Cr(OH)3(s) + OH-(aq) in balance net ionic form. show physical form
Added by Michelle A.
Step 1
To write the balanced net ionic equation for the reaction of chromium(III) hydroxide, Cr(OH)₃(s), with hydroxide ions, OH⁻(aq), we will follow these steps: ** Show more…
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Choose the chromium hydroxide that is amphoteric, and write a balanced net ionic equation for its reaction with hydroxide ion. What is the oxidation state of the chromium and the color of the product? (a) $\mathrm{CrO}_{2}(\mathrm{OH})_{2} \quad$ (b) $\mathrm{Cr}(\mathrm{OH})_{3} \quad$ (c) $\mathrm{Cr}(\mathrm{OH})_{2}$
Cr + ClO4- -> Cr(OH)3 + ClO3- balance the equation in basic medium
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Chromium(III) hydroxide is amphiprotic. a) Write a balanced chemical equation showing how an aqueous suspension of this compound reacts to the addition of a strong acid. Use H+ to represent the strong acid. (Hint): Amphiprotic substances can behave as either an acid or a base. The formula of chromium(III) hydroxide is Cr(OH)3(s). b) Write a balanced chemical equation showing how an aqueous suspension of this compound reacts to the addition of a strong base. Use OH– to represent the strong base. (Hint): Amphiprotic substances can behave as either an acid or a base. The formula of chromium(III) hydroxide is Cr(OH)3.
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