Question

a) Use the below to fill in the graph

- 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.  

-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.  

- 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)

A solution labelled "Solution 2" contains 3.00 grams of AgNO3.  

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

c) Check your answer to a) and explain the laboratory procedure you used to perform this check. (0.5 marks)   

Answer 1

Given data is,

A solution labelled "Solution 2" contains 3.00 grams of AgNO3.  

b) If excess NaCl is added to the solution, how many grams of AgCl(s) will be formed?

AgNO3 mass = 3 gm

For 169.87 gm of AgNO3 , 58.44 gm of NaCl required

3 gm of AgNO3, NaCl required = 3*58.44/169.87

= 1.03 gm NaCl required.

58.44 gm of NaCl, AgCl produced will be 143.32 gm.

So for 1.03 gm of NaCl, AgCl produced = 1.03*143.32/58.44

= 2.52 gm.

Please post the A  and C questions seperately.