The answer is b. The solubility of Ca(CH3COO)2 will increase.
Since the solution becomes hot when Ca(CH3COO)2 is dissolved, the dissolution is exothermic, and the heat is released together with the dissolved ions:
Ca (CH3COO) 2 (s) == Ca2 + (aqueous solution) + 2 CH3COO- (aqueous solution) + heat
According to Le Chatelier's principle, lowering the temperature can eliminate heat and shift the balance to the right.
Therefore, the reaction will proceed in the forward direction, and more Ca(CH3COO) 2 will be dissolved, resulting in an increase in solubility.
When solid Ca(CH3COO)2 is dissolved in a nearly saturated solution of Ca(CH3COO)2 the solution...
Please explain every part, especially the equilibrium
shifts
6. When a saturated solution of LiCI was chilled some solid solute formed. Answer parts a. - d (12) LiCl (s) Li+ (aq) + Cl. (aq) → a. The stress placed on the system was (an increase / a decrease) in temperature. b. The system's response was an attempt to (increase / decrease) the temperature. c. As a result the equilibrium shifted to the (right/ left) and the solubility of LiCI (increased...
It is found when an unknown solid solute is dissolved in water that the solubility of the solid increases if temperature is increased. What can be determined about the entropy and enthalpy of the dissolution of this unknown solid? entropy is decreased, exothermic O entropy is increased, endothermic not enough information to make a determination entropy is decreased, endothermic entropy is increased,exothermic
It is found when an unknown solid solute is dissolved in water that the solubility of the solid...
1. A solution in which the dissolved solute is in dynamic equilibrium with the solid solute is called: A) an unsaturated solution B) a dilute solution C) a supersaturat ed solution D) a concentrated solution E) a saturated solution F) vant Hoff solution G) none of the above are correct H) all of the above are correct 2. Which of the following statements is generally TRUE? A) The solubility of a solid is not dependent on either temperature or pressure....
For the saturated aqueous solution of O2(g) at 20 C and 1 atm
with the solubility increase, decrease or stay no charge when the
indicated change occurs?
For a saturated aqueous solution of O2(3) at 20 °C and 1 atm, will the solubility increase, decrease or stay no change when the indicated change occurs? (1) The solubility of O23) [Select] when pressure increases. (2) The solubility of O2(s) [ Select ] when temperature increases.
3. Barium hydroxide Ba(OH)2 was dissolved in pure water at 5 Cuntil a saturated solution was obtained. The pH of this solution was found to be 12.25. a) (2 marks) What is the molar solubility of Ba(OH), in pure water at this temperature? Express your answer in mol/L. Show your work. b) (1 mark) What is the Kp of Ba(OH)2 at this temperature? Show your work. c) (0.5 marks) If Ba(OH)2 was added to a solution already containing 0.100 M...
2. Which of the statements about a solution of a gas dissolved in water is true? a. Increasing the temperature of the solution will increase the solubility of the gas. b. Decreasing the temperature of the solution will decrease the solubility of the gas. c. Increasing the temperature of the solution will decrease the solubility of the gas. d. Increasing the temperature of the solution will not change the solubility of the gas.
A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH)2 as it could hold. A 93.4-mL sample of this solution was withdrawn and titrated with 0.0830 M HBr. It required 88.3 mL of the acid solution for neutralization. (a) What was the molarity of the Ca(OH)2 solution? (b) What is the solubility of Ca(OH)2 in water, at the experimental temperature, in grams of Ca(OH)2 per 100 mL of solution?
A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH)2 as it could hold. A 93.4-mL sample of this solution was withdrawn and titrated with 0.0830 M HBr. It required 88.3 mL of the acid solution for neutralization. (a) What was the molarity of the Ca(OH)2 solution? (b) What is the solubility of Ca(OH)2 in water, at the experimental temperature, in grams of Ca(OH)2 per 100 mL of solution?
When some ionic solids (for example, potassium chloride) are dissolved in room temperature water, the beaker becomes cold. a) Based on this observation, is the enthalpy of dissolution positive, negative or zero? b) Since potassium chloride spontaneously dissolves in water at room temperature, does the entropy of the system increase or decrease as the solid dissolves? Briefly explain your answer. c) Based on your answers to parts a) and b), will potassium chloride become more soluble or less soluble as...
1. The Molar Solubility of Ca(10), in Pure Water Temperature of the saturated solution of calcium iodate: Volume (or mass) of saturated calcium iodate solution titrated: 25 °C 10 ml (or g) Dat Trial 1 Trial 2 Trial 3 Volume of Na S o titrant Final buret reading Initial buret reading ml mL mL mL Net volume of Na So 26.621 mL 30.019 mL Calculated concentration of 10 Standardized 0.05 M sodium thiosulfate (Na,8,0,) solution (10,51(E) - TIL 10 mols.0.2...