I would appreciate to check my work and understanding. Thank you.
I would appreciate to check my work and understanding. Thank you. = 5.11 °C kg-mol ....
ADVANCED MATERIAL Using the Kland Kb equations with electrolytes A certain liquid X has a normal freezing point of 2.60 °C and a freezing point depression constant k, = 5.29 °C kg-mol . A solution is prepared by dissolving some ammonium chloride (NHCl) in 800. g of X. This solution freezes at 0.9 °C. Calculate the mass of NHCl that was dissolved. Round your answer to 2 significant digits. Explanation Check
= 4.47 °C-kg-mol. Calculate the freezing point of a A certain liquid X has a normal freezing point of 4.20 °C and a freezing point depression constant K solution made of 22.g of potassium bromide (KBr) dissolved in 550. g of X. Round you answer to 2 significant digits. 3°C X 5 ?
A certain liquid X has a normal freezing point of 7.80 °C and a freezing point depression constant K,=3.03 °C kg mol. Calculate the freezing point of a solution made of 15.6g of urea (CH N,0) dissolved in 200. g of X. Be sure your answer is rounded to the correct number of significant digits. O°C
When 116. g of alanine (C,H,NO,) are dissolved in 900. g of a certain mystery liquid X, the freezing point of the solution is 6.8 °C lower than the freezing point of pure X. On the other hand, when 116. g of ammonium chloride (NH,CI) are dissolved in the same mass of X, the freezing point of the solution is 17.9 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for ammonium chloride in X....
When 70.4 g of benzamide (C,H,NO) are dissolved in 850. g of a certain mystery liquid X, the freezing point of the solution is 2.7 C lower than the freezing point of pure X. On the other hand, when 70.4 g of ammonium chloride (NH CI) are dissolved in the same mass of X, the freezing point of the solution is 9.9 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for ammonium chloride in...
A certain substance X melts at a temperature of -9.9 °C. But if a 250. g sample of X is prepared with 9.10 g of urea ((NH) CO dissolved in it, the sam is found to have a melting point of -12.0 °C instead. Calculate the molal freezing point depression constant K, of X. Be sure your answer has the correct number of significant digits. [°C mol'.kg x 5 ? Save For Later Sult Check
C kg mol Calculate the boiling point of a solution A certain liquid X has a normal boiling point of 96.80 C and a boiling point elevation constant k-1.23 made of 221.g of barium hydroxide (Ba(OH)2) dissolved in 800. g of X. Round your answer to 5 significant digits. Dec X 5 ?
A certain substance X has a normal freezing point of 6.8 C and a molal freezing point depression constant Kf=7.51C kg x mol-1 . A solution is prepared by dissolving some urea ((NH2)2CO) in 600 of X. This solution freezes at 5.0 C . Calculate the mass of urea that was dissolved. Be sure your answer has the correct number of significant digits.
A certain liquid X has a normal freezing point of 5.50 °C and a freezing point depression constant K =4.39 °C-kgmol. A solution is prepared by dissolving some urea (CH4N20) in 800. g of X. This solution freezes at 3.6 °C. Calculate the mass of CH4N20 that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. x 6 ?
The normal freezing point of a certain liquid X is 6.60 °C, but when 27. g of potassium bromide (KBr) are dissolved in 300. g of X the solution freezes at 4.9 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Be sure your answer is rounded to the correct number of significiant digits. Ķ, = 0 °C kg x s ?