Do you have a solubility or a Ksp to use. There is a good bit of disagreement on the net about the correct value for Ksp for MgCO3.
Oh sorry the Ksp=4x10^(-5)
MgCO3 ==> Mg^+2 + CO3^-2
Ksp = (Mg^+2)(CO3^-2) - (x)(x)
x = sqrt(4E-5) = 0.00632 moles/L or 0.00632 x 84 = 0.531 g/L
In 500 mL there will be 1/2 that or .265 grams.
If we evaporate water until the volume is 120 mL, then 0.531 g/L becomes
0.531 g/L x (120 mL/1000 mL) = 0.0637 g.
We started with 0.265 g in 500
............less 0.0637 in 120 mL =
solid ppting.....0.201 g which rounds to 0.2 g to 1 significant figures (from the Ksp value).
Thanks! But im confused on why you would subtract the .0637g in 120mL from .265g in 500mL. Why dont you do (grams from 500mL-grams from 380mL)?
NO Soup For You!
(10 points possible)
Calculate the number of moles of nitrogen dioxide, NO2, that could be prepared from 79.0 mol of nitrogen oxide and 82.0 mol of oxygen.
79 - correct
Identify the limiting reagent and the excess reagent in the reaction. What would happen to the potential yield of NO2 if the amount of NO were increased?
increase - correct
What if the amount of O2 were increased?
no change - correct
Calculate the wavelength (in m) of a photon capable of exciting an electron in Li2+ from the state n= 3 to the state n=5
1.4239*10^-7 - correct
Charge Me Up, Scotty!
Determine the potential (V) by which a proton must be accelerated so as to assume a particle wavelength of 0.0293 nm.
0.9544 - correct
PES S+P 500
Shown below are the photo electron spectra for phosphorous and sulfur
The PES spectra for phosphorous and sulfur are shown above. Answer the following questions concerning these spectra.
Why is the phosphorous peak at 1.06 MJ/mole greater in energy than the sulfur peak at 1.00 MJ/mole?
paired electron easier to remove - correct
Why is the phosphorous peak at 1.95 less energy than the sulfur peak at 2.05?
sulfur has larger Z - correct
What should be the ratio of intensities of the phosphorous peak at 1.06 to the phosphorous peak at 13.5?
1/2 - correct
/* 1-5 */
You'll Learn About Electrons, I Guarantee It
Which of the following orbital diagrams is/are incorrect for all electrons in the lowest-energy levels of an atom?
1,2,4 - correct
Which of the following is the correct electronic configuration for the bromide ion, Br-?
[Ar]4s23d104p6 - correct
Which of the following orders of filling orbitals is/are incorrect? They should be in the exact order that they would be filled in.
3s, 4s, 5s - correct
5s, 5p, 5d - correct
5s, 4d, 5p
6s, 4f, 5d
6s, 5f, 6p - correct
CaF2, Great for Teeth!
Calculate the lattice energy of CaF2 given the information below (in kJ/mol):
- 2615.4 - correct
Select the single most important reason below to justify your choice should have the higher melting point
- Both molecules are nonpolar but the higher melting includes hydrogen bonding
- Both molecules are nonpolar but the higher melting is more polarizable
- The higher melting molecule is polar and the other is not
- The lower melting molecule is polar and the other is not
- The higher melting molecule has smaller Van der Waals forces than the lower melting
- The higher melting molecule has greater Van der Waals forces than the lower melting
- The higher melting molecule is ionic and the other is not
- The lower melting molecule is ionic and the other is not
- The higher melting molecule has hydrogen bonds and the other does not
- The lower melting molecule has hydrogen bonds and the other does not
- Both molecules are ionic but the higher melting has a larger cohesive energy
- Both molecules are ionic but the lower melting has a larger cohesive energy
- The higher melting molecule is ionic and the other is not.
- Ionic bonds are stronger than hydrogen bonds
- The lower melting molecule is ionic and the other is not.
- onic bonds are weaker than hydrogen bonds
- The higher boiling molecule is ionic and the other is not.
- Ionic bonds are stronger than Van der Waals forces
- The lower boiling molecule is ionic and the other is not.
- Ionic bonds are weaker than Van der Waals forces
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