Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: kamehamehaaa on September 24, 2006, 10:33:11 PM
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Hello can someone help me calculate the mass of Cu(NO3)23H2O needed to prepare 50.0mL of a .50 M Cu(II) solution?
I would appreciate it if you can help me through this problem by telling me what I should do rather than give me the answer.
Thanks
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Do you know how to figure out what the molar mass of Cu(NO3)2*3H2O is?
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Yeah I got the molar mass to be 241.599 grams, but I don't know how to set it up from there.
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i'm not sure if i'm right :-\ . but i think first of all , you would have to write a balanced chemical equation .from that you can figure it out. i think so. :P
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Yeah I got the molar mass to be 241.599 grams, but I don't know how to set it up from there.
How would you go from here in the case of Cu(NO3)2?
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The molar mass would be 241.599 g/mol
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Yeah I got the molar mass to be 241.599 grams, but I don't know how to set it up from there.
When Copper (II) Nitrate dissolves, how many moles of Cu2+ are released per mole of Cu(NO3)2?