- #1
higherme
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Question:
Given
mass of hexaammine complex [Ni(NH3)6](NO3)2 is 0.0937 g
mass of Ni2+ is 0.0193 g
if the mass of [Ni(NH3)6](NO3)2 was 0.0886 g instead of 0.937g, this would indicate that the hexaammine complex was not pure and some ammonia had been lost. Calculate the value of n in the formula [Ni(NH3)n](NO3)2
my attempt:
- Take the mass of Ni2+ and find the moles of it using Ni2+ molar mass. This mole would then be the same as the moles of the complex (1:1 ratio) --> i found to be 0.0003288 moles
- then take the grams of the complex 0.0886 g and divide by that mole: 0.0886g/0.0003288moles = 264.4404 g/mol which would be the molar mass of the complex
- then i subtracted the molar masses of Ni2+ and (NO3)2 from that molar mass and what is left is the amount of (NH3)n. Then i took that amount and divided by the molar mass of one NH3 to see how many NH3 I have.
am I thinking right?
Given
mass of hexaammine complex [Ni(NH3)6](NO3)2 is 0.0937 g
mass of Ni2+ is 0.0193 g
if the mass of [Ni(NH3)6](NO3)2 was 0.0886 g instead of 0.937g, this would indicate that the hexaammine complex was not pure and some ammonia had been lost. Calculate the value of n in the formula [Ni(NH3)n](NO3)2
my attempt:
- Take the mass of Ni2+ and find the moles of it using Ni2+ molar mass. This mole would then be the same as the moles of the complex (1:1 ratio) --> i found to be 0.0003288 moles
- then take the grams of the complex 0.0886 g and divide by that mole: 0.0886g/0.0003288moles = 264.4404 g/mol which would be the molar mass of the complex
- then i subtracted the molar masses of Ni2+ and (NO3)2 from that molar mass and what is left is the amount of (NH3)n. Then i took that amount and divided by the molar mass of one NH3 to see how many NH3 I have.
am I thinking right?