Question

Use the References to access important value needed for this question. A student weighs out a 10.7 g sample of Ni(CH, C00)2, transfers it to a 300. ml. volumetric flask, adds enough water to dissolve it and then adds water to the 300. mL tick mark. What is the molarity of nickel(II) acetate in the resulting solution? Volanty Molarity = M Submit Answer Retry Entire Group 9 more group attempts remaining

Answer 1

Mass of Ni (CH₃COO) ₂ = 10.7 g

Molar mass of Ni (CH₃COO) ₂ = 58.71 + ( 4 $\times$ 12.01 ) + ( 6 $\times$ 1.0079) + ( 4 $\times$ 16.00 ) = 176.80 g/mol

We have, No. of moles = Mass / Molar mass

$\therefore$ No. of moles of Ni (CH₃COO) ₂ = 10.7 g / ( 176.80 g / mol) = 0.06052 mol

Volume of solution = 300.0 ml = 0.3000 L

We have, [Ni (CH₃COO) ₂ ] = No. of moles of Ni (CH₃COO) ₂ / volume of solution in L

[Ni (CH₃COO) ₂ ] = 0.06052 mol / 0.3000 L = 0.202 M

ANSWER : Molarity = 0.202 M