Desert countries like Saudi Arabia have built reverse osmosis plants to produce freshwater Irom seawater. Assume that seawa- ter has the composition 0.470M NaCl and 0.068 M MgCl, and that both compounds are completely dissociated. (a) What is the osmotic pressure of seawater at 25 "C? sure of 100.0 atm at 25,0 C, what is the maximum volume of freshwater thal can be oblalned from 1.00 Lof seawater

Desert countries like Saudi Arabia have built reverse osmosis plants to produce freshwater Irom seawater. Assume that seawa- ter has the composition 0.470M NaCl and 0.068 M MgCl, and that both compounds are completely dissociated. (a) What is the osmotic pressure of seawater at 25 "C? sure of 100.0 atm at 25,0 C, what is the maximum volume of freshwater thal can be oblalned from 1.00 Lof seawater

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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2. A student was asked to identify a sample of unknown hydrate. Student was provided with the following experimental data. 3.51 g sample of the hydrate when heated loses water completely and the mass of the residue was found to be 2.22 g. Student was provided with two reference compounds from which student needs to identify the unknown: Cu(NO3)2. 3H2O and Cu(NO3)2. 6H20. Answer the followings. a. Calculate percent water of hydration in the sample. (show your calculations)
Aspirin can be prepared from salicylic acid (C7H6O3 ), which has a molar mass of 138.12 g/mol, and acetic anhydride (C4 H6 O3), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C;H,O3 + C4H6O3 → C9HgO4 + C2H3O2 What is the theoretical yield, in grams, of aspirin (C9H3O4), which has a molar mass of 180.15 g/mol, possible when reacting 3.06 g of salicylic acid with 3.71 mL of acetic anhydride? Type answer:
6. Consider the following chemical reaction: 2 Cr(OH)3(aq) >Cr₂O3(s) + 3H₂0(1) 12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced. O 18.00 moles O 1.500 moles O 4.00 moles O 12.00 moles
What mass of Cu(IO3)2 can be formed from 0.650 g of CuSO4 · 5H2O? What mass of KIO3 is needed to convert the copper in 0.2750 g of CUSO4 - 5H2O to Cu(IO3)2?
Balance the following equations. (Use the lowest possible integer coefficients.) (a) UO₂ (s) + HF() → UF4 (s) + H₂O(l) UO₂ (s) + 4 HF () →> (b) B2O3(s) + HF() → BF3 (s) + H₂O(l) B₂O3(s) + HF (1) - (c) BF3 (s) + H₂O(l) → HF() + H3 BO3(s) BF3 (s) + H₂O(l) →→→→ 2 UF4 (s) + BF3 (s) + HF () + 2 H₂O(l) H₂O(l) H3 BO3(s)
ml of 0.3 normali (hydrochloric acid) was taken to prepare a solution with a concentration of 0.09 normali of hydrochloric acid in 180 ml. Note that the atomic weights of chlorine = 35.5 and = 9 Hydrogen = 1 85 O 45 O 54 60
72
2. A mixture of Na2SO4 and its hydrate Na2SO4-10H₂O has a mass of 1.5099 g. After heating to drive off all the water, the mass is only 1.1410 g. What is the weight percentage of Na2SO4.10H₂O in the original mixture? Report your answer to 4 significant figures. Molar masses: Na2SO4 142.04 g/mol; Na2SO4.10H₂O 322.19 g/mol.
A student performed a similar experiment to the one you performed: They took a crucible and lid, cleaned them, heated them over a flame, and after cooling found their combined mass to be 22.538 g. The student then added a sample of zinc(II) sulfate hydrate (ZnSO4·“n”H2O) to the crucible so the combined mass of the sample, crucible, and lid was 25.896 g. They heated this sample for 10 minutes with the lid ajar, let it cool, and measured the mass of the crucible, sample, and lid to be 25.054 g. a. Based on this experiment, what is the formula for they hydrated zinc(II) sulfate compound? b. The student later looked on the reagent bottle for zinc(II) sulfate hydrate and found the actual formula was ZnSO4·7H2O. If everything had been done correctly, what value should the student have expected for the final mass of their sample, crucible, and lid after heating?
Aa.103.
1. Find the necessary amount of Ag,CO; in grams in order to obtain 79.1 g of silver. A92CO3 · Ag(s) + CO2 + 02 (unbalanced) C: 12 g/mol, O: 16 g/mol, Ag: 107.9 g/mol