AP Chemistry basic reaction problem

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SUMMARY

The discussion focuses on the reaction between cobalt(II) nitrate and sodium hydroxide, highlighting the solubility rules for hydroxides. When these solutions are mixed, cobalt(II) hydroxide precipitates while sodium nitrate remains soluble. The reaction is characterized as a neutralization process, where cobalt(II) nitrate, being acidic, reacts with the alkali sodium hydroxide, potentially leading to thermal decomposition of cobalt(II) hydroxide into cobalt oxide and water.

PREREQUISITES
  • Understanding of acid-base reactions
  • Knowledge of solubility rules for hydroxides
  • Familiarity with precipitation reactions
  • Basic concepts of thermal decomposition in chemistry
NEXT STEPS
  • Study the solubility rules for common hydroxides
  • Learn about neutralization reactions in aqueous solutions
  • Explore the thermal decomposition of metal hydroxides
  • Review the properties and reactions of cobalt compounds
USEFUL FOR

High school students taking AP Chemistry, chemistry educators, and anyone interested in understanding acid-base reactions and precipitation processes in aqueous solutions.

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Homework Statement



Solutions of cobalt(II) nitrate and sodium hydroxide are mixed.
What are the solubility rules for the hydroxides?

and it occurs in a aqueous solution

Homework Equations



I have no idea how to solve these problems from my chem class lasty year and we will be getting a problem similar to this tommorow (first day AP Chem class) and I was woundering if anyone could walk me through the steps you need to know to solve this and the answer.

The Attempt at a Solution

 
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Cobalt (II) Nitrate is acidic, and Sodium Hydroxide is an alkali, so they will undergo neutralization reaction. Sodium Nitrate will form and Cobalt Hydroxide will precipitate. It is possible that some Cobalt Hydroxide can undergo thermal decomposition into Cobalt oxide and water due to exothermic neutralization reaction.
 

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