Show with balanced equations what happens when the following are mixed:

Aqueous solution of potassium chromate and acid.

None of these
$2 C r O_{4}^{2 -} + 6 H^{+} ⇌ {C r}_{2} O_{5}^{2 -} + 3 H_{2} O$ .
$2 C r O_{4}^{2 -} + 2 H^{+} ⇌ {C r}_{2} O_{7}^{2 -} + H_{2} O$ .
$2 C r O_{4}^{2 -} + 10 H^{+} ⇌ {C r}_{2} O_{3}^{2 -} + 5 H_{2} O$ .

Question

Show with balanced equations what happens when the following are mixed:

Aqueous solution of potassium chromate and acid.

None of these
$2 C r O_{4}^{2 -} + 6 H^{+} ⇌ {C r}_{2} O_{5}^{2 -} + 3 H_{2} O$ .
$2 C r O_{4}^{2 -} + 2 H^{+} ⇌ {C r}_{2} O_{7}^{2 -} + H_{2} O$ .
$2 C r O_{4}^{2 -} + 10 H^{+} ⇌ {C r}_{2} O_{3}^{2 -} + 5 H_{2} O$ .

Toppr Admin · Accepted Answer

Yellow-colored chromate changes to orange colored dichromate but chromium stays in -6 oxidation in both the compounds- 2CrO2-x2212-4-2H-x2192-Cr2O2-x2212-7-H2O

Show with balanced equations what happens when the following are mixed:Aqueous solution of potassium chromate and acid.None of these2CrO2−4+6H+⇌Cr2O2−5+3H2O.2CrO2−4+2H+⇌Cr2O2−7+H2O.2CrO2−4+10H+⇌Cr2O2−3+5H2O.

Yellow-colored chromate changes to orange colored dichromate but chromium stays in +6 oxidation in both the compounds. 2CrO2−4+2H+→Cr2O2−7+H2O

Yellow-colored chromate changes to orange colored dichromate but chromium stays in +6 oxidation in both the compounds.
$2 C r O_{4}^{2 -} + 2 H^{+} \to {C r}_{2} O_{7}^{2 -} + H_{2} O$