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Sagot :
Answer
5.299 grams
Explanation
Given:
Concentration of Cl⁻ = 0.059 M
Volume of solution = 462 mL = 0.462 L
What to find:
The grams of NiCl₂ in 462 mL solution
Step-by-step solution:
The first step to write a balanced equation for the dissolution of NiCl₂:
[tex]\text{NiCl}_{2(s)}\rightarrow Ni^{2+}+2Cl^-[/tex]From the balanced equation; 1 mole of NiCl₂ produces 2 moles of Cl⁻
Given that the concentration of Cl⁻ = 0.059 M, so the concentration of Ni⁺ will be:
[tex]\frac{\lbrack Cl^-\rbrack}{2}=\frac{0.059}{2}=0.0295\text{ }M\text{ }Ni^{2+}[/tex]So that Molarity, M, of NiCl₂ = 0.059 M + 0.0295 = 0.0885 M
[tex]Number\text{ of moles NiCl}_2=Molarity\times Vol\text{ume in L}[/tex]Number of moles of NiCl₂ = 0.0885 M x 0.462 L = 0.040887 mol
The last step is to convert the number of moles of NiCl₂ to grams using the formula below:
[tex]\text{Number of moles }=\frac{Mass}{Molar\text{ mass}}[/tex]From the Periodic Table;
Molar mass of NiCl₂ = 129.5994 g/mol
So, mass of NiCl₂ in 462 mL solution = 0.040887 mol x 129.5994 g/mol = 5.299 grams
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