In a saturated solution of MgF2 at 16 °C, the concentration of Mg2+ is 1.44x10 –3 M
The equilibrium is represented by the equation
MgF2 -->Mg 2+ + 2 F-.
A.Write the expression for the solubility product constant, Ksp.
B.Calculate the value of Ksp at 16°C for MgF2
Note: Your answer is assumed to be reduced to the highest power possible.
C.Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 16°C to which 0.450 mole of solid KF has been added. The KF dissolves completely and causes no change in volume.
Note: Your answer is assumed to be reduced to the highest power possible.
D.Calculate Q to determine if a precipitate will form when 250.0 mL of a 0.00200 M solution of Mg(NO3)2 is mixed with 250.0 mL of a 0.00200 M NaF solution at 16°C.
Note: Your answer is assumed to be reduced to the highest power possible.
E.Does a precipitate form? yes or no
F.At 24°C the concentration of Mg2+ in a saturated solution of MgF2 is 1.87 x 10 –3 M.
Is the dissolving of MgF2 in water an endothermic or exothermic process. Give an explanation to support your choice. choose one of the choice below to answer F.
|
|||
|
|||
|
|||
|
In a saturated solution of MgF2 at 16 °C, the concentration of Mg2+ is 1.44x10 –3...
MgF2(s) <--> Mg2+(aq) + 2 F–(aq) In a saturated solution of MgF2 at 18 0C, the concentration of Mg2+ is 1.21 x 10–3 molar. The equilibrium is represented by the equation above. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 0C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 liter of saturated MgF2 solution at 18 0C to which 0.100 mole of solid KF has been added. The KF dissolves completely. Assume...
A saturated solution of magnesium fluoride , MgF2, was prepared by dissolving solid MgF2 in water. The concentration of Mg2+ ion in the solution was found to be 1.18
If the concentration of a saturated solution of MgF2 is 0.000216 M, What is the Ksp for MgF2? Units are not required. Round your answer to two decimal places. Report answers in scientific notation in the form provided in the following example. (ex. 4.57e-15)
What is the concentration of iron(II) ions in a saturated solution of iron(II) sulfide? Ksp(FeS) = (3.765x10^-19) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: Question 68 options: x10 Answer units
b. MgCl, is dissolved in distilled water at 25°C until the saturated solution is obtained (system reaches equilibrium). The concentration of Mg2 in the saturated solution is 1.35 x 10-'M. The dissolution of MgCl, in distilled water is endothermic. Write the balanced chemical equation to obtain the saturated solution Calculate the solubility product, K of MgCl2. Explain the effect of increasing the temperature on the amount of MgCl, Justify your answer. C. When solid Pbl, is added to pure water...
3. What is the concentration of all species at equilibrium for a saturated solution or Ag3AS04 given that the Ksp for this salt is 1.03 x 10-22? What is the concentration of all species at equilibrium for the same salt in a solution that already has a concentration of silver ions of 0.1 M?
Data Sheet Experiment 1 (Room Temperature): Temp. of Saturated Borax Solution: 2 c ka HCI Concentration: A Trial 2 Trial 1 Volume of borax solution titrated: Initial Burette Reading Final Burette Reading 14.62 m jt.k2 1462 E2 mo Volume of HCl used Moles of HCI used Moles of B&Os(OH)2 present in titrant Concentration of BaOs(OH) in titrant 29 34 A2926 Concentration of Na' in titrant Average Conc. of B4Os(OH)e2 in titrant Op294 Average Conc. of Na in titrant Ksp= KEquilibrium...
Please answer all! 1. a. Calculate the moles of Calcium hydroxide in a solution if 32.4 mL of saturated calcium hydroxide solution is titrated with 0.0500M HCl. 14.90mL of HCl was needed to completely react with the calcium hydroxide. (5pts) 2. a.) Calculate the free energy in a saturated solution of Ca(OH)2 if the Ksp = 6.5x10-6 at 25?C. Show all work. (5pts) b.) Is the reaction spontaneous or nonspontaneous? Briefly explain your answer. (5pts) 3. What is the symbol...
help Misert Draw Design Layout References Mailings >> Share Comme Times New... 16 A A Aa Ao BI U rab x X² AvovArt Paragraph Styles Sensitivity 3. Adjust the temperature for an endothermic reaction. Then adjust the temperature for an exothermic reaction. What happens? Sign of AH / When T'increases, K... When I decreases, K... Positive (endothermic) Negative (exothermic) a. Write the chemical equation for the endothermic reaction when An = 0. Is heat a reactant or a product? b....
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...