Consider the solubilities of a particular solute at two different temperatures. Temperature (*C) Solubility (g/100 g H,O) 20.0 45.9 30.0 68.7 Suppose a saturated solution of this solute was made using 70.0 g H,O at 20.0 °C. How much more solute can be added if the emperature is increased to 30.0 °C? mass:

Consider the solubilities of a particular solute at two different temperatures. Temperature (*C) Solubility (g/100 g H,O) 20.0 45.9 30.0 68.7 Suppose a saturated solution of this solute was made using 70.0 g H,O at 20.0 °C. How much more solute can be added if the emperature is increased to 30.0 °C? mass:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Part C A sucrose solution is prepared to a final concentration of 0.140 M. Convert this value into terms of g/L, molality, and mass %. (Use the following values: molecular weight MW sucrose = 342.296 g/mol; density Psol'n = 1.02 g/mL ; and mass of water, mwat=972.1 g). Note that the mass of solute is included in the density of the solution. Express the concentrations in grams per liter, molality, and mass percent to three significant figures separated by commas. ► View Available Hint(s) | Doto r o for Part redo for eart C restor Part C keyboard shortcuts for Part C help for Part C sucrose concentrations = 47.9,1.4410-4,4.93 Submit Previous Answers X Incorrect; Try Again; 2 attempts remaining for Part for Part Gravimetric analysis Gravimetric analysis is a technique by which information is obtained based on massed values. One application of gravimetric analysis can allow the solubility of a solid to be determined. This is achieved by adding a known mass of solid to solution, then…
46.29 g of KOH is dissolved in 250. mL of water. (Please pay attention to sig figs!) What is the mass percent of KOH in this solution? (use the density of water 1.00g/mL) a. b. What is the concentration, expressed in molal (m = moles solute/kg solvent), of this initial solution? What is the concentration, expressed in molar (M = moles solute/liters solvent), of this initial solution? (assume that the addition of the KOH to the water did not change the C. volume, which is still 250.mL) d. If I add 500.mL of pure water to this 250.mL solution, what is the new concentration expressed in molar (M)? (Careful, what is the new volume after mixing?) e. If, instead, I took the 250. mL solution and evaporated the water until the solution had a volume of 150.mL, what would be the concentration of this this new solution expressed in molar (M)?
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…
The solubility of a compound is 84 g per 100.0 g solvent at 25 °C. If 84 g of the compound is dissolved in 200.0 g of solvent at 25 °C, the solution is dilute unsaturated saturated supersaturated
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A solution is made using 95.0 g of potassium nitrate in 300. mL of water at 70.0 ℃. If the solution is quickly cooled to to 20.0 ℃, how many grams of potassium nitrate precipitate out?
Consider the solubilities of a particular solute at two different temperatures. Temperature (C) Solubility (g/100 g H,O) 20.0 41.3 30.0 71.3 Suppose a saturated solution of this solute was made using 77.0 g H,O at 20.0 °C. How much more solute can be added if the temperature is increased to 30.0 °C? mass: g * TOOLS x10
An aqueous solution of isopropanol (MM = 60.10 g/mol) has a molality of 7.91 m and a density of 1.18 g/mL. What is the molarity of isopropanol in the solution?
CHAPTER 8 - SOLUTIONS Submit Qu O Previous Page 9 of 35 E Next O References Use the References to access important values if needed for this question. A certain salt is known to have a solubility in water of 28.9g/100g water at 100°C and 10.9g/100g water at 20°C. The salt is dissolved in 230 g of water at 100°C until no more solid will dissolve How much salt will crystallize out when the solution is cooled to 20°C?
What are the strongest solute-solvent interactions present in an aqueous solution of magnesium chloride?
Consider the solubilities of a particular solute at two different temperatures. Temperature (°C) Solubility (g/100 g H₂O) 20.0 44.4 30.0 78.2 Suppose a saturated solution of this solute was made using 81.0 g H₂O at 20.0 °C. How much more solute can be added if the temperature is increased to 30.0 °C? mass: g
k esc fn 14 → For gases that do not react with the solvent, Henry's law predicts a simple relationship between solubility and pressure. If the solubility of oxygen gas (O₂) in water at 20°C is 0.036 g L¹ at a pressure of 0.84 atm., what would the solubility be at the same temperature and a pressure of 2.0 atm.? 1 2 Q Type here to search A O 0.015 gl O 0.060 g L1 O 0.086 g L¹ O some other value eTextbook and Media N Hint Save for Later 12 @ 2 S F # W E X 3 alt $ JOI 4 C O R D F ts % 5 V T A 40 ° 9 6 109. ✔ & Y G H 7 $ hp B N U 4+ * 8 00 J 0x 1 M a 144 ( 9 K to Attempts: 0 of 2 used Submit Answer ► 11 ) O O L > DI P : S alt { AD 4x ? + [ = 1 * insert } 1 ctrl ← backspace ↑ pause 814 F 9/7/20 prt sc