liquid X has a normal boiling point of 144.20 °C and a boiling point elevation constant K,=0.76 °C·kg•mol g some ammonium chloride (NH,Cl) in 150. g of X. This solution boils at 145.3 °C. Calculate the mass of NH,C your answer is rounded to the correct number of significiant digits.

A soft drink contains an unknown mass of citric acid, C3H5O(COOH)3. It requires 6.42 mL of 9.580 × 10−2-M NaOH to neutralize the citric acid in 10.0 mL of the soft drink. C3H5O(COOH)3(aq) + 3 NaOH(aq) → Na3C3H5O(COO)3(aq) + 3 H2O(ℓ) Determine which step in these calculations for the mass of citric acid in 1 mL soft drink is incorrect? Why? n (NaOH) = (6.42 mL)(1L/1000 mL)(9.580 × 10−2 mol/L) n (citric acid) = (6.15 × 10−4 mol NaOH) × (3 mol citric acid/1 mol NaOH) m (citric acid in sample) = (1.85 × 10−3 mol citric acid) × (192.12 g/mol citric acid) m (citric acid in 1 mL soft drink) = (0.354 g citric acid)/(10 mL soft drink) Determine the correct result.

You want to prepare a 1.0 mol/kg solution of ethyleneglycol, C2H4(OH)2, in water. Calculate the mass of ethylene glycol you would need to mix with 950. g water.

Potassium sulfate has a solubility of 15 g/ 100 g water at 40C. A solution is prepared by adding 39.0 g of potassium sulfate to 225 g of water, carefully heating the solution, and cooling it to 40C. A homogeneous solution is obtained. Is this solution saturated, unsaturated, or supersaturated? The beaker is shaken, and precipitation occurs. How many grams of potassium sulfate would you expect to crystallize out?

Without consulting your textbook, list and explain the main postulates of the kinetic molecular theory for gases. How do these postulates help us account for the following bulk properties of a gas: the pressure of the gas and why the pressure of the gas increases with increased temperature; the fact that a gas tills its entire container; and the fact that the volume of a given sample of gas increases as its temperature is increased.

What is the difference between (a) mass and density? (b) an extensive and an intensive property? (c) a solvent and a solution?

1 A certain liquid X has a normal boiling point of 144.80 °C and a boiling point elevation constant K,=2.39 °C•kg•mol A solution is prepared by dissolving some glycine (C,H,NO,) in 650. g of X. This solution boils at 148.5 °C. Calculate the mass of C,H,NO, that was dissolved. Round your answer to 2 significant digits. olo Ar

A certain substance X has a normal boiling point of 131.9°C and a molal boiling point elevation constant =Kb·1.78°C·kgmol−1. A solution is prepared by dissolving some urea ((NH2)2  CO) in 600.g of X. This solution boils at 133.7°C. Calculate the mass of urea that was dissolved. Round your answer to 2 significant digits.

What is the freezing point of a ethanol solution if that same solution boils at 79.5 ℃? The normal boiling point and freezing point of pure ethanol (C2H5OH) are 78.29 ℃ and -114.2 ℃, respectively. For ethanol, Kb = 1.23 ℃/m and Kf = 1.99 ℃/m.Please enter your response in standard notation to one decimal place.

1 A certain substance X has a normal freezing point of 7.9 °C and a molal freezing point depression constant K,=5.08 °C·kg•mol . A solution is prepared by dissolving some urea ((NH,) CO) in 600. g of X. This solution freezes at 6.5 °C. Calculate the mass of urea that was dissolved. 2 Round your answer to 2 significant digits. g