AgNO3 was dissolved in water to make 10mL of solution. Then 3.0mL of that solution was used to make a new solution with a total volume of 1.000L. What was the concentration of the silver ion in the final solution?

I have no idea. You didn't give a mass of AgNO3 used. I can give you a template to use, however, if we assume the mass AgNO3 used initially was 1 gram.

Then the original concn was 1 g/10 mL = 0.1 g/mL. Then you took 3 mL of that and diluted to 1000 mL so the new concn is
0.1 g/mL x (3 mL/1000 mL) = ??

To find the concentration of the silver ion in the final solution, we need to understand the dilution process and use the concept of molarity.

Step 1: Calculate the initial concentration of AgNO3 solution:
The initial volume of the AgNO3 solution is 10 mL. However, the question does not provide the concentration of AgNO3 in that solution. Without this information, we cannot directly determine the initial concentration. We need more information or assumptions to continue.

Step 2: Calculate the final concentration of the AgNO3 solution:
Given that 3.0 mL of the initial solution was used to make a final solution with a total volume of 1.000 L, we can assume the final concentration of AgNO3 remains the same.

Using the formula:

C1V1 = C2V2

where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration, and V2 is the final volume, we can plug in the known values:

C1(3.0 mL) = C2(1.000 L)

Since we do not know the initial concentration (C1), we cannot explicitly calculate the final concentration. To continue, we need more information or additional assumptions.

Therefore, without the given initial concentration of AgNO3, we cannot determine the concentration of the silver ion in the final solution.