In a saturated solution that is in contact with solid Mg(OH)2, the concentration of Mg2+ is 1.12×10–4 M. What is the solubility product for Mg(OH)2?
Mg(OH)2(s)⇌Mg2+(aq)+2OH−(aq)
In a saturated solution that is in contact with solid Mg(OH)2, the concentration of Mg2+ is...
In a saturated solution that is in contact with solid Pb(IO3)2, the concentration of Pb2+ is 1.79 x 10-5 M. What is the solubility product for Pb(103)2? Pb(10g),(s) – Pb²+ (aq) + 210(aq) Select the correct answer below: O 2.29 x 10 O 6.74 x 10-15 O4,50 10-14 O 6.41 x 10-10
(aq) (1) Mg(OH)2 is partially dissolved in water: Mg(OH), (s) = Mg2+ (aq) + 2OH Write the Kop expression for Mg(OH)2 : Kp = (2) Solid AgCl is partially dissolved in water: AgCl 2 Ag+ + CI''. If the molar solubility is known as [Ag +) = [CI''] = 1.3x 10 M, AgCl Kip =- (a) 1.3 x 10 (b) 1.69 x 10-10 (c) 2.6 x 10 (d) none of these (3) At 25 °C, the solubility of solid AgCl...
How should the solid compound Mg(OH)2 be represented in a net ionic equation? Mg(s) + (OH)2(s) Mg(OH)2(s) Mg2+(s) + (OH-)2(s) Mg2+(aq) + 2OH- (aq) Mg2+(s) + 2OH-(s)
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...
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...
What is Ksp for the following equilibrium if Mg(OH)2 has a molar solubility of 1.1×10−4 M? Mg(OH)2(s)↽−−⇀Mg2+(aq)+2OH−(aq)
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....
An acidic solution is 0.01 M in Mg2+, Cu2+, and Fe2+. The pH of the solution is adjusted by adding NaOH. What is the maximum pH that removes only the Cu2+? Mg(OH)2(s) ↔ Mg2+(aq) + 2OH–(aq) Ksp = 6.3 x 10–10 Fe(OH)2(s) ↔ Fe2+(aq) + 2OH–(aq) Ksp = 4.1 x 10–15 Cu(OH)2(s) ↔ Cu2+(aq) + 2OH–(aq) Ksp = 2.2 x 10–20
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 85 ∘C , where [Fe2+]= 3.60 M and [Mg2+]= 0.210 M 1) What is the value for the reaction quotient, Q, for the cell? Express your answer numerically. 2) What is the value for the temperature, T, in kelvins? Express your answer to three significant figures and include the appropriate units. 3) What is the value for n? Express your answer as an integer and include the appropriate units (i.e. enter mol for moles). 4)...
Hydroxyapatite, Ca10(PO4)6(OH)2 , has a solubility constant of Ksp = 2.34×10−59 , and dissociates according to Ca10(PO4)6(OH)2(s)↽−−⇀10Ca2+(aq)+6PO3−4(aq)+2OH−(aq) Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca2+ in this solution if [OH−] is fixed at 1.40×10−6 M ?