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August 30, 2014

Homework Help: More Chemistry

Posted by Liz on Thursday, February 15, 2007 at 7:48pm.

I have the answers, I just want to be sure...I'm a little hesitant..


1. Explain how strong acid solutions conduct an electric current:

-Strong acids readily release ions creating electro negativity.

2. Will a strong acid or weak acid conduct electricity better? Why?

-A strong acid because the readily releasing ions have more energy.

3. Balance:
CaCO3+HCl->CaCl2+H2O+CO2

I got CaCO3+2HCl->CaCl2+H2O+CO2

4. Write the net ionic equation of the above reaction:

I got 2HCl->Cl2+H2O


5. Identify spectