The 500 ppm Cr(VI) solution was prepared from potassiumdichromate (K2Cr2O7). We

Question

The 500 ppm Cr(VI) solution was prepared from potassiumdichromate (K2Cr2O7). We measured out 100.0 mL of the Cr(VI) solution. Explain how Cr has the 6+ oxidationstate. Also, calculate how many grams of K2Cr2O7were used to prepare 1 L of solution at 500 ppm (mg/L). If you could show how to do all the math, that would begreat. Thank you. The 500 ppm Cr(VI) solution was prepared from potassiumdichromate (K2Cr2O7). We measured out 100.0 mL of the Cr(VI) solution. Explain how Cr has the 6+ oxidationstate. Also, calculate how many grams of K2Cr2O7were used to prepare 1 L of solution at 500 ppm (mg/L). If you could show how to do all the math, that would begreat. Thank you.

Explanation / Answer

The OS of K = +1 The OS of O = -2 The net charge is zero cause the molecule, including twoK, two Cr, and seven O, is neutral. So 2 x (+1) + Cr x 2 + -2 x 7 =0 Cr x 2 = 12 so Cr = +6

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