Question

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.  

The solution labeled "Solution 2" in the virtual lab stockroom contains 3.00 grams of AgNO3.  

c. If excess NaCl is added to the solution, how many grams of AgCl(s) will be formed? Show your calculations. _____ (1 mark)  

d. Use the virtual lab to check your answer to 3 (a). Explain the laboratory procedure you used to perform this check. (0.5 marks)

Answer 1

a. According to the equation, NaCl + AgNO3 gives AgCl + NaNO3,

one mole of NaCl react with one mole of AgNO3

Here amount of NaCl is 2g. Converting into moles

2g of NaCl = given mass/ molar mass = 2/58.5 = 0.034 mol

Molar mass of AgNO3 = 169.87 g/mol

0.034 mol of NaCl react with 0.034 mol of AgNO3

0.034 mol of AgNO3 = number of mol * molar mass = 0.034*169.87 = 5.776 g

Therefore, 5.776 grams of Silver Nitrate must be added to the solution to completely react with 2g Sodium Chloride.

answered by: anonymous