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Calculate the molarity for 25mL of H2C2O4 in a titration with 12.46mL of KMnO4

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This is a Quantitative Redox titration. (KMnO4) = 1.8 G.. 500 ML after the experiment we had to record the data of the 3 trials. 1. Trial - VolUme FeSO4 = 10.00 Ml - VOlume KMnO4 11.00 Ml 2. Trial - VolUme FeSO4 = 10.00 ML - VOlume …
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A titration. 12.46 mL of KMnO4 are titrated with 25 mL of H2C2O4. The half reaction is 2H2O+H2C2O4 ARROW 2H2CO3+2H+2e-. How do I get the molarity of H2C2O4?
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A titration. 12.46 mL of KMnO4 are titrated with 25 mL of H2C2O4. The half reaction is 2H2O+H2C2O4 ARROW 2H2CO3+2H+2e-. How do I get the molarity of H2C2O4?
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A 0.5537-g sample containing oxalic acid required 21.62 mL of 0.09377 M NaOH for titration. If the reaction is H2C2O4 + 2NaOH  Na2C2O4 + 2H2O, calculate the % H2C2O4 in the sample.
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How would the calculated molarity of KMNo4 be affected when KMno4 is added to rapidly and too much KMnO4 is added, overshooting the endpoint.
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If 8.72 grams of oxalic acid, H2C2O4, a diprotic acid, is neutralized when 23.4 mL of a solution of KOH is added, what is the molarity of KOH?
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In order to standardize a KMnO4 solution, 0.3498 g Na2C2O4 was dissolved in 30 mL water and 15 mL 3.0 M H2SO4. The KMnO4 solution was added to the Na2C2O4 solution until a pale pink color persisted. The titration took 29.5 mL of KMnO4 …
8. ### Chemistry HELP!

In order to standardize a KMnO4 solution, 0.3498 g Na2C2O4 was dissolved in 30 mL water and 15 mL 3.0 M H2SO4. The KMnO4 solution was added to the Na2C2O4 solution until a pale pink color persisted. The titration took 29.5 mL of KMnO4 …
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100mL of oxalic acid (H2C2O4) requires 35mL of 0.04M KMnO4 to titrate it to the endpoint. calculate the molarity of the oxalic acid.
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2 KMnO4 + 5 H2C2O4 + 3 H2SO4 ---> 2 MnSO4 + 10 CO2 + 8 H2O + K2SO4 How many milliliters of a 0.123 M KMnO4 solution is needed to react completely with 3.141 of oxalic acid?

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