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juin [17]
3 years ago
12

A solution is prepared by mixing 0.10 of 0.12 M sodium chloride with 0.23 L of a 0.18 M magnesium chloride solution. What is the

pCl- of the resulting solution?
Chemistry
1 answer:
Ad libitum [116K]3 years ago
7 0

Answer:

pCl⁻ = 0.54

Explanation:

First we <u>calculate how many Cl⁻ moles are coming from each substance</u>, using the <em>given volumes and concentrations</em>:

  • 0.12 M NaCl * 0.10 L = 0.012 mol NaCl = 0.012 mol Cl⁻
  • 0.18 M MgCl₂ * 0.23 L = 0.0414 mol MgCl₂ = (0.0414 * 2) 0.0828 mol Cl⁻

The final volume of the mixture is = 0.10 L + 0.23 L = 0.33 L

Now we <u>calculate [Cl⁻]</u>, using the<em> total number of Cl⁻ moles and the final volume:</em>

  • [Cl⁻] = (0.012 mol + 0.0828 mol) / 0.33 L = 0.29 M

Finally we <u>calculate the pCl⁻ of the resulting solution</u>:

  • pCl⁻ = -log[Cl⁻]
  • pCl⁻ = 0.54
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