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julsineya [31]
3 years ago
8

Question 8 4 pts What would be the resulting molarity of a solution made by dissolving 31.3 grams of Ca(OH)2 in enough water to

make a 1050-milliliter solution? Show all of the work needed to solve this problem.
Chemistry
2 answers:
Tcecarenko [31]3 years ago
4 0

Answer : The molarity of the solution is, 0.4028 mole/L

Explanation : Given,

Mass of Ca(OH)_2 = 31.3 g

Molar mass of Ca(OH)_2 = 74 g/mole

Volume of solution = 1050 ml

Molarity : It is defined as the moles of solute present in one liter of solution.

Formula used :

Molarity=\frac{\text{Mass of }Ca(OH)_2\times 1000}{\text{Molar mass of }Ca(OH)_2\times \text{volume of solution in ml}}

Now put all the given values in this formula, we get:

Molarity=\frac{31.3g\times 1000}{74g/mole\times 1050ml}=0.4028mole/L

Therefore, the molarity of the solution is, 0.4028 mole/L

Gennadij [26K]3 years ago
3 0
Answer is: <span>molarity of a solution is 0,401 M.
</span>m(Ca(OH)₂) = 31,3 g.
n(Ca(OH)₂) = m(Ca(OH)₂) ÷ M(Ca(OH)₂).
n(Ca(OH)₂) = 31,3 g ÷ 74 g/mol.
n(Ca(OH)₂) = 0,422 mol.
V(solution) = 1050 mL · 0,001 L/mL = 1,050 L.
c(Ca(OH)₂) = n(Ca(OH)₂) ÷ V(solution).
c(Ca(OH)₂) = 0,422 mol ÷ 1,050 L.
n(Ca(OH)₂) = 0,401 mol/L = 0,401 M.
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