Homework Answers
Crystallization is a technique which generally used to purify solid compounds. In this process solids are being dissolved in a liquid at higher temperature. At higher temperature more solids can be dissolved in liquid as the kinetic energy in the solution increases and the solid molecules move faster in the solution which increase their chances to meet more solvent molecules in the way. As a result solubility also increases. In this process when the the hot solution becomes saturated, they are being cooled and the crystals are started to form as kinetic energy decreases. The solubility of most of the ionic liquids increases in solution including NaCl.
a. Heating the solution to evaporate the water is not crystallization, it is just a process to evaporate the solvent to dryness. In this process the dry NaCl remains as a solid. Therefore it is not a right option.
b. Dissolving more NaCl to cause supersaturation is also not crystallization. The solutions remains in supersaturated state if the temperature is constant. No crystal will form. Therefore this is also not right option.
c. Cooling a saturated solution will cause crystallization as the kinetic energy of the solution decreases and solid molecules have lesser amount of water to interact. Consequently the crystals started to grow in the solution and come down as precipitate. This is a right option.
d. Diluting a saturated solution just increase the availability of solvent molecules for NaCl and the solution becomes unsaturated. Therefore no crystallization will occur. The crystallization happens when saturated solutions are being cooled. Therefore this is not a right option.
e. As a and b options are already ruled out so it is not a correct option.
After analyzing all the options the "option c" comes out as right option.
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14. (three marks) Which of the following would cause crystallization of NaCl from a solution? a...
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e) volume. d) number of moles of solute. 14) Which of the following substances would be...
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answer 1-4 Which of the following (a-d) is TRUE regarding solid NaCl dissolving in water The...
answer 1-4
Which of the following (a-d) is TRUE regarding solid NaCl dissolving in water The attraction of the water to the ions in NaCl is through dipole-dipole IFs. Water is considered the solute and NaCl the solvent. The partially positive oxygen in water is attracted to the chloride ion. d. The process of separating the sodium ions from the chloride ions is endothermic. All of these statements are true. polar For the following solution, describe the deviation with respect...
g. Which of the following situations would most likely cause gases to deviate from a) Low...
g. Which of the following situations would most likely cause gases to deviate from a) Low pressure and high temperature b) High pressure and low temperature c) High pressure and high temperature d) Gases never deviate from ideal behavior e) Low pressure and low temperature 10. A gas mibxture has three components Na. F and He, their partial pressures are 0.45 atm, 0.160 atm and 0.20 atm respectively. What is the pressure of the gas mixture? a) 1.05 atm b)...
1.What would be the predominate form(s) of the following elements in a pH-7 aqueous solution each...
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10 Equal masses of the following non-volatile solutes are dissolved in 1000g of H20(0). Which solution...
10 Equal masses of the following non-volatile solutes are dissolved in 1000g of H20(0). Which solution will have the LOWEST freezing point. A. NaCl B. KCI C. LiCl D. CsCl E. RbCl Suppose that the reaction A → products proceeds in one step and is exothermic. It has an activation barrier of 75 k/mol. How would the energy diagram change if a catalyst is added to the reaction? Select all the statements that could be true. 11 Addition of the...
Saturated, Unsaturated & Supersaturated Solutions Solution, in which the concentration of solute is that determined by...
Saturated, Unsaturated & Supersaturated Solutions Solution, in which the concentration of solute is that determined by its solubility (at given temperature) is called SATURATED solution. One cannot add more solute to such a solution. We also say that a saturated solution is in equilibrium with pure solute: If we add solid Nacl to an already saturated solution of NaCl, that solid remains in equilibrium with dissolved Naci. Solution containing less solute than would be in the saturated solution, is UNSATURATED...
please answer all dmperstu Use the solubility curve provided on the right to determine the answers to the followi...
please answer all
dmperstu Use the solubility curve provided on the right to determine the answers to the following questions: 7. How many grams of solute are required to saturate 100 g of water in each of the following solutions? a) KCL at 80 C b) KCIO, at 90°C c) NaNO, at 10°C d) SO2 at 20 °C e) NH Cl at 70°C esd. 8. What is each of the solutions below: saturated, unsaturated or supersaturated? All of the solutes...
please help me with all the steps. 15. Which of the following mixtures would result in...
please help me with all the steps.
