The solubility of NaCl in water is 35.7g NaCl/100g H2O. Suppose that you have 500.0g of NaCl. What is the minimum volume of water you would need to dissolve it all? (Assume that de density of water is 1.0 g/mL.)
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To solve this problem, we need to determine the minimum volume of water required to dissolve the given amount of NaCl.
First, let's convert the mass of NaCl to moles using its molar mass. The molar mass of NaCl is approximately 58.44 g/mol.
Number of moles of NaCl = mass of NaCl / molar mass of NaCl
= 500.0 g / 58.44 g/mol
Calculate this to get the value of moles of NaCl.
Next, we can use the solubility of NaCl in water to find the volume of water required. Solubility is given as 35.7 g NaCl/100 g H2O, which means 35.7 g NaCl can dissolve in 100 g of water.
Now, we can set up a proportion to find the minimum volume of water needed:
(35.7 g NaCl) / (100 g H2O) = (500.0 g NaCl) / (x mL H2O)
Cross-multiplying, we get:
35.7 g NaCl * x mL H2O = 500.0 g NaCl * 100 g H2O
Simplifying, we have:
x mL H2O = (500.0 g NaCl * 100 g H2O) / 35.7 g NaCl
Finally, we divide the numerator by the denominator and convert g H2O to mL using the given density of water (1.0 g/mL).
x mL H2O = (500.0 * 100) / 35.7 mL H2O
Evaluate this expression to determine the minimum volume of water required to dissolve 500.0 g of NaCl.