VLab: Precipitation Reactions
Unit 2 Online Simulation-II (50 points)
VLab: Precipitation Reactions: Data & Observations
Navigate to: http://www.sascurriculumpathways.com/portal/#/search?searchString=&searchSubject=3&searchCategory=20 Enter the following username: job5circle
(No password required)
Enter 867 GO
There are thirty-five combinations of aqueous solutions for you to investigate. (Note Table 1 on the Data Sheet.) Some of these combinations will produce precipitates; others will not.
Step-by-step instructions for experimenting with the first combination (AgNO3 and NaCl) are listed below. For the first solution, select AgNO3.
For the second solution, select NaCl.
The Erlenmeyer flasks that appear are filled with the two aqueous solutions.
Note the color of each solution. This information has already been recorded for you in Table 1.
If a reaction were to occur between these two aqueous solutions, what would the products be?
(Given your knowledge of exchange reactions, you should expect the products to be NaNO3 and AgCl.)
Begin building the chemical equation by dragging a sodium ion to the first product box and a nitrate ion to the second product box. Place your cursor over each ion to display its charge. Since these ions have equal but opposite charges (+1 and -1), you do not need to drag any additional ions to this area. NaNO3 is a valid chemical formula.
Finish building the chemical equation by dragging a silver ion and a chloride ion to the third and fourth product boxes, respectively. These two ions also have equal but opposite charges (+1 and -1), so you have produced another valid chemical formula.
Balance the chemical equation by selecting any needed coefficients. For this example, the equation is already balanced. (The simulation recognizes blanks as coefficients of "1.")
Select the Check button to check your work. If your product(s) had been incorrect, the product box(es) would have turned red.
VLab: Precipitation Reactions: Data & Observations
Navigate to: http://www.sascurriculumpathways.com/portal/#/search?searchString=&searchSubject=3&searchCategory=20 Enter the following username: job5circle
(No password required)
Enter 867 GO
There are thirty-five combinations of aqueous solutions for you to investigate. (Note Table 1 on the Data Sheet.) Some of these combinations will produce precipitates; others will not.
Step-by-step instructions for experimenting with the first combination (AgNO3 and NaCl) are listed below. For the first solution, select AgNO3.
For the second solution, select NaCl.
The Erlenmeyer flasks that appear are filled with the two aqueous solutions.
Note the color of each solution. This information has already been recorded for you in Table 1.
If a reaction were to occur between these two aqueous solutions, what would the products be?
(Given your knowledge of exchange reactions, you should expect the products to be NaNO3 and AgCl.)
Begin building the chemical equation by dragging a sodium ion to the first product box and a nitrate ion to the second product box. Place your cursor over each ion to display its charge. Since these ions have equal but opposite charges (+1 and -1), you do not need to drag any additional ions to this area. NaNO3 is a valid chemical formula.
Finish building the chemical equation by dragging a silver ion and a chloride ion to the third and fourth product boxes, respectively. These two ions also have equal but opposite charges (+1 and -1), so you have produced another valid chemical formula.
Balance the chemical equation by selecting any needed coefficients. For this example, the equation is already balanced. (The simulation recognizes blanks as coefficients of "1.")
Select the Check button to check your work. If your product(s) had been incorrect, the product box(es) would have turned red.