Conclusion: The general conclusion that I was able to produce about the effects of salt on the boiling point temperature of water is that with the addition of salt, the boiling point temperature of water increases. The results of the lab experiment do agree with my predictions and I can accept my initial hypothesis. However, I believe the data would be more consistent and solid had 2M and 4M of NaCl had been included in the experiment, rather than jumping from 1M to 3M to 5M.
Discussion:
For this lab experiment, the independent variable is the sodium chloride, as it was the variable being manipulated throughout the course of the experiment. The dependent variable is the boiling point temperature, as it was the variable being measured. The experimental control is the water that received 0M NaCl, which provided data that the experimental results could be compared to. A number of variables were controlled during this experiment, including the type of salt used (NaCl), the use of deionized water, and the same solution volume (100 ml). While variables were controlled, potential sources of error for this …show more content…
Since the 1M solution resulted in a temperature of 99°C and the 3M solution resulted in a temperature of 100°C, the average of the two would produce 99.5°C as the potential final boiling point temperature for a solution of 2M. Similarly, based on the graph depicting the final results of the lab experiment, I would predict that final boiling point temperature of 101.6°C would correlate with a 3.4M NaCl solution. I derived this prediction by finding the average temperature between the 3M and 5M solution, then continued to break it down farther so I would end up in a rage of the asking temperature of 101.6°C. By narrowing the window of variation, I am able to make the most plausible
Discussion:
For this lab experiment, the independent variable is the sodium chloride, as it was the variable being manipulated throughout the course of the experiment. The dependent variable is the boiling point temperature, as it was the variable being measured. The experimental control is the water that received 0M NaCl, which provided data that the experimental results could be compared to. A number of variables were controlled during this experiment, including the type of salt used (NaCl), the use of deionized water, and the same solution volume (100 ml). While variables were controlled, potential sources of error for this …show more content…
Since the 1M solution resulted in a temperature of 99°C and the 3M solution resulted in a temperature of 100°C, the average of the two would produce 99.5°C as the potential final boiling point temperature for a solution of 2M. Similarly, based on the graph depicting the final results of the lab experiment, I would predict that final boiling point temperature of 101.6°C would correlate with a 3.4M NaCl solution. I derived this prediction by finding the average temperature between the 3M and 5M solution, then continued to break it down farther so I would end up in a rage of the asking temperature of 101.6°C. By narrowing the window of variation, I am able to make the most plausible