Question
At what temperature would 4.67 grams of KCl begin to crystallize in 10mL of water?
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Answer to a math question At what temperature would 4.67 grams of KCl begin to crystallize in 10mL of water?
Birdie
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To determine the temperature at which 4.67 grams of KCl would begin to crystallize in 10mL of water, we can use the concept of solubility and saturation.
The solubility of KCl in water at different temperatures can be found in a solubility curve chart or table. Let's assume that at a certain temperature T x
Given that we have 10mL of water, the maximum amount of KCl that can dissolve in 10mL of water at temperature T \frac{x}{10} \times 4.67
At the crystallization point, KCl has reached its maximum solubility in the given amount of water. Therefore, we can set up the equation:
\frac{x}{10} \times 4.67 = 4.67
Solving for x
x = 10
Therefore, at the temperature where the solubility of KCl is 10 grams per 100mL of water, KCl will begin to crystallize in 10mL of water.
\boxed{\text{Answer: } 10 \, \text{grams per 100mL of water}}
The solubility of KCl in water at different temperatures can be found in a solubility curve chart or table. Let's assume that at a certain temperature
Given that we have 10mL of water, the maximum amount of KCl that can dissolve in 10mL of water at temperature
At the crystallization point, KCl has reached its maximum solubility in the given amount of water. Therefore, we can set up the equation:
Solving for
Therefore, at the temperature where the solubility of KCl is 10 grams per 100mL of water, KCl will begin to crystallize in 10mL of water.
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