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Consider the following reaction: Na2CO3 + NiCl2 ¨ NiCO3 + 2NaCl Using the solubility rules determine the solubility of all reactants and products. Explain your answer Please. Which product is the precipitate in this reaction? Write the complete ionic equ...

1. A solution containing 0.100 mol of Na2CO3 and 0.100 mol of NiCl2 is allowed to react. Which reactant is the limiting reactant? 2. A solution containing 0.100 mol of Na2CO3 and 0.100 mol of NiCl2 is allowed to react. How many moles of precipitate form i...

Na2CO3 + NiCl2 ¨ NiCO3 + 2NaCl Using the solubility rules determine the solubility of all reactants and products. Explain your answer. I answered Na2 as soluble, Co3 as soluble, NiCl2 as soluble ---->NiCO3 as insoluble, and 2NaCl as soluble. My explanati...

A solution containing 0.100 mol of Na2CO3 and 0.100 mol of NiCl2 is allowed to react. What mass of precipitate forms in this reaction?

A solution containing 0.100 mol of Na2CO3 and 0.100 mol of NiCl2 is allowed to react. What mass of precipitate forms in this reaction? I just don't understand how to get the answer. Can someone please show me and explain to me how to do this.

what is the complete and net ionic equation? I just done understand.... HELP please!

So the net equation is CO3^2-(aq)+Ni^2+(aq)----->NiCO3(s)

Can you explain how I get the moles and I should be able to do it from there.

Thank You that really helped

So it would be NiCl2 right?

I Think the answer is Na2CO3 but its a 1:1 ratio but I don't know if I need to find the molar masses of each compound? HELP PLEASE!