Solubility of an Unknown Solute 80 60 Solubility (g solute/ 100g H,0) 40 20 10 20 30 40 50 60 70 80 90 100 Temperature (°C) According to the solubility curve above, dissolving 20 grams of solute in 100g of water at 50°C would make a solution that was [ Select ] Dissolving 50g of solute in 100g of water at 60°C would [ Select] [ Select] saturated unsaturated supersaturated

Solubility of an Unknown Solute 80 60 Solubility (g solute/ 100g H,0) 40 20 10 20 30 40 50 60 70 80 90 100 Temperature (°C) According to the solubility curve above, dissolving 20 grams of solute in 100g of water at 50°C would make a solution that was [ Select ] Dissolving 50g of solute in 100g of water at 60°C would [ Select] [ Select] saturated unsaturated supersaturated

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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Extra information: freezing point depression constant for the solvent (20.0 degrees Celcius kg/mol for cyclohexane)
What is a colligative property
Solute S has a distribution constant of 5.1 between water (phase 1) and hexane (phase 2). A 71.0 mL solution of S in water is extracted three times with 12.0 mL of hexane. Calculate the fraction of S remaining in the aqueous phase. fraction remaining: 0.0575 Incorrect
Solubility (g of salt in 100 g H,O) KNOS 100 06 NANO 80 70 60 CaCl 50 Pb(NO)2 40 NaCl KCT 30 20 10 KCIO, Ce,(SO,), 10 20 30 40 50 60 70 80 90 100 Temperature (C) If 25.0 grams of K2Cr207 have been dissolved at 80oC, how many more grams are needed to create a saturated solution? Format BIU
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The experimental data in the table was collected during a freezing point depression study where BHT (butylated hydroxytoluene) was the solvent. Mass of BHT Mass of unknown Freezing point of pure BHT Freezing point of BHT and unknown solution Kf for BHT 7.709 g7.709 g 1.252 g1.252 g 74.17 ∘C74.17 ∘C 70.91 ∘C70.91 ∘C 6.83 ∘C/?6.83 ∘C/m Use this data to calculate the molar mass of the unknown solute. molar mass =
olve Mass % of glucose ercentage of solu mass of solute (glucose) and the mass of solvent (water). age by using Equation 13.5. The mass of the soluti Solve ppm = mass glucose mass soln Comment The mass percentage of water in this solution is (100-11.9) % = 88.1%. 1 x 10g, 5.4 µg = 5.4 x 10g. b) Analyze In this case we are given the number of micrograms of solute. Because 1 µg is Plan We calculate the parts per million using Equation 13.6. 5.4 X 10-6 2.5 g mass of solute mass of soln Q X 100 = X 106 = 13.5 g 13.5 g + 100 g g X 100 = 11.9% X 106 = 2.2 ppm Practice Exercise 1 Calculate the mass percentage of NaCl in a solution containing 1.50 g of NaCl in 50.0 g of water. (a) 0.0291%, (b) 0.0300%, (c) 0.0513%, (d) 2.91%, (e) 3.00%. Practice Exercise 2 A commercial bleaching solution contains 3.62% by mass of sodium hypochlorite, NaOCI. What is the mass of NaOCl in a bottle containing 2.50 kg of bleaching solution? Mole Fraction, Molarity, and Molality Concentration expressions are often…
Boiling Point Elevation/Freezing Point DepressionT = m KWhere: T = T(solution) - T(pure solvent) * m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Solvent Formula Kb (°C / m) Kf (°C / m) Water H2O 0.512 -1.86 Ethanol CH3CH2OH 1.22 -1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 -5.12 Diethyl ether CH3CH2OCH2CH3 2.02 note that ΔT as defined above will be a negative number for freezing point depression. Therefore, Kf must also be given as a negative number.
Assuming 100% dissociation, calculate the freezing point (T) and boiling point (T) of 1.81 m CaCl₂(aq). Colligative constants can be found in the chempendix. Tf= Tь = F 2 # 3 с $ 4 G Search or type URL % 5 MacBook Pro ^ 6 & 7 * 8 ( ( 9 ) I O 4) °C °C
A chemist attempts to prepare some very pure crystals of borax by dissolving 100g of Na2B4O7 in 200 grams of boiling water. He then cools the solution slowly until some borax crystallizes out. Calculate the grams of borax recovered in the crystals per 100 grams of initial solution (NazB4O7 plus water), if the residual solution at 55°C after the crystals are removed contains 12.4% NazB4O7.What is the percent yield or percent recovery of Na2B4O7.
Extra information: freezing point depression constant for the solvent (20 degrees celsius kg/mol for cyclohexane) I am trying to figure out this problem and need a step by step guide in order to find the answer using the data given. Thank you!
When 3.92 grams of an unknown non-volatile, non-electrolytic solute is added to 17.2 g of a particular solvent, the boiling point of the solvent increases by 2.80". Given that the molal boiling point constant is kb = 1.90 "/m_ What is the molar mass of the unknown solute (g/mol)? Equation: ikŕm 4T ΔΤ =