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3. Which of the following changes to a saturated solution of Mg(OH)2 will cause the solubility of Mg(OH)2 to increase, dissolving more of the solid? A. Addition of soluble NaOH B. Addition of soluble Mg(NO3)2 C. Addition of Mg(OH)2(5) D. Lowering the pH of the solution E. Increasing the pH of the solution 4. Which of the following best describes the redox reaction occurring in the hydrogen fuel cell? A. H2 + 2OH → 2H2O B. H* + OH-H20 C....
e) volume. d) number of moles of solute. 14) Which of the following substances would be the most soluble in water? a) AgC1 b) NaCl c) PbCl2 d) Hg2Cl2 15) What is the molarity of the resulting solution when 300. mL of a 0.400 M solution is diluted to 800. mL? (2 point)
answer 1-4
Which of the following (a-d) is TRUE regarding solid NaCl dissolving in water The attraction of the water to the ions in NaCl is through dipole-dipole IFs. Water is considered the solute and NaCl the solvent. The partially positive oxygen in water is attracted to the chloride ion. d. The process of separating the sodium ions from the chloride ions is endothermic. All of these statements are true. polar For the following solution, describe the deviation with respect...
g. Which of the following situations would most likely cause gases to deviate from a) Low pressure and high temperature b) High pressure and low temperature c) High pressure and high temperature d) Gases never deviate from ideal behavior e) Low pressure and low temperature 10. A gas mibxture has three components Na. F and He, their partial pressures are 0.45 atm, 0.160 atm and 0.20 atm respectively. What is the pressure of the gas mixture? a) 1.05 atm b)...
1.What would be the predominate form(s) of the following elements in a pH-7 aqueous solution each under the following conditions. Remember that more than one compound may be present in a solution. For each element, provide the species under the three following conditions. a) saturated with 02 b) saturated with air c) saturated with H2 A. Nb B. Tc C. Co D. Cu E. Fe
10 Equal masses of the following non-volatile solutes are dissolved in 1000g of H20(0). Which solution will have the LOWEST freezing point. A. NaCl B. KCI C. LiCl D. CsCl E. RbCl Suppose that the reaction A → products proceeds in one step and is exothermic. It has an activation barrier of 75 k/mol. How would the energy diagram change if a catalyst is added to the reaction? Select all the statements that could be true. 11 Addition of the...
Saturated, Unsaturated & Supersaturated Solutions Solution, in which the concentration of solute is that determined by its solubility (at given temperature) is called SATURATED solution. One cannot add more solute to such a solution. We also say that a saturated solution is in equilibrium with pure solute: If we add solid Nacl to an already saturated solution of NaCl, that solid remains in equilibrium with dissolved Naci. Solution containing less solute than would be in the saturated solution, is UNSATURATED...
please answer all
dmperstu Use the solubility curve provided on the right to determine the answers to the following questions: 7. How many grams of solute are required to saturate 100 g of water in each of the following solutions? a) KCL at 80 C b) KCIO, at 90°C c) NaNO, at 10°C d) SO2 at 20 °C e) NH Cl at 70°C esd. 8. What is each of the solutions below: saturated, unsaturated or supersaturated? All of the solutes...
please help me with all the steps.
15. Which of the following mixtures would result in a buffered solution? a. Mixing 100.0 mL of 0.100 M HCl with 100.0 mL of 0.100 M NaOH. b. Mixing 100.0 mL of 0.100 M NH3 (K5=1.8 x 10-5) with 100.0 mL of 0.100 M NaOH. c. Mixing 100.0 mL of 0.100 M HCl with 100.0 mL of 0.100 M NH; (K =18x 10 %. d. Mixing 50.0 mL of 0.100 M HCl with...
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