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a retro calculation of the amount of Ni(Nh3)6Cl2 that is needed if 20mL of 0.10M HCl are used to neutralize ammonia. The number I got was 0.07727 g.

So then I measured out Ni(Nh3)6Cl2 ..about 0.0776g.

Molarity of the HCl I used was 0.104M
Volume of HCl to neautralize was 18.8 mL

How do I find the mols of HCl?, (It says in the lab mols HCl = NH3) Mass of NH3, and % NH3 in product?

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