The formate ion, (CHO2-), is related to the acetate ion and forms ionic salts with many metal ions. Assume that 9.7416 g of M(CHO2)2 (where M represents the atomic symbol for a particular metal) are dissolved in water. When a solution of 0.200 M sodium sulfate is added, a white precipitate forms. The sodium sulfate solution is added until no more precipitate forms, then a few excess milliliters are added. The precipitate is filtered, washed, and dried. It has a mass of 9.389 g. The filtrate is placed aside.
A potassium permanganate solution is standardized by dissolving 0.9234 g of sodium oxalate in dilute sulfuric acid, which is then titrated with the potassium permanganate solution. The principal products of the reaction are manganese(II) ion and carbon dioxide gas. It requires 18.55 mL of the potassium permanganate solution to reach the end point, which is characterized by the first permanent, but barely perceptible, pink (purple) color of the permanganate ion.
The filtrate from the original reaction is diluted by pouring all of it into a 250-mL volumetric flask, diluting to the mark with water, then mixing thoroughly. Then 10.00 mL of this diluted solution is pipetted into a 125-mL Erlenmeyer flask, approximately 25 mL of water is added, and the solution is made basic. What volume of the standard permanganate solution will be needed to titrate this solution to the end point? The principal products of the reaction are carbonate ion and manganese(IV) oxide. Find M.
I haven't worked the problem; however, I have a few observations to make.
Paragraph 1 is all you need to identify M; but, I question the numbers. The formate ion has an ionic mass of 45 and two of them makes 90. Thus the molar mass of M(CHO2)2 is M + 90. When M forms the sulfate the new molar mass of the sulfate is M + 96. The way I see it; the sulfate must weigh more than the formate. According to the post the sulfate weighs less. Unless I've missed something the numbers just don't add up. That plus the fact that the mass of the formate is given to five places while the sulfate ppt is given to only four makes me suspicious that one digit may have been omitted from the sulfate ppt mass.
The purpose of paragraph 2 is to determine the molarity of KMnO4.
The purpose of paragraph 3 is to determine the mL KMnO4 needed to titrate the formate placed there by the actions in paragraph 1.
I would be interested in knowing what others think.
I have the same problem and the mass is larger after the precipitate is filtered washed and dried. I have 9.9389 on my paper. I think the person who posted the question mistyped the number
To find the volume of the standard permanganate solution needed to titrate the solution in the Erlenmeyer flask, we need to use the information given in the problem.
First, let's list the relevant information provided:
Mass of M(CHO2)2 = 9.7416 g
Mass of precipitate after filtration and drying = 9.389 g
Volume of the filtrate = 250 mL
Volume of the solution pipetted into the Erlenmeyer flask = 10.00 mL
Volume of water added to the Erlenmeyer flask = 25 mL
Volume of standard permanganate solution used to titrate sodium oxalate = 18.55 mL
Now, let's start by calculating the number of moles of M(CHO2)2 used:
1. Determine the molar mass of M(CHO2)2:
The molar mass of M(CHO2)2 is calculated by summing the atomic masses of each element in the formula: M + 2(C) + 2(H) + 2(O)
You may need to refer to the periodic table to find the atomic masses of the elements. Add the masses together to get the molar mass.
2. Calculate the number of moles of M(CHO2)2:
To calculate the moles, divide the mass of M(CHO2)2 by its molar mass.
Next, let's calculate the concentration of M(CHO2)2 in the filtrate:
3. Calculate the number of moles of M(CHO2)2 in the filtrate:
To calculate the moles, multiply the moles of M(CHO2)2 (calculated in the previous step) by the dilution factor, which is the volume of the filtrate divided by the volume pipetted into the Erlenmeyer flask.
4. Calculate the concentration of M(CHO2)2 in the filtrate:
To calculate the concentration, divide the moles of M(CHO2)2 in the filtrate by the volume of the filtrate.
Now we can calculate the moles of sodium oxalate used to standardize the potassium permanganate solution:
5. Calculate the number of moles of sodium oxalate:
To calculate the moles, divide the mass of sodium oxalate by its molar mass.
Finally, let's find the concentration of the potassium permanganate solution:
6. Calculate the concentration of the potassium permanganate solution:
To calculate the concentration, divide the moles of sodium oxalate by the volume of the potassium permanganate solution used.
Now that we have the concentration of the potassium permanganate solution, we can use it to calculate the volume needed to titrate the solution in the Erlenmeyer flask:
7. Calculate the volume of the potassium permanganate solution needed:
To calculate the volume, multiply the concentration of the potassium permanganate solution by the moles of carbonate ion present in the solution in the Erlenmeyer flask.
Please note that step 7 requires additional information about the reaction between potassium permanganate and carbonate ion, which is not provided in the question. You will need to look up the balanced equation or obtain that information from another source to complete step 7.
By following these steps, you should be able to find the volume of the standard permanganate solution needed to titrate the solution in the Erlenmeyer flask.