A sample of a chromium-containing alloy weighing 3.450 g was dissolved in acid, and all the...

A sample of a chromium-containing alloy weighing 3.450 g was dissolved in acid, and all the chromium in the sample was oxidized to 2CrO42–. It was then found that 3.18 g of Na2SO3 was required to reduce the 2CrO42– to CrO2– in a basic solution, with the SO32– being oxidized to SO42–. Write a balanced equation for the reaction of 2CrO42– with SO32- in a basic solution. How many grams of chromium were in the alloy sample? What was the percentage by mass of chromium in the alloy? Review Problem 5.097a Incorrect. Did you have the chromium being reduced? Did you balance out the electrons properly so none remained in the final balanced equation? Enter a balanced net ionic equation for the reaction between 2CrO42- and SO32- in a basic solution.

Expert Solution

write the balanced equation in the basic medium and then calculate the moles required and then calculate the mass and mass percent as follows

queen_honey_blossom answered 1 year ago

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