How to calculate the volume of 0.1 M KMnO4 solution needed to oxidize 20ml of 0.2...

Question

Question

How to calculate the volume of 0.1 M KMnO4 solution needed to oxidize 20ml of 0.2 M FeSO4?

Answer 1

Answer #1

The balanced redox reaction is 5 Fe ² + + MnO4 + 84 a 55.3t & Mg 24 at 4H₂O Now, moles of te soy = 0.2 x 20 = 0.004 moles Fro thank you vmuch....

Answer 2

Similar Homework Help Questions

how many ml of a 0.050 M kMno4 solution are required to oxidize 2.00 g of feso4 in a dilute...

how many ml of a 0.050 M kMno4 solution are required to oxidize 2.00 g of feso4 in a dilute solution
How many mL of 0.265 M KMnO4 solution are needed to react with 4.42 g of...

How many mL of 0.265 M KMnO4 solution are needed to react with 4.42 g of iron (II) sulfate? 2 KMnO4 + 10 FeSO4 + 8 H2SO4 –> 5 Fe2(SO4)3 + 2 MnSO4 + K2SO4 + 8 H2O
How did they get these answers? How much volume of 0.2 M NaOH should be added...

How did they get these answers? How much volume of 0.2 M NaOH should be added to achieve the equivalence point? 50 mL 25 mL 20mL 15mL not listed here What's the pH of solution when you added 15 mL of 0.2 M NaOH solution to 30 mL of 0.1 M HCI solution? 16 2.8 3.8 4.8

What volume of 0.152 M KMnO4 solution would completely react with 20.0 mL of 0.381 M...

What volume of 0.152 M KMnO4 solution would completely react with 20.0 mL of 0.381 M FeSO4 solution according to the following net ionic equation? 5 Fe2+ + 8 H+ + MnO4- → 5 Fe3+ + Mn2+ + 4 H2O 4.00 mL 250 mL 50.0 mL 10.0 mL 125 mL
25. A 16.42-mL volume of 0.1327 M KMnO solution is needed to oxidize 2500 mL of...

25. A 16.42-mL volume of 0.1327 M KMnO solution is needed to oxidize 2500 mL of a FeSO: solution in an acidic medium. What is the concentration of the Feso solution in molarity? The net ionic equation is 5Fe2+ MnOr - BH - Mn + 5Fe + 4H2O [8 pts] 26. A common laboratory preparation of oxygen gas is the thermal decomposition of potassium chlorate (KCIO.). Assuming complete decomposition, calculate the number of grams of Oz gas that can be...
How to calculate the volume of 0.025 M Hcl that would completely neutralize 20ml of 0.0125M...

How to calculate the volume of 0.025 M Hcl that would completely neutralize 20ml of 0.0125M Ca(OH)2?

The titration of 50.00 mL solution of a 0.1 M OAc- with 0.2 M HCl. OAc-...

The titration of 50.00 mL solution of a 0.1 M OAc- with 0.2 M HCl. OAc- is a weak base. Ka for acetic acid = 1.75 * 10^-5. a) Calculate the pH of the 50.0 mL of 0.1 M OAc- solution before the addition of any HCl. b) Calculate the pH of the resulting solution after the addition of 5.0 mL of 0.2 M HCl to the 50.0 mL of 0.1 M OAc- solution. c) Calculate the pH of the resulting...
A weak acid, HA, is 0.1% ionized in a 0.2 M solution. Answer the following questions:...

A weak acid, HA, is 0.1% ionized in a 0.2 M solution. Answer the following questions: a) What is the equilibrium constant (Ka) for the dissociation of this acid? b) What is the pH of the solution? c) How much ‘weaker’ in active acidity of the HA solution compared to 0.2 M HCl solution? d) How many mls of 0.1 M NaOH would be needed to neutralize completely 250 ml of the 0.2 M HA solution?
Calculate pH of 0.2 M solution of Tartaric acid. Calculate the volume of 1 M solution...

Calculate pH of 0.2 M solution of Tartaric acid. Calculate the volume of 1 M solution of NaOH required to neutralize 20 mL of 0.2 M tartaric acid solution (final pH should be 7). (pKa's of Tartaric acid are 3.0 and 4.4). 3.

How many mL of 0.250 M KMnO4 are needed to react with 3.55 g of Iron...

How many mL of 0.250 M KMnO4 are needed to react with 3.55 g of Iron (II) sulfate FeSO4? The reaction is as follows: 10FeSO4(aq) + 2KMnO4(aq) + 8H2SO4(aq) → 5Fe2(SO4)3(aq) + 2MnSO4(aq) + K2SO4(aq) + 2H2O(l)