# CHEMISTRY

1.) A solution is prepared by dissolving 5.00 g of stannic nitrate in enough water to make 250.0 mL of stock solution. A 15.0 mL aliquot (portion) of this stock solution is then removed and added to 75.0 mL of water. Calculate the concentrations of all ions in the final solution.

This is my first time learning this so please do the above as an example. I have more to do so this can be an example.

1. Step 1 is to calculate the concn of the stock solution so you will know what you're starting with.
mols Sn(NO3)4 = grams/molar mass
Step 2. The M of the stock soln is mols/L soln or mol/0.250. Let's call this y molar.

Then dilutions are handled with the dilution formula which is
c1v1 = c2v2 where
c = concn
v = volume.
In this problem you will have
15.0mL x yM = ?M x 90 mL and you solve for ?M. This is all true IF volumes are additive. Technically they are not (and they aren't here) but the difference is so small it won't make any difference. I'm sure the asker means for you to add the 75 mL to 15 mL to end up with a solution volume of 90 mL.

Now you have M of the diluted solution of Sn(NO3)4.
Since there is 1 mol Sn^4+ per 1 mol Sn(NO3)4 the M Sn^4+ is the same as M of the solution.
M of the NO3^- is 4x M of Sn(NO3)4 because there are 4 mols NO3^- for each mol Sn(NO3)4.

posted by DrBob222

## Similar Questions

1. ### Chemistry(reposts #1)

A solution is prepared by dissolving 5.00 g of stannic nitrate in enough water to make 250.0 mL of stock solution. A 15.0 mL aliquot (portion) of this stock solution is then removed and added to 75.0 mL of water. Calculate the
2. ### CHEMISTRY

Ion Concentrations 1.) A solution is prepared by dissolving 5.00 g of stannic nitrate in enough water to make 250.0 mL of stock solution. A 15.0 mL aliquot (portion) of this stock solution is then removed and added to 75.0 mL of
3. ### Chemistry

determine the molarity of a solution of silver nitrate prepared by dissolving 5g of silver nitrate in 25.0mL of water
4. ### Chemistry

What is the molarity of a solution prepared by dissolving 4.92 g of calicum nitrate in 250 mL of water?
5. ### Chemistry

A solution is prepared by dissolving 10.8 g of ammonium nitrate in enough water to make 100.0 mL of solution. A 10.0 mL portion of this sample is diluted to 50.0 mL total volume. What is the molarity of the final solution?
6. ### chem21

A potassium nitrate solution is prepared by dissolving 2.8 g of KNO3 in 27 mL of water. What is the concentration of this solution in units of grams of solute per 100 mL of solvent?
7. ### chemistry

A potassium nitrate solution is prepared by dissolving 2.3 g of KNO3 in 25 mL of water. What is the concentration of this solution in units of grams of solute per 100 mL of solvent?
8. ### AP Chem

What is the freezing point in degrees Celsius of a solution prepared by dissolving 11.3 (g) of calcium nitrate in 115 (g) of water? K of f for water is 1.86 degrees Celsius/m
9. ### chemistry

Calculate the concentration of nitrate ions, NO3- , in mol dm-3, of a solution made by dissolving 2.5000 g of ferric nitrate nonahydrate in water to give 2.000 L of solution.
10. ### Chemistry

1. A chemist prepares a solution by dissolving 4.603 g of NaNO3 in enough water to make 200 mL of solution. What molar concentration of sodium nitrate should appear on the label? Answer in units of M 2.If the chemist mistakenly

More Similar Questions