34.0 g The actual solubility of KCl in water at 20°C is given in a solubility table as your result compare to your experimental molality? Is it acceptable error? KC1/100 g water, which is equal to a molality of 4.56 m. How does %error = actual value-experimental value -×100% actual value 4056-00048 U.S4 At 50°C, the solubility of KCl in water is 42.6 g in 100 g water. What is th molality of KCl in water?
34.0 g The actual solubility of KCl in water at 20°C is given in a solubility table as your result compare to your experimental molality? Is it acceptable error? KC1/100 g water, which is equal to a molality of 4.56 m. How does %error = actual value-experimental value -×100% actual value 4056-00048 U.S4 At 50°C, the solubility of KCl in water is 42.6 g in 100 g water. What is th molality of KCl in water?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I got 0.0048 mol/kg as the molarity. How do i solve this?
![### Solubility and Molality of KCl in Water: A Study Guide
#### Solubility at 20°C
The actual solubility of potassium chloride (KCl) in water at 20°C is given as 34.0 grams of KCl per 100 grams of water. This corresponds to a molality of 4.56 m.
#### Calculating Percent Error
To compare your experimental molality to this actual molality, you can calculate the percent error using the formula:
\[ \% \text{error} = \left( \frac{|\text{actual value} - \text{experimental value}|}{\text{actual value}} \right) \times 100\% \]
Below this explanation, there is a hand-written calculation that demonstrates the application of this formula:
\[ \left(\frac{4.56 - \text{experimental value}}{4.56}\right) \times 100\% \]
#### Solubility at 50°C
At 50°C, the solubility of KCl in water increases to 42.6 grams per 100 grams of water. You can determine the molality of KCl in water by using the solubility value.
#### Polarity of Liquids
From the miscibility table:
- Water is noted to be **polar** (handwritten note).
This indicates that the miscibility of liquids can help in determining their polarity:
- **Polar** substances typically mix well with other polar substances but not with nonpolar substances.
- **Nonpolar** substances mix well with other nonpolar substances but not with polar substances.
This exercise is fundamental in understanding the principles of solubility, molality, and the effect of temperature on solubility, as well as the importance of polarity in miscibility.
This guide should help you analyze similar problems and provide a foundational understanding of these chemical properties.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbedd39f0-4129-491f-813c-1ede66f9e927%2F1b6e2f6f-7eb8-4b07-a4cb-1d648d4c8694%2F9n6eahm_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Solubility and Molality of KCl in Water: A Study Guide
#### Solubility at 20°C
The actual solubility of potassium chloride (KCl) in water at 20°C is given as 34.0 grams of KCl per 100 grams of water. This corresponds to a molality of 4.56 m.
#### Calculating Percent Error
To compare your experimental molality to this actual molality, you can calculate the percent error using the formula:
\[ \% \text{error} = \left( \frac{|\text{actual value} - \text{experimental value}|}{\text{actual value}} \right) \times 100\% \]
Below this explanation, there is a hand-written calculation that demonstrates the application of this formula:
\[ \left(\frac{4.56 - \text{experimental value}}{4.56}\right) \times 100\% \]
#### Solubility at 50°C
At 50°C, the solubility of KCl in water increases to 42.6 grams per 100 grams of water. You can determine the molality of KCl in water by using the solubility value.
#### Polarity of Liquids
From the miscibility table:
- Water is noted to be **polar** (handwritten note).
This indicates that the miscibility of liquids can help in determining their polarity:
- **Polar** substances typically mix well with other polar substances but not with nonpolar substances.
- **Nonpolar** substances mix well with other nonpolar substances but not with polar substances.
This exercise is fundamental in understanding the principles of solubility, molality, and the effect of temperature on solubility, as well as the importance of polarity in miscibility.
This guide should help you analyze similar problems and provide a foundational understanding of these chemical properties.
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