Provide a sample calculation as to how you determined the Ksp at a particular temperature. Using data below: Mass of KNO3 (g): 2 h2O (mL): 5.5 precipitation temp. (celsius): 23.9 Concentration KNO3 (M): 3.6 Ksp of KNO3 (M): 12.96
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Provide a sample calculation as to how you determined the Ksp at a particular temperature. Using data below: Mass of KNO3 (g): 2
h2O (mL): 5.5
precipitation temp. (celsius): 23.9
Concentration KNO3 (M): 3.6
Ksp of KNO3 (M): 12.96
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- Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small animals, the pharmacist or veterinarian must suspend it in water, so that it can be administered orally with a medicine dropper. The label says to dispose of unused suspension after 14 days. It also points out that refrigeration is required. In the context of this chapter, what is implied in the latter two statements?Explain in terms of the Kinetic Molecular Theory the following situations: a) Why does compressing a gas raise the temperature of the system? b) Explain why the density of a gas is so much lower than the density of its liquid form? c) Explain in detail the dissolving process of KCl in water. d) Explain why the solid precipitate AGl (s) forms when solutions of KCl (aq) and AgNO3 (aq) are mixed.Consider the following reaction where Ke = 9.52x10 at 350 K. CHa(9) + CCla(0) =2CH,Cl2(9) A reaction mixture was found to contain 3.07x102 moles of CHa(g), 3.96x10 moles of CCIA(g) and 1.21x102 moles of CH,Cl2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qo equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
- 100 90 80 NANO 70 60 CaCl 50 Pb(NO)2 40 KCI NaCi 30 20 KCIO 10 Ce,(SO.) 10 20 30 40 50 60 70 80 90 100 Temperature ('C) • If 25 g KNO.is dissolved in 100 g water at 10°C and the solution s cooled to 5°C, how much of the salt crystallizes out of the solution? Solubility (g of salt in 100 g H,O) KNO3 K,Cr,O,6.) Since all the products have the same molecular weight, you can closely approximate the density of the product mixture by averaging the densities of the products. Using the average product density, determine the theoretical yield in mL when 1.5 mL of 3,3-dimethyl-2-butanol and 7 drops of H2SO4 (conc) are heated together at 70°C.A mixture combining 60 mL ethanol (C₂H6O) with 75 mL water (H₂O) is prepared at 280 K. The partial molar volumes of ethanol (E) and water (W) when mixed in these proportions (right column below) and in pure form (left column below) are ethanol water pure substance molar volume 58.2 mL/mol 18.00 mL/mol partial molar volume 55.3 mL/mol 17.7 mL/mol Determine the volume of the ethanol-water mixture. [Hint: You will need to determine the moles of each component.]
- 2. In the determination of water of crystallization for the hydrated salt BaCl2.2H20, the following data were obtained by a student. = 22.3505 g = 26.0005 Mass of crucible and lid (g) Mass of crucible, lid and sample (g) Mass of crucible, lid and sample after 1st heating (g) = 25.4931 Mass of crucible, lid and sample after 1$st heating (g) = 25.4931 a) What is the mass of the BaCl2.2H2O sample? Solution: b) What is the mass of water driven off? Solution:Water and acetonitrile, CH3CN, are miscible (can be mixed in any proportions). However, whenwater and acetonitrile are mixed, the volumes are not additive (the total volume of the resultingsolution is not equal to the sum of the pure liquid volumes). For example, when 100.0 mL ofwater and 100.0 mL of CH3CN(l), are mixed at 20 °C, the total volume of the solution is 192.0mL,not 200.0 mL.a. Provide an explanation for this phenomenon.b. Calculate the molarity, molality and mol fraction of CH3CN in a solution preparedby mixing 100.0 mL of water and 100.0 mL of CH3CN(l) at 20 °C. The total volume of themixture is 192.0 mL and the densities of water and acetonitrile are 0.998 g/mL and 0.782g/mL, respectively, at this temperature.c. When 70.0 g H2O and 190.0 g CH3CN(l) are mixed, to resulting solution has adensity of 0.860 g/mL at 20 °C. Calculate the volumes of the pure liquid samples and thesolution, and show that the pure liquid volumes are not additive.Consider the reaction at 500 degrees Celsius. N2(g) + 3H2(g) <> 2NH3(g) Kc =0.061 If analysis shows that the composition of the reactions mixture at 500 degrees Celsius is at 0.765 mol • L^-1 N2, 3.70 mol • L^-1 H2, and 4.82 mol • L^-1 NH3, what is the value of the reaction quotient Q ?
