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 9.9389 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.
wait I found M to be Pb, but I don't know what to do next.
I'll help you do the first part and leave the second part for you.
The first part is the formation of MSO4.
mass MSO4 = 9.9389
mass M(CHO2) = 9.7416.
You can identify M from this.
9.9389 x (molar mass of the Mformate)/(molar mass MSO4) = 9.7416
Substitute for molar mass of the Mformate (M + 90) which is the molar mass M + molar mass of 2*formate.
Substitute for MSO4 (M + 96) which is molar mass M + molar mass of SO4^2-.
Solve for M. I think it is Pb.
Now you do the second part. The permanganate will oxidize the formate. Post your work if you get stuck.
To determine the volume of the standard permanganate solution needed to titrate the diluted solution to the end point, we need to calculate the number of moles of the reacting species in both solutions.
1. Calculate the number of moles of sodium oxalate in the sodium oxalate solution:
- Given mass of sodium oxalate = 0.9234 g
- Molar mass of sodium oxalate = 134.00 g/mol
- Number of moles of sodium oxalate = (0.9234 g) / (134.00 g/mol) = 0.006895 mol
2. Determine the stoichiometry of the reaction between sodium oxalate and potassium permanganate:
- From the balanced equation, we know that 5 moles of sodium oxalate react with 2 moles of potassium permanganate to form 10 moles of manganese(II) ion and 10 moles of carbon dioxide gas.
3. Convert moles of sodium oxalate to moles of potassium permanganate:
- Since the stoichiometry ratio between sodium oxalate and potassium permanganate is 5:2, the number of moles of potassium permanganate required to react with the sodium oxalate is: (5/2) × 0.006895 mol = 0.0172375 mol
4. Calculate the concentration of the potassium permanganate solution:
- Volume of potassium permanganate solution used = 18.55 mL = 0.01855 L
- Concentration of potassium permanganate solution = 0.0172375 mol / 0.01855 L = 0.93071 M
5. Determine the number of moles of manganese(IV) oxide formed in the diluted solution:
- Based on the stoichiometry of the balanced equation, 2 moles of potassium permanganate react to produce 1 mole of manganese(IV) oxide.
- The number of moles of manganese(IV) oxide formed = 0.0172375 mol / 2 = 0.0086188 mol
6. Find the volume of the diluted solution used for titration:
- Volume of the diluted solution used = 10.00 mL = 0.01000 L
7. Calculate the volume of the standard permanganate solution required:
- Volume of the standard permanganate solution required = (0.0086188 mol) / (0.93071 M) = 0.009267 L = 9.267 mL (rounded to three decimal places)
Therefore, approximately 9.267 mL of the standard permanganate solution will be needed to titrate the diluted solution to the end point.
To determine the volume of standard permanganate solution needed to titrate the solution in the 125-mL Erlenmeyer flask, we can use the stoichiometry of the reaction and the balanced equation between the permanganate ion and the carbonate ion.
The balanced equation between the permanganate ion (MnO4-) and the carbonate ion (CO3^2-) is as follows:
2 MnO4- + 5 CO3^2- + 6 H+ → 2 MnO2 + 5 CO2 + 3 H2O
From the information given, we know that it requires 18.55 mL of the potassium permanganate solution (MnO4-) to reach the end point when titrating the sodium oxalate solution. Now we need to determine the volume of the standard permanganate solution needed to titrate the solution in the 125-mL Erlenmeyer flask.
First, let's calculate the number of moles of sodium oxalate (Na2C2O4) used in the titration:
molar mass of Na2C2O4 = 22.99 g/mol (2 Na) + 12.01 g/mol (C) + 16.00 g/mol (2 O) + 16.00 g/mol (2 O) = 134.00 g/mol
moles of Na2C2O4 = mass / molar mass = 0.9234 g / 134.00 g/mol = 0.00689 mol
According to the balanced equation, the ratio between the moles of Na2C2O4 and the moles of MnO4- is 1:2. Therefore, the number of moles of MnO4- used in the titration is:
moles of MnO4- = 2 * moles of Na2C2O4 = 2 * 0.00689 mol = 0.01378 mol
Now, let's calculate the concentration of the standard permanganate solution (KMnO4):
volume of KMnO4 = 18.55 mL = 0.01855 L
moles of MnO4- = 0.01378 mol
concentration of KMnO4 = moles / volume = 0.01378 mol / 0.01855 L = 0.744 M
We now have the concentration of the standard permanganate solution. To determine the volume needed to titrate the solution in the 125-mL Erlenmeyer flask, we can use the stoichiometry of the reaction.
According to the balanced equation, the ratio between the moles of MnO4- and the moles of CO3^2- is 2:5. Therefore, the number of moles of CO3^2- in the 10.00 mL of the diluted solution in the Erlenmeyer flask is:
moles of CO3^2- = (0.744 M) * (0.01000 L) * (5 moles CO3^2- / 2 moles MnO4-) = 0.0186 mol
Now, let's calculate the volume of the standard permanganate solution needed to titrate the solution in the 125-mL Erlenmeyer flask:
volume of KMnO4 = moles / concentration = 0.0186 mol / 0.744 M = 0.025 L = 25 mL
Therefore, the volume of the standard permanganate solution needed to titrate the solution in the 125-mL Erlenmeyer flask is 25 mL.