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Suppose 0.987 g of nickel(ii) chloride is dissolved in 150. ml of a 68.0 mm aqueous solution of potassium carbonate.rnrncalculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the nickel(ii) chloride is dissolved in it.rnrnround your answer to 3 significant digits.
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SOLUTION
First, determine the number of moles of chloride ion present in 0.987 g of nickel(II) chloride (NiCl2):
n_text{Cl}^- = 0.987 g NiCl_2 times frac{1 mol NiCl_2}{129.60 g NiCl_2} times frac{2 mol Cl^-}{1 mol NiCl_2} = 0.0152 mol Cl^-
Next, we need to account for the chloride ions already present in the 150. mL of 68.0 mM potassium carbonate (K2CO3) solution:
n_text{Cl}^- (initial) = 150 mL times frac{1 L}{1000 mL} times 68.0 mmol/L times frac{1 mol}{1000 mmol} = 0.0102 mol Cl^-
The total moles of chloride ions in the final solution is the sum of the initial moles and the moles added from NiCl2:
n_text{Cl}^- (total) = 0.0152 mol Cl^- + 0.0102 mol Cl^- = 0.0254 mol Cl^-
Finally, we can calculate the final molarity of chloride ions:
[Cl^-] = frac{0.0254 mol Cl^-}{0.150 L solution} = boxed{0.170 M}
The final molarity of chloride anion in the solution is 0.170 M.
First, determine the number of moles of chloride ion present in 0.987 g of nickel(II) chloride (NiCl2):
n_text{Cl}^- = 0.987 g NiCl_2 times frac{1 mol NiCl_2}{129.60 g NiCl_2} times frac{2 mol Cl^-}{1 mol NiCl_2} = 0.0152 mol Cl^-
Next, we need to account for the chloride ions already present in the 150. mL of 68.0 mM potassium carbonate (K2CO3) solution:
n_text{Cl}^- (initial) = 150 mL times frac{1 L}{1000 mL} times 68.0 mmol/L times frac{1 mol}{1000 mmol} = 0.0102 mol Cl^-
The total moles of chloride ions in the final solution is the sum of the initial moles and the moles added from NiCl2:
n_text{Cl}^- (total) = 0.0152 mol Cl^- + 0.0102 mol Cl^- = 0.0254 mol Cl^-
Finally, we can calculate the final molarity of chloride ions:
[Cl^-] = frac{0.0254 mol Cl^-}{0.150 L solution} = boxed{0.170 M}
The final molarity of chloride anion in the solution is 0.170 M.
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