if the concentration of nitrate ions in a solution of copper (II) nitrate is 0.50 mol/L what is the concentration of the copper (II) ions in the solution??
A. 0.075 mol/L
B. 0.25 mol/L
C. 1.00 mol/L
D. 0.50 mol/L
Thanks I just dont get how to do it :(
A. 0.075 mol/L
B. 0.25 mol/L
C. 1.00 mol/L
D. 0.50 mol/L
Thanks I just dont get how to do it :(
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Well first, we need to write out the formula for the solution. Since copper has a +2 charge, as you can see from the (II) in the name, and nitrate (NO3) has a -1 charge, the formula is: Cu(NO3)2. We know that there is 0.5mol/L of nitrate, and that (thanks to the formula) the the ratio between NO3- and Cu is 1:2. We can multiply the 0.5mol/L by our ratio of 1/2, and our result is: 0.5 x 1/2 = 0.25. I hope this helped you understand it a little better!
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I'm no chemist and the last class I had in it was a very long time ago. So I haven't kept up to date and you'd be very wise to think about my logic here before embracing any of it. That said, here goes:
Ask yourself, "How many moles of Cu(NO3)2 are needed to produce 0.5 mole of NO3?" Well, since you get two moles of NO3 for one mole of Cu(NO3)2, you'd only need 0.25 mole of Cu(NO3)2 to get 0.5 moles of NO3. But there is only one Cu, so you'd have 0.25 mole of Cu. So the answer is B -- in my poorly educated opinion.
By the way, the molar mass of anything you can enter there may be found at the web site below.
Ask yourself, "How many moles of Cu(NO3)2 are needed to produce 0.5 mole of NO3?" Well, since you get two moles of NO3 for one mole of Cu(NO3)2, you'd only need 0.25 mole of Cu(NO3)2 to get 0.5 moles of NO3. But there is only one Cu, so you'd have 0.25 mole of Cu. So the answer is B -- in my poorly educated opinion.
By the way, the molar mass of anything you can enter there may be found at the web site below.
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wow i think i failed my chemistry final exam today... but my guess would be D. im pretty good at guessing, so give it a shot!