Freezing point depression lab report answers. Lab Luis Rodríguez, Arturo melgar and Maria Muñoz 10B: FREEZING POINT DEPRESSION LAB REPORT 2022-10-27
Freezing point depression lab report answers
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Lab Luis Rodríguez, Arturo melgar and Maria Muñoz 10B: FREEZING POINT DEPRESSION LAB REPORT
Adding salt to the beaker with ice causes a temperature drop that slows the melting rate and increases the freezing one. The more solute added in H2O, lower freezing point it will have. Having weak points in an experiment is normal because in the lab the 're involved lots of factors that makes it easier to get a mistake. While more mass of sugar is added, more molality there's in the solution. Also, we were very precise at the time of getting the correct measurements. A point to take into consideration is the position of the table.
We're going to place all the test tubes when different measurements of sugar in a big beaker with some ice cubes and salt. Introduction The purpose of this lab was to determine the freezing points of the solution with and without biphenyl, and then use the difference in temperature to calculate an experimentally determined value of the molar mass of biphenyl. We get the amount of water needed and all the elements we needed to use. As I said before, the freezing point of water freezes at 0ºC, however, it's going to be lowered when salt is added. This means their vapour pressures are equal. Thus, the solid will reach equilibrium with a solution at lower temperature than with the pure solvent. We were extremely careful in this part because in other experiments, not taking perfectly and carefully the right measurements caused a complete disaster and non-sense results.
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We followed the measurements that were in the method exactly as they were. This is because the chemical potential of solvent in the mixture is lower than the pure solvent. The final result is that the ice melts slowly after the addition of salt. For, the next lab session we should learn about these small mistakes and correct them: Firstly, we had some problems, as we didn´t know when we had to take out the thermometer. That way, the results must vary from other groups experiments and might not be as accurate as we wanted them to be. We started off by preparing a water bath with a sufficient liquid level, about 650 mL in a 800 mL beaker, to cover the bottom half of the test tube when it was placed into the water bath.
Freezing Point Depression Lab Report
The liquid solution which has been formed has a lower freezing point than the pure solvent. So, what happens when we place the test tubes in a salt ice mixture beaker? This experiment is also conduct to determine the molar mass of the unknown solid using freezing point depression method. On the other hand, during the experiment we had some weak points. Another point to take into consideration is that as more solute, more molality, and as more molality,the freezing point gets lowered. While completing the table and creating the graph we've noticed that as the molality increases, the freezing point depression decreases ºC. The freezing point is the temperature at which the liquid solvent and solid solvent are at equilibrium. Some of these properties include vapor pressure lowering, boiling-point elevation, freezing point lowering, and osmotic pressure.
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The calculated value for the molar mass was 134. Then, the way of calculating the temperature with those thermometers and continuously taking out from the solution and putting again in, is not a very precise and accurate way of completing and getting the freezing point of a solution. The freezing point depression is negative, that's why the molality, which is positive is in the upper part of the graph, and all the dots go down in the graph when the molalityis bigger and the freezing point depression is lowered According to the hypothesis and the background information , the results obtained match with what we said before in the hypothesis Evaluation Discussing problems and suggesting improvements : On one hand, there were few strong points such as when calculating the temperature, we were aware that it remained constant and didn't change and when we were sure about this, we took out the thermometer form the cold or ice. We used molar mass and percent error, however both of these concepts were. This is because the freezing point of solutions is all lower than that of the pure solvent. We began heating the beaker with the water while stirring with a stir.
Freezing Point Depression Lab Report (3)
Freezing Point Depression - Chemwiki. The salt dissolves into the liquid water in the ice and lowers its freezing point. The physical properties that the solution and solute do not share are known as colligative properties and they depend solely on the solute concentration. The vapour pressure of solution is also the lower than the pure solvent. When more molality, the change in freezing point is going to be lowered.
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Freezing point depression is known as the decrease of freezing point of solvent when a non-volatile solute is added. The dissolution of a solute with very low vapor pressure, or a nonvolatile solute, raises the boiling point and lowers the freezing point. This is because adding the solute will disrupt the equilibrium, t he salt molecules dissolve in the water, but do not pack easily into the molecules in the solid ice , making thefreezing point of water being lowered when salt is added. At this moment, the gaseous and liquid states of the solvent are in dynamic equilibrium and the molecules change from the liquid to the gaseous states and from the gaseous to liquid states at equal rates. This clearly shows what we've said, and this is because the freezing point depression is directly proportional to the molality of the solute. . Science Fair Projects - The effect of salt and sugar on the freezing point of water.
The solvent boils when the vapor pressure, or tendency of solvent molecules to escape, is equivalent to the atmospheric pressure. This lowering is affected by entropy. . . . .
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