What is the balanced equation of NaOH+NiCl2, I'm not understanding my on line lab question, please help!!

Thank you for posting your question to the Ask Me Help Desk.

Here are some steps to help you.

1. Use the general equation for this type of reaction to help you in finishing the equation.

AB + CD --> AD + CB

2. Remember that all oxidation numbers must zero out when writing the formulas.

3. Balance using the proper rules.

Let me know what you come up with.

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Originally Posted by budnip

What is the balanced equation of NaOH+NiCl2, I'm not understanding my on line lab question, please help!!!

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Im pretty sure you need to know what that yeilds... is it a double replacement if so.. you get NaOH + NiCl2 --> NaCl2 NiOH... I think...

Never mind actually you can't balance that because there is no reaction... OH molecules are insoluble... read solubility rules...

Quote:

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Originally Posted by paris305

Im pretty sure you need to know what that yeilds... is it a double replacement if so .. you get NaOH + NiCl2 --> NaCl2 NiOH .... i think...

Nevermind actually you can't balance that because there is no reaction... OH molecules are insoluble... read solubility rules...

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Ummm... no.

You need to understand the rules a little better.

Yes most hydroxides are insoluble... but NaOH isn't. Anyone who has taken chem lab has most likely used aqueous sodium hydroxides.. . now, many other OH salts are insoluble... its true, and relevant to this question. But your post makes it sound like the reagent isn't soluble.

Please make sure you know the answer before you post.

Quote:

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Originally Posted by budnip

What is the balanced equation of NaOH+NiCl2, I'm not understanding my on line lab question, please help!!!

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2NaOH + Ni(Cl)2 -> 2NaCl + Ni(OH)2

First of all it would be NiOH that is the product. And this is insoluble. If it's insoluble it means there is a precipitate which means there was a reaction.