An unknown 0.0500 M metal nitrate solution is either cobalt(II) nitrate or iron
ID: 507049 • Letter: A
Question
An unknown 0.0500 M metal nitrate solution is either cobalt(II) nitrate or iron (III) nitrate. Both react with NaOH to form insoluble metal hydroxides (see Eqs. 12 and 13). 10.00 mL of 0.0500 M an unknown metal nitrate solution is titrated with 0.100 M NaOH solution (see titration curve below). A. Calculate the number of mole of unknown metal ion solution used in the reaction. B. Calculate the number of moles of NaOH needed to completely precipitate the metal ions from solution. C. Calculate the ratio of moles NaOH to moles unknown metal nitrate solution. D. Is the unknown metal nitrate solution Co(NO_3)_3 or Fe(NO_3)_3?Explanation / Answer
From the titration curve and the data given above,
A. moles of metal ion in solution = molarity x volume
= 0.05 M x 10 ml
= 0.5 mmol
B. moles of NaOH needed to precipitate metal ion = molarity of NaOH x volume at equivalence point
= 0.1 M x 15.1 ml
= 1.51 mmol
C. ratio (moles NaOH/moles metal ion) = 1.51/0.5
= 3.02
D. Unknown metal nitrate in solution = Fe(NO3)3
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