Describe how would you prepare .005M solution of IO3^-1 starting with potassium iodate KIO3

I am thinking I need to work backwords on this problem so here is my math if anyone can confirm it for me that would be great.

.005M IO3-1 * .5 Lsolutions = .0025 moles of IO3-1

Then I took .0025 mol IO3= .0025 mol KIO3

Then I took .0025 mol KIO3 * 214.001 g/mol=.535g KIO3

pretty much I do not know if this is all the professor is looking for but I do not know where else to go from here.

Yes, the math is correct for 500 ml. of 0.005 M/l. solution. Since 500 ml is not specified in the question, you have to mention it somewhere in your answer.

Also, since this is a chemistry question, you need to describe fully how to do this, the aparatus required, the precautions necessary to fill up exactly to 500 ml, temperatures, etc.
You can read up articles on titration and how to prepare the solutions, for example:
http://en.wikipedia.org/wiki/Titration

Thank you

To prepare a 0.005 M solution of IO3^-1 using potassium iodate (KIO3), you will need to follow these steps:

1. Determine the molar mass of KIO3: The molar mass of potassium iodate (KIO3) is calculated by adding the atomic masses of each element present in the compound. The atomic mass of potassium (K) is approximately 39.1 g/mol, iodine (I) is approximately 126.9 g/mol, and oxygen (O) is approximately 16.0 g/mol. So, the molar mass of KIO3 is (39.1 + 126.9 + (16.0 × 3)) g/mol.

2. Calculate the volume of KIO3 needed: To prepare a 0.005 M solution, we use the formula M1V1 = M2V2, where M1 is the initial molar concentration (0.005 M), V1 is the volume of the solution we want to prepare (in liters), M2 is the molar concentration of the solute (which is KIO3), and V2 is the volume of the solute (in liters).

Since we want to prepare 0.005 M solution and the molar concentration of KIO3 is equal to its molar concentration in the solution, M1 and M2 are both 0.005 M. Let's assume we want to prepare 1 liter of the solution, which means V1 is 1 liter (L).

Using the formula, we can rearrange it to solve for V2: V2 = (M1V1) / M2. Substituting the values, V2 = (0.005 M × 1 L) / 0.005 M.

Therefore, the volume of KIO3 needed is 1 liter (L).

3. Weigh the required amount of KIO3: Since the molar mass of KIO3 is known, we can calculate the mass of KIO3 needed using the formula: mass = molar mass × volume.

The molar mass of KIO3 was determined in step 1, and the volume of KIO3 needed is 1 liter (L). Plug in these values to calculate the mass of KIO3 required.

4. Dissolve KIO3 in the appropriate amount of water: Weigh out the calculated mass of KIO3 and add it to a beaker. Then, add a sufficient amount of distilled water to dissolve the KIO3 completely. Stir the solution gently until the KIO3 is fully dissolved.

5. Dilute the solution: If you need less than 1 liter of the 0.005 M solution, you can use a volumetric flask or a graduated cylinder to measure the desired volume accurately. Make sure to consider the final desired volume and adjust the amount of water accordingly.

Remember to wear appropriate protective equipment, such as gloves and goggles, while handling chemicals. Also, ensure that you are using accurate measuring equipment and following proper laboratory techniques.