Answer:
0.0812 grams of nitrate ions are there in the final solution.
Explanation:
Mass of cobalt (II) nitrate = 3.00 g
Moles of cobalt(II) nitrate =
Volume of the solution = 100 mL = 0.100 L
1 mL = 0.001 L
Molarity of the solution =
Cobalt (II) nitrate in its aqueous solution gives 1 mole of cobalt(II) ion and 2 moles of nitrate ions.
Molarity of the nitrate ion before solution =
Volume of the nitrate ion before solution =
Molarity of the nitrate ion after solution =
Volume of the nitrate ion after solution =
( Dilution)
Moles of nitrate ions in 275 ml = n
Molarity of the nitrate ion after solution =0.00477 M
volume of the final solution = 275 mL = 0.275 L
Mass of 0.00131 moles of nitrate ions:
0.00131 mol × 62 g/mol = 0.0812 g
0.0812 grams of nitrate ions are there in the final solution.