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K 2 Cr 2 O 7 (aq) + 2 KOH → 2 K 2 CrO 4 + H 2 O. Or, the fusion of potassium hydroxide and chromium trioxide: 2 KOH + CrO 3 → K 2 CrO 4 + H 2 O. In solution, the behavior of potassium and sodium dichromates are very similar. When treated with lead(II) nitrate, it gives an orange-yellow precipitate, lead(II) chromate.
3 c 2 h 5 oh + 2 k 2 cr 2 o 7 + 8 h 2 so 4 → 3 ch 3 cooh + 2 cr 2 (so 4) 3 + 2 k 2 so 4 + 11 h 2 o The excess dichromate is determined by titration against sodium thiosulfate . Adding the amount of excess dichromate from the initial amount, gives the amount of ethanol present.
2 CrO 2− 4 + 2 H + ⇌ Cr 2 O 2− 7 + H 2 O The predominance diagram shows that the position of the equilibrium depends on both pH and the analytical concentration of chromium. [ notes 1 ] The chromate ion is the predominant species in alkaline solutions, but dichromate can become the predominant ion in acidic solutions.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Electron configuration is also a major factor, illustrated by the fact that the rates of water exchange for [Al(H 2 O) 6] 3+ and [Ir(H 2 O) 6] 3+ differ by a factor of 10 9 also. [4] Water exchange usually follows a dissociative substitution pathway, so the rate constants indicate first order reactions.
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Aqueous solutions are dark violet and turns green when it is heated above 50 °C. [1] In addition to the dodecahydrate , the hexahydrate KCr(SO 4 ) 2 ·6H 2 O, dihydrate KCr(SO 4 ) 2 ·2H 2 O, and the monohydrate KCr(SO 4 ) 2 ·H 2 O are known.
Substance Formula 0 °C 10 °C 20 °C 30 °C 40 °C 50 °C 60 °C 70 °C 80 °C 90 °C 100 °C Barium acetate: Ba(C 2 H 3 O 2) 2: 58.8: 62: 72: 75: 78.5: 77: 75