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Why is Brown turbidity sometimes seen while titrating KMnO4 solution with oxalic acid?
Brown turbidity may be observed when titrating KMnO4 with oxalic acid due to the formation of manganese dioxide (MnO2) as a byproduct. This occurs when excess oxalic acid reduces MnO4- to Mn2+ ions, which then react with oxygen in the air to form manganese dioxide. The brown color of MnO2 leads to turbidity in the solution.
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Why brown turbidity found in titrating KMno4 with oxalic acid?
Brown turbidity in the titration of KMnO4 with oxalic acid may be due to the formation of manganese dioxide (MnO2). This reaction occurs in acidic conditions and indicates that the end point of the titration has been reached. MnO2 is insoluble and can appear as a brown precipitate, causing turbidity in the solution.
Is it necessary to know the exact concentration of oxalic acid to determine the concentration of the base?
No, it is not necessary to know the exact concentration of oxalic acid if you are titrating it with a base. You can determine the concentration of the base by measuring the volume of the base solution required to neutralize the acid solution.
Calculate the required amount of oxalic aciddihydrate to prepare 200 mL of 0.50M oxalic acid solution?
To prepare 200 mL of 0.50M oxalic acid solution, you would need 0.1 moles of oxalic acid. Since oxalic acid is a dihydrate (H2C2O4·2H2O), you would need to account for the water content. The molar mass of oxalic acid dihydrate is 126.07 g/mol, so you would need 12.607 grams of oxalic acid dihydrate to prepare the solution.
How do you prepare saturated solution given 1gram of oxalic acid in 7g of water?
To prepare a saturated solution of oxalic acid, dissolve 1 gram of oxalic acid in 7 grams of water at a given temperature until no more oxalic acid can dissolve. This will result in a saturated solution where the maximum amount of oxalic acid has dissolved in the water at that temperature.
How prepare 0.1 N oxalic acid?
To prepare 0.1 N oxalic acid solution, you would need to dissolve 0.634 g of oxalic acid dihydrate (H2C2O4·2H2O) in distilled water and make up the solution to a final volume of 1 liter. This will give you a 0.1 N (normality) solution of oxalic acid.
Why brown turbidity found in titrating KMno4 with oxalic acid?
Brown turbidity in the titration of KMnO4 with oxalic acid may be due to the formation of manganese dioxide (MnO2). This reaction occurs in acidic conditions and indicates that the end point of the titration has been reached. MnO2 is insoluble and can appear as a brown precipitate, causing turbidity in the solution.
Is it necessary to know the exact concentration of oxalic acid to determine the concentration of the base?
No, it is not necessary to know the exact concentration of oxalic acid if you are titrating it with a base. You can determine the concentration of the base by measuring the volume of the base solution required to neutralize the acid solution.
How do you determine the pka of oxalic acid?
To determine the pKa of oxalic acid, you can perform a titration experiment. By titrating a solution of oxalic acid with a strong base such as sodium hydroxide (NaOH) and monitoring the pH changes, you can identify the point where the acid is half-neutralized and calculate the pKa value. This is typically done using a pH meter or pH indicator to track the changes in acidity as the titration progresses.
Calculate the required amount of oxalic aciddihydrate to prepare 200 mL of 0.50M oxalic acid solution?
To prepare 200 mL of 0.50M oxalic acid solution, you would need 0.1 moles of oxalic acid. Since oxalic acid is a dihydrate (H2C2O4·2H2O), you would need to account for the water content. The molar mass of oxalic acid dihydrate is 126.07 g/mol, so you would need 12.607 grams of oxalic acid dihydrate to prepare the solution.
How do you prepare saturated solution given 1gram of oxalic acid in 7g of water?
To prepare a saturated solution of oxalic acid, dissolve 1 gram of oxalic acid in 7 grams of water at a given temperature until no more oxalic acid can dissolve. This will result in a saturated solution where the maximum amount of oxalic acid has dissolved in the water at that temperature.
How prepare 0.1 N oxalic acid?
To prepare 0.1 N oxalic acid solution, you would need to dissolve 0.634 g of oxalic acid dihydrate (H2C2O4·2H2O) in distilled water and make up the solution to a final volume of 1 liter. This will give you a 0.1 N (normality) solution of oxalic acid.
How do you prepare saturated oxalic acid?
To prepare saturated oxalic acid solution, simply add oxalic acid powder to water in a container and stir until no more dissolves. This will result in a saturated solution where the water has dissolved as much oxalic acid as it can at that temperature. It's important to wear appropriate protective gear when handling oxalic acid as it can be harmful if not handled properly.
Could you prepare oxalic acid by adding hcl to a solution og sodium oxalate?
Yes, oxalic acid can be prepared by adding hydrochloric acid (HCl) to a solution of sodium oxalate. The reaction that occurs is double displacement reaction where sodium chloride and oxalic acid are formed. Oxalic acid can be obtained by precipitating it out of the solution by adjusting the pH.
What is the enthalpy change of solution of oxalic acid?
Enthalpy of solution of oxalic, succinic, adipic, maleic, malic, tartaric, and citric acids, oxalic acid dihydrate, and citric acid monohydrate in water at 298.15 K
Which of the following might you use to titrate an oxalic acid solution?
You could use a standardized solution of potassium permanganate (KMnO4) to titrate an oxalic acid solution. Potassium permanganate is a strong oxidizing agent that reacts with oxalic acid in an acidic medium, forming carbon dioxide gas, manganese dioxide, and water.
How many milliliters of a 0.270 M solution are needed to react completely with 3.245 g of oxalic acid?
To determine the volume of 0.270 M solution needed to react completely with 3.245 g of oxalic acid, first calculate the number of moles of oxalic acid (by dividing the mass by its molar mass). Then, use the mole ratio between the acid and the solution (from the balanced chemical equation) to find the moles of solution required. Finally, use the molarity to calculate the volume using the formula: volume (in liters) = moles / molarity. Convert the volume to milliliters, if needed.
Why addition of water to oxalic doesn't affect the molarity?
Adding water to a solution of oxalic acid does not affect its molarity because the total number of moles of oxalic acid in the solution remains the same. Molarity is calculated based on the number of moles of solute divided by the volume of the solution, so as long as the number of moles of oxalic acid stays constant, the molarity remains unchanged.
