5. A solution of sodium nitrate at a temperature of 60*C contains 45% of sodium nitrate by weight (a) How saturated is this salt solution (express in percentage)? (b) Calculate the weight of NaNO3 that will be crystallized if 100 g of this solution is cooled to o*c (c) Calculate the percentage yield of this crystallization process (d) What is the molarity of the original solution. The density of the solution is 1.3371 at 60*C (e) What is the molality of the original solution? (f) What is the concentration of sodium nitrate in the original solution in grams per 100 g of water? Temperature "C 10 20 30 40 50 60 70 80 90 100 Solubility g/100g water 80.8 87.6 94.9 73 102 112 122 135 148 164 180

5. A solution of sodium nitrate at a temperature of 60C contains 45% of sodium nitrate by weight (a) How saturated is this salt solution (express in percentage)? (b) Calculate the weight of NaNO3 that will be crystallized if 100 g of this solution is cooled to oc (c) Calculate the percentage yield of this crystallization process (d) What is the molarity of the original solution. The density of the solution is 1.3371 at 60*C (e) What is the molality of the original solution? (f) What is the concentration of sodium nitrate in the original solution in grams per 100 g of water? Temperature "C 10 20 30 40 50 60 70 80 90 100 Solubility g/100g water 80.8 87.6 94.9 73 102 112 122 135 148 164 180

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...

See similar textbooks

Similar questions

a student separated 7ml of ethyl acetate and butyl acteta via distillation. At the end of the distillation the student obtained 2.7 grams of ethyl acetate. Given that the density of ethly acetate is 0.902g/ml, what is the percent recovery of ethyl acetate
86.5 g of MgCl2 (m.m. = 95.211 g mol−1), asoluble salt, is dissolved in pure water. Howmany moles (to one decimal place) of soluteparticles does this result in? The answer is 2.7
Solubility Curves of Selected Compounds 150 140 130 120 110 100 NaNO, 90 80 70 60 NH C KCI Nac 50 40 30 20 KCIÓ 10 Cez(SO4)3 10 20 30 40 50 60 70 90 100 Temperature (C) The compound whose solubility increases the fastest with an increase in temperature is: OKI O NANO3 O KNO3 O NH, O NH&CI O KCI O NaCI O KCIO, O Ce:(SOala DELL Grams of solute per 100 g H,O NH FONX
concentration of the solution. (c) the mass in grams of NiCl2 contained in each liter O. A 12.5% (w/w) NiCl2 (129.6l g/mol) solution has a density of 1.149 g/mL. Caleulate(a) the molar concentration of NiCl, in this solution. (b) the molar CI oncentration of the solution. (c) the mass in grams of NiCl, contained in each liter of this solution. 10- Describe the preparation of (a) 2.50 L of 21.0% (w/v) aqueous glycerol (C.HO: (92.1 g/mol). (b) 2.50 kg of 21.0% (w/w) aqueous glycerol. (c) 2.50 L of 21.0% (v/v) aqueous glycerol. U- Describe the preparation of 900 mL of 3.00 M HNO, from the commercial reagent that is 70.5% HNO, (w/w) and has a specific gravity of 1.42. 12- A solution containing 10.0 mmol CaCl, is diluted to 1 L. Calculate the number of grams of CaCl2. 2H2O per milliliter of the final solution. 13- Calculate the grams of each substance required to prepare the following solutions: (a) 250mL of 0.100 M KOH, (b) 1.00 L of 0.0275 M K;Cr,O, (c) 500ml of 0.0500 M CUSO4. 38 0%…
A solid mixture consists of 25.5 g of KNO3 (potassium nitrate) and 4.5 g of K₂SO4 (potassium sulfate). The mixture is added to 130. g of water. Use this solubility curve (Figure 1) to answer the Part C If the solution described in the introduction is cooled to 0 °C what mass of K2SO4 will crystallize?
What volume of 30.0% hydrogen peroxide solution is required to provide the mass 3.0618 in a 25.00mL solution of 3.6M H2O2 (density30.00% H2O2 = 1.11 g/mL)?
The solubility of N₂ in blood is a serious problem for divers breathing compressed air (78% N₂ by volume) at depths greater than 50 ft (see the margin note, p. 522). (a) What is the molarity of N₂ in blood at 1.00 atm? (b) What is the molarity of N₂ in blood at a depth of 50. ft? (c) Find the volume (in mL) of N₂ , measured at 25°C and 1.00 atm, released per liter of blood when a diver at a depth of 50. ft rises to the surface (kH for N₂ in water at 25°C is 7.0X10⁻⁴ mol/Latm and at 37°C is 6.2X10⁻⁴ mol/L atm; assume dof water is 1.00 g/mL).
please put calculations in the given frame
A solution was prepared by dissolving 0.687 g of sulfur, S, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and boiling point of the solution. (K, = 3.08°C/m and Kf = 3.59°C/m, T, = 118.5°C and T† = 16.60°C) Freezing point: °C Boiling point: °C
Calculate the mass (in grams) of magnesium chloride (〖????〗_2) that would be needed to prepare 150 mL 0f a 20 % by mass aqueous solution of the salt. The density of a solution is 1.1g/mL.
How is the term solubilty: Represent and quantify chemical reactions at the atomic level?
10. An element has two isotopes of relative atomic masses 41.0 u and 44.0 u. The relative abundance of the isotopes are 90.0% and 10.0% respectively. The average atomic mass of the element is: (A) 41.0u (B) 41.3u (C) 42.5u (D) 43.7u 2 11. Which of the following phrases best describes the term solubility? (A) the ability of a solvent to dissolve in a solute (B) the ability of a solute to dissolve in a solvent (C) the maximum amount of solute that will dissolve in solvent at a given temperature (D) the maximum amount of solvent that will dissolve in a solute at a given temperature 4