A sample of a chromium-containing alloy weighing 3.450 g wasdissolved in acid, and all the chromium in the sample was oxidizedto 2CrO42–. It was then found that 3.18 g of Na2SO3 was required toreduce the 2CrO42– to CrO2– in a basic solution, with the SO32–being oxidized to SO42–. Write a balanced equation for the reactionof 2CrO42– with SO32- in a basic solution. How many grams ofchromium were in the alloy sample? What was the percentage by massof chromium in the alloy? Review Problem 5.097a Incorrect. Did youhave the chromium being reduced? Did you balance out the electronsproperly so none remained in the final balanced equation? Enter abalanced net ionic equation for the reaction between 2CrO42- andSO32- in a basic solution.
