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Exploring The Effects Of Salt On Freezing Point Depression: A Comparative Study Of Ice Water And Salt Water

This Homework Answers document investigates the impact of salt on freezing. Download now!

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Exploring the Effects of Salt on Freezing Point Depression: A ComparativeStudy of Ice Water and Salt Water1. compare your readings taken for the ice water and salt water. Howdo you explain the observedtemp change?By considering the readings taken for ice water and salt ice water we can observe a lowertemperature in the case of the salt water beaker. Indeed if salt is added to water it lowers thetemperature of change phase (from liquid to solid and from solid to liquid). In order to change phasefrom solid to liquid, heat energy is required from the surrounding environment so as to snaphydrogen bonds that hold ice together : due to the salt added the freezing point is lowered thereforemore energy is required to melt the ice. In the salt solution some ice melts and some of the salt isdissolved : heat is drawn from the ice that makes it colder : ice keeps melting to reach the freezingtemperature point of the salt solution.2. explain why salt was added to only one of the beakersSalt was added to only one of the beaker so as to compare the temperature of both beaker and toanalyze the effects of salt on the freezing point of the solution : the beaker without salt can beconsidered as a β€œreference” solutionfrom which all the measures of the salt water beaker will becompared.3. salt is a strong electrolyte that produces two ions, Na+ and cl-when it dissociates in water. explainwhy this is important to consider when calculating the colligative property of freezing pointdepressionA freezing-point depression occurs when a solute (salt) is added to a solvent (water) and produces adecrease in the freezing point. The colligative property of freezing point depressionis determined bythe ratio :π‘π‘’π‘šπ‘π‘’π‘Ÿπ‘œπ‘“π‘ π‘œπ‘™π‘’π‘‘π‘’π‘šπ‘œπ‘™π‘’π‘π‘’π‘™π‘’π‘ π‘π‘’π‘šπ‘π‘’π‘Ÿπ‘œπ‘“π‘ π‘œπ‘™π‘£π‘’π‘›π‘‘π‘šπ‘œπ‘™π‘’π‘π‘’π‘™π‘’π‘ In the case of salt water the number of dissolved particles isgreater than ice waterbecause of the presence of salt dissolved in the water. Two ions are producedwhen salt dissociates in water (Na+and Cl-) : the presence of a solute lowers the freezing point of apure solvent solution (ice water considered as a pure solvent), the decrease in temperature isproportional to the number of dissolved particles in the solution. A useful formula to estimate thechange in freezing point is :βˆ†π‘‡=π‘–πΎπ‘šwhereβˆ†π‘‡is the change in freezing point temperature, i is thenumber of ions present per formula unit (in this case i = 2) and K is the freezing point depressiondepression constant for the solvent (K = 1.86Β°C.kg/mol for water)4. predict wheather it would be better to use coarse rock salt or fine table salt when makinghomemade ice cream.Explain?In order to make ice cream it’s betterto use the coarse salt. But in order to produce rapid cold tablesalt would be better. Indeed if you use table salt the salinity of the melting water increases to

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Chemistry

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