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AURORKA [14]
3 years ago
12

You have an aqueous solution of chromium(III) nitrate that you titrate with an aqueous solution of sodium hydroxide. After a cer

tain amount of titrant has been added, you observe a precipitate forming. You add more sodium hydroxide solution and the precipitate dissolves, leaving a solution again. What has happened?1) The precipitate was chromium hydroxide, which then reacted with more hydroxide to produce a soluble complex ion, Cr(OH)4?.2) The precipitate was chromium hydroxide, which dissolved once more solution was added, forming Cr3+(aq).3) The precipitate was sodium nitrate, which reacted with more nitrate to produce the soluble complex ion Na(NO3)2?.4) The precipitate was sodium hydroxide, which re-dissolved in the larger volume.
Chemistry
1 answer:
barxatty [35]3 years ago
7 0

Answer:

The precipitate was chromium hydroxide, which then reacted with more hydroxide to produce a soluble complex, Cr(OH)4

Explanation:

The following reaction takes place when chromium(III) nitrate reacts with NaOH:

Cr(NO)_{3} +3 NaOH → Cr(OH)_{3} (s)+ NaNO_{3}

The precipitate that is formed is chromium hydroxide, Cr(OH)_{3}

When more NaOH is added, the precipitate reacts with it which then results in the formation of a soluble complex ion:

Cr(OH)_{3}(s) + OH^{-}(aq) → Cr(OH)_{4} ^{-}(aq)

Cr(OH)_{4} ^{-} is soluble complex ion

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