Suppose 2.90g of nickel(II) iodide is dissolved in 150ml of a 0.70M aqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the nickel(II) iodide is dissolved in it. Round your answer to 3 significant digits.
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Ответ:
0.124 M.
Explanation:
Hello!
In this case, since the nickel iodide has the following formula:
NiI₂
So its molar mass is 312.5023 g/mol, in order to compute the molarity of the iodide anion, we first need the moles in 2.90 g:
Now, since one mole of nickel(II) iodide contains two mole of iodide anions, we infer there are 0.0186 moles of iodide cations. Moreover, since the molarity is computed by dividing the moles of those ones by the volume of the solution in liters, 150 mL (0.150 L) as it does not change, it turns out:
Best regards!
Ответ:
Hey there!
I am not the greatest in this subject but I believe that 2C2H2+502 is balanced!
If i am incorrect, I am very sorry and would love any feedback!
Hope i made your day easier.
Have a nice day and happy Halloween!