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Now, the molar solubility of this generic salt #"X"_n"Y"_m# tells you the number of moles of salt that can be dissolved in one liter of solution to form a saturated solution. Let's assume that you are given a molar solubility equal to #s# #"mol L"^(-1)# for this salt in water at room temperature.
s=5.65xx10^(-5)g/L Manganese(II) carbonate dissociate in water according to the following equation: MnCO_3(s)rightleftharpoonsMn^(2+)(aq)+CO_3^(2-)(aq)" " "K_(sp)=2 ...
Now, the molar solubility of the compound, #s#, represents the number of moles of lead(II) chloride that will dissolve in aqueous solution at a particular temperature. Notice that every mole of lead(II) chloride will produce #1# mole of lead(II) cations and #color(red)(2)# moles of chloride anions. Use an ICE table to find the molar solubility ...
In your case, the molar solubility of magnesium fluoride will be 6.4 * 10^(-7)"mol/L". You need the value of the solubility product constant, K_(sp), for magnesium fluoride; now, there are several values listed for K_(sp), so I'll choose one -> 6.4 * 10^(-9). If this is not the value given to you, just replace it in the calculations with whatever value you have. So, the equilibrium equation ...
How do you calculate the solubility (moles/L) of Mg(OH)2 in water.The Ksp=#5.0*10^-11#? Chemistry Chemical Equilibrium Solubility Equilbria. 1 Answer
This time, you're interested in finding the molar solubility of silver sulfate in a solution that is #"0.10 M"# silver nitrate, #"AgNO"_3#. Unlike silver sulfate, silver nitrate is soluble in aqueous solution, which means that it dissociates completely to form silver cations and nitrate anions
This is the molar solubility. (b) To find the mass solubility we multiply by the mass of 1 mole. I will assume we are using the anhydrous salt #sf(CaSO_4)# for which the #sf(M_r=136.1)# #:.# Mass solubility = #sf(4.9xx10^(-3)xx136.1=0.67color(white)(x)"g/l")#
The Ksp of cobalt(II) hydroxide, #Co(OH)_2#, is #5.92 × 10^-15#. Calculate the molar solubility of this compound?
The closest value is c. K_text(sp) = 4.9 ×10^"-17" > Step 1. Calculate the molar solubility s = (2.1 × 10^"-4" color(red)(cancel(color(black)("g"))))/"1 L" × "1 ...
Here's how you can do that. What you need to do here is set up an ICE table based on the equilibrium reaction that describes the way barium sulfate, "BaSO"_4, dissolves in aqueous solution. The salt is considered insoluble in water, so right from the start you know that the solution will contain very little amounts of dissolved ions, since most of the compound will remain undissociated as a ...