Interpretation:
Addition of
Concept introduction
Freezing point is the temperature at which liquid turns into solid.
The Freezing point depression
Where,
From given mass of substance moles could be calculated by using the following formula,
Molality: It is a measure of the concentration of a solute in a solution in terms of amount of substance in the amount of mass of solvent.
Where, m is molality; mole is moles of solute and kg is mass of solvent.
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Chemistry: The Molecular Science
- The dispersed phase of a certain colloidal dispersion consists of spheres of diameter 1.0 102 nm. (a) What are the volume (V=43r2) and surface area (A = r2) of each sphere? (b) How many spheres are required to give a total volume of 1.0 cm3? What is the total surface area of these spheres in square meters?arrow_forwardA certain liquid X has a normal freezing point of −3.40 °C and a freezing point depression constant K .=5.74 °C·kg⋅mol¯¹. A solution is prepared by dissolving some zinc chloride (ZnCl₂) in 700. g of X. This solution freezes at -5.0 °C. Calculate the mass of ZnCl₂ that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. g ☐ x10 Xarrow_forward1. The solubility of L-glutamic acid (an amino acid) in water has been determined to be as follows (all values are grams of L-glutamic acid/100 mL of water): Temp. 0 °C 0.34 50 °C 2.19 75 °C 5.53 100 °C 14.00 (a) What is the minimum volume of water (rounded to the nearest mL) that you would use to recrystallize 50.0 g of L-glutamic acid? Please show all work. (c) Where is the missing L-glutamic acid? (b) How much purified L-glutamic acid would you expect to recover at 0°C assuming no losses due to technique? Please show all work.arrow_forward
- Gg.176.arrow_forwardA certain liquid X has a normal freezing point of 6.90°C and a freezing point depression constant =Kf 2.27·°C·kgmol−1. Calculate the freezing point of a solution made of 92.g of glycine (C2H5NO2) dissolved in 700. g of X. Round your answer to 2 significant digits.arrow_forwardA certain liquid X has a normal freezing point of 0.90°C and a freezing point depression constant Kf=6.96·°C·kgmol−1.A solution is prepared by dissolving some barium hydroxide (Ba(OH)2) in 900.g of X. This solution freezes at−3.7°C. Calculate the mass of Ba(OH)2 that was dissolved. Round your answer to 2 significant digits.arrow_forward
- A certain liquid X has a normal freezing point of 3.00°C and a freezing point depression constant Kf=6.96·°C·kgmol−1. Calculate the freezing point of a solution made of 80.7 g of benzamide (C7H7NO) dissolved in 900.g of X. Round your answer to 3 significant digits.arrow_forwardA certain liquid X has a normal freezing point of 3.30°C and a freezing point depression constant =Kf 5.91·°C·kgmol−1. Calculate the freezing point of a solution made of 9.69 g of benzamide (C7H7NO) dissolved in 400.g of X. Round you answer to 3 significant digits.arrow_forwardWhen 571. mg of a certain molecular compound X are dissolved in 60.0 g of benzene (CH), the freezing point of the solution is measured to be 4.8 °C. Calculate the molar mass of X. If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. 0 X x10 Sarrow_forward
- The molal freezing point depression constant K,=2.51 °C·kg•mol ((NH,),CO) CO are dissolved in 100. g of 2 for a certain substance X. When 6.12 g of urea X, the solution freezes at 0.6 °C. Calculate the freezing point of pure X. Be sure your answer has the correct number of significant digits. °Carrow_forward3. You are asked to calculate the Kf for t-butyl alcohol (MW = 74.122 g/mol). You gather the following information in your experiment. You weigh out 2.124 g t-butyl alcohol and you determine the freezing point of the solvent t-butyl alcohol is 21.6 °C (freezing point pure t-butyl alcohol). You then add water to the test tube with the t-butyl alcohol and measure the freezing point to be 15.3 °C. What key piece of information are you missing to calculate the Kf?arrow_forwardWhen 238. mg of a certain molecular compound X are dissolved in 90.0 g of benzonitrile C6H5CN , the freezing point of the solution is measured to be −13.0 °C . Calculate the molar mass of X. If you need any additional information on benzonitrile, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 1 significant digit.arrow_forward
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