A 50.0-mL solution is initially 1.55% MgCl2 by mass and has a density of 1.05 g>mL. What is the freezing point of the solution after you add an additional 1.35 g MgCl2? (Use i = 2.5 for MgCl2.)

Remember that the boiling point elevation constant for water is Kb = 0.512 C/kg, and the freezing point depression constant for water is Kf = 1.86 C/kg Use the table provided to answer the question. 1.00 g of Lead (II) Sulfate is mixed into 5.75 L of water. a) How many moles of the Lead (III) Sulfate will actually dissolve into the water? b) How many grams of Lead (III) Sulfate will be left un-dissolved? c) At what temperature will the solution now boil and freeze?

Use the solubility curve below to answer the following questions: 150 140 130 120 110 100 NANO3 90 80 70 60 NH&Cl KCI NaCi 50 40 30 20 KCIO3 10 Ce2(SOals O 10 20 30 40 50 60 70 80 90 100 Temperature (c) Q1) As the temperature increases, the solubility of the NH3 in water Q2) The solute, NH3, is MOST likely a (increases/decreases/stays the same). (solid, liquid, or gas). Q3) How many grams of NH4CI are dissolved in 500 g of water at 90 °C? Q4) If you had 50 grams of NH4CI in 100 g of water at 40 °C, would the solution be saturated, unsaturated, or supersaturated? Q5) You heat a solution of KCIO3 to 80°C and saturate the solution. You then allow the solution to cool down to 50°C. How many grams of solute would precipitate out of the solution? NH3 per 100 g H,0 Grams of solute ONO CON

The names and chemical formulae of some chemical compounds are written in the first twa columns of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. Then, write down in the third column of the table the chemical formula of the major chemical species that will be present in this solution. For example, you know water itself will be present, so you can begin each list with the chemical formula for water (H,O).

When 0.52 g of an unknown nonelectrolyte are dissolved in 35.0 g cyclohexane, the freezing point of the solution is 5.1ºC.  Pure cyclohexane freezes at 6.6ºC and has a Kf of 20.0ºC/m. What is the molar mass of the unknown in g/mol? Enter your answer with no decimal places (round to the nearest whole number). Do not include units. Do not worry about significant figures. Example: 2

A solution is prepared by adding 62 g Pb(NO3)2 to 100 g water at 20 °C. Is the solution saturated, unsaturated, or supersaturated? The temperature is raised to 80 °C. There is a temperature at which the solution is no longer classified by the term you answered above. What is that temperature? Just list the number, don't include the °C unit. At 80 °C, is the solution classified as saturated, unsaturated, or super saturated?

At 20 °C and a partial pressure of 760 mmHg, the solubility of CO₂ in water is 0.169 g/100 mL. Part A What is the solubility of CO₂ at 2.0×104 mmHg? Express your answer using two significant figures. xa || ΑΣΦ Xb C= 3.38.10³ √x xx x x IXI Submit Previous Answers Request Answer * Incorrect; Try Again; 5 attempts remaining X.10 g/100 mL

Camphor is a white solid that melts at 179.50°C. It has been used to determine the molecular weights of organic compounds because of its unusually large freezing-point-depression constant (39.7°C/m), which allows ordinary thermometers to be used. The organic compound is dissolved in camphor, and then the melting point of the solution is determined. If 1.08 g of an unknown compound is dissolved in 73.6 g camphor, the freezing point is found to be 177.09°C. What is the molecular weight of the unknown compound?

Molarity!A solution is prepared by dissolving 20.0 g of Chloroform (CHCl3) in 60.0 gram of benzene (C6H6). The density of the solution was found to be .856 g/mL.The molar mass of CHCL3 is 119.4 g/molThe molar mass of C6H6 is 78.11 g/molWhat is the Molarity of the solution?

Colligative properties are those that depend on the number of solute particles. Because electrolytes dissociate into ions, the concentration of particles in the solution is greater than the formula-unit concentration of the solution. For example, if 1 mol of NazSO4 totally dissociates, 3 mol of ions are produced (2 mol of Nat ions and 1 mol of SO, ions). Thus, a colligative property such as osmotic pressure will be three times greater for a 1 M NazSO, solution than for a 1 M nonelectrolyte solution. Part A Assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that freezes at - 14.5 °C? The freezing point for pure water is 0.0 °C and Kf is equal to 1.86 °C/m. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) However, complete dissociation of electrolytes does not always occur. The extent the van't Hoff factor, i: dissociation is expressed by HA moles of…