of the solid AgCl formed.
- The resulting mass of AgCl is 2.52g, confirming the calculated value in 3(a).
Visit: VIRTUAL LAB: Textbook Style Limiting Reagents Problems on Chem collective
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Please use the HELP tab for information on how to pour one solution to another.
1.) Use the virtual lab to answer the questions below.
a. The solution labeled "1.00g NaCl" contains 1.00g of NaCl dissolved in water. Use the solution viewer to determine the number of grams of Na+ and Cl- in the solution, and confirm that these add to 1.00g.
b. The solution labeled "1.00g AgNO3" contains 1.00g of solid AgNO3. Add 100ml of water to this solution. Use the solution viewer to determine the number of grams of Ag+ and NO3- in the solution.
c. Now add the 1.00g of solid AgNO3 to the 1.00g solution of NaCl. Write down the mass of each species in solution and the mass of solid AgCl formed. Confirm that the amounts of these species are consistent with what you say in parts (2) and (3).
Table 1: Mass of each species after reaction (2.5 marks)
Species Mass (g)
Na+
Cl-
NO3-
Ag+
AgCl(s)
2.) The solution labeled "Solution 1" in the virtual lab stockroom contains 2.00 grams of Sodium Chloride.
a. How many grams of Silver Nitrate must be added to the solution to completely react with Sodium Chloride according to the reaction above? Show your calculations. _____ (1 mark)
b. Use the virtual lab to add that amount of Silver Nitrate to the solution. Check to make sure the reaction was complete, by making sure the amount of Ag+ and Cl- in the solution are both less than 0.01g.
3.) The solution labeled "Solution 2" in the virtual lab stockroom contains 3.00 grams of AgNO3.
If excess NaCl is added to the solution, how many grams of AgCl(s) will be formed? Show your calculations. _____
4.) Use the virtual lab to check your answer to 3 (a). Explain the laboratory procedure you used to perform this check.
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