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# us solution containing sodium chloride that has a density of 1-01 g-mL.docx

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# us solution containing sodium chloride that has a density of 1-01 g-mL.docx

us solution containing sodium chloride that has a density of 1.01 g/mL. Assume the behaves ideally. The freezing point of this solution at 1.0 atm is -1.28 Â°C. solution (a) Calculate the percent composition of this solution (by mass). (Kr for water 1.86 Ckg/mol) (3pts) (b) Why is the observed freezing-point depression for electrolyte solutions sometimes less than the calculated value? Is the difference greater for concentrated or dilute solutions? (3pts)
Solution
change in freezing point=M*i*kf.
This is because,the additives it contain like NaCl in this question,they break into respective ions increasing the i.
This increases ions reduce the freezing point
.

us solution containing sodium chloride that has a density of 1.01 g/mL. Assume the behaves ideally. The freezing point of this solution at 1.0 atm is -1.28 Â°C. solution (a) Calculate the percent composition of this solution (by mass). (Kr for water 1.86 Ckg/mol) (3pts) (b) Why is the observed freezing-point depression for electrolyte solutions sometimes less than the calculated value? Is the difference greater for concentrated or dilute solutions? (3pts)
Solution
change in freezing point=M*i*kf.
This is because,the additives it contain like NaCl in this question,they break into respective ions increasing the i.
This increases ions reduce the freezing point
.

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### us solution containing sodium chloride that has a density of 1-01 g-mL.docx

1. 1. us solution containing sodium chloride that has a density of 1.01 g/mL. Assume the behaves ideally. The freezing point of this solution at 1.0 atm is -1.28 Â°C. solution (a) Calculate the percent composition of this solution (by mass). (Kr for water 1.86 Ckg/mol) (3pts) (b) Why is the observed freezing-point depression for electrolyte solutions sometimes less than the calculated value? Is the difference greater for concentrated or dilute solutions? (3pts) Solution change in freezing point=M*i*kf. This is because,the additives it contain like NaCl in this question,they break into respective ions increasing the i. This increases ions reduce the freezing point