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19 Nov 2019

Hey could someone please help me with this mix how it dissociate in water: KH2PO4+KCl+Mg(NO3)2x6H2O+Ca(NO3)2x4H2O+KNO3+CH4N2O+NH4NO3

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Trinidad Tremblay
Trinidad TremblayLv2
27 Apr 2019

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Related questions

Can someone please help me?! I've been trying but can'tfigureout how to write a equation for these reactions.....
Ca(NO3)2 + Na2CO3 + CO2 --->
Ca(NO3)2 + Na2CO3 + HCI ---->
Ca(NO3)2 + NaHCO3 ----->
Ca(NO3)2 + NaHCO3 + heat ---->
Ca(NO3)2 + NaHCO3 + heat + HCl----->
Ca(NO3)2 + solid CaCO3 + HCl---->
Thanks very much! Really appreciate it!

Which of the following aqueous samples has the lowest vapor pressure above the pure liquid? (For ionizing solutes, assume complete ionization, with no ion-pairing.)

a) 0.4 m NH4NO3 b) 0.5 m Na2SO4 c) 0.2 m Ca(NO3)2

d) 0.3 m KCl AND 0.2 m Na2SO4 e) pure water

I know that for V.P. the solution with the greatest number of disruption sites will have the lowest V.P. I don't understand how to find the ions/formula unit. Please explain how to find thay using the examples above.

Put five drops of 0.1 M Ca(NO3)2 in well A1. Put four drops of distilled water in wells A2 through A7. Use the fine tip pipet to put two mini drops from A1 into A2. Return the excess solution back into well A1. Mix the solution in well A2 by drawing it up into the fine tip pipet and returning it several times. Use the fine tip pipet to put two mini drops from A2 into A3. Mix as in procedure 4. Return the excess solution back into well A2. Put two mini drops from A3 into A4 and mix the solution. Continue this procedure with wells A5, A6, and A7. Discard two mini drops from A7.

A1 initial concentration of calcium nitrate- 0.1 M (five drops Ca(NO3)2)

A2 initial concentration- 0.02 M (four drops distilled water in A2-A7)

A3- 0.004

A4- 0.0008 M

A5- 1.6 x 10^-4 M

A6- 3.2 x 10^-5 M

A7- 6.4 x 10 ^-6 M

The lab then asks to put one drop of 0.1 M NaC2O4 in each well and stir, wait five minutes and look for the first well that has no precipitate. I found that as well A5. Please help!

4. Calculate the concentrations of Ca2+ and C2O4 2- in the first well without a precipitate. Note: In the well without a precipitate, all the Ca(NO3 )2 and the Na2C2O4 dissolved and disassociated.

5. Use the concentrations of Ca2+ and C2O4 2- that you determined above to calculate the solubility product constant of CaC2O4.

6. Molecular motion increases with temperature. How does temperature affect the observed value of the solubility product constant? Why?

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