The concentration of Mg2+ at equilibrium (25oC) is 0.000144 M. What is the value of Ksp at this temperature?
The concentration of Mg2+ at equilibrium (25oC) is 0.000144 M. What is the value of Ksp...
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)
The reaction MgCO3(s) ⇌ Mg2+(aq) + CO32-(aq) has Ksp = 6.8x10-6 at 25oC. The reaction MgCO3(s) = Mg2+(aq) + C032 (aq) has Ksp = 6.8x10 at 25°C. What is the value of Osp when [Mg2+] = 0.00150 M and (CO321 = 0.00120 M? 2.2x10-9 1.8x10-6 O 3.2x10-12 5.6x105 Under these concentration conditions given in the question above, is this reaction moving in the forward or reverse direction to reach equilibrium? Why? forward, because Q>K forward, because Q<K reverse, because Q>K...
Using the appropriate Ksp values, find the concentration of NO3- ions in the solution at equilibrium after 600 mL of 0.45 M aqueous Cu(NO3)2 solution has been mixed with 400 mL of 0.25 M aqueous KOH solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19). Submit Answer Tries 0/99 Now find the concentration of OH ions in this solution at equilibrium. (Enter in M.) Submit Answer Tries 0/99
Help with equilibrium questions?Magnesium hydoxide is only very slightly soluble inwater. The reaction by which it goes into solution is :Mg(OH)2? Mg2+ +2OH-a. Formulate the expression for the equilibrium constant, Ksp, for he above reaction.b. It is possible to dissolve significant amounts of Mg(OH)2 in solutions in which the concentration ofeither Mg2+ or OH- is very , very small. Explain, using Ksp, whythis is thecase.c. Explain why Mg(OH)2 might have very appreciable solubility in 1 M HCl.
The concentration of Mg2+ in seawater is 5.0 * 10-2 M. What hydroxide concentration is needed to remove 90% of the Mg2+ by precipitation? (For Mg(OH)2, Ksp - 12 * 10-11)
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) Your answer should include three significant figures.
If the concentration of Mg2+ ion in seawater is 1.21x103 mg/L, what OH- concentration is required to precipitate Mg(OH)2 ? Ksp(Mg(OH)2)=5.6x10-12 -OH concentration must be greater than _____ M.
If the concentration of Mg2+ ion in seawater is 1.29 × 103 mg/L, what OH concentration is required to precipitate Mg(OH)2? Ksp (Mg(OH)2) 5.6x 10-1 OH- concentration must be greater than M.
please help me with these questions! Thank you :-) What concentration of so-is in equilibrium with Ag,SO,(s) and 1.00 x 10-3 M Agt? The Kap of Ag,SO, can be found in this table. [s03-] = The Ksp of cadmium carbonate, CACO3, is 1.0 x 10-2. Calculate the molar solubility, S, of this compound. At 25 °C, only 0.0290 mol of the generic salt AB2 is soluble in 1.00 L of water. What is the Ksp of the salt at 25...
The "insoluble" salt, silver sulfide, has a solubility product, Ksp=6.3*10^-51 at 298 K. Ag2S(s)=2Ag+ (aq)+ S2-(aq) What is the concentration of Ag+ at equilibrium, at this temperature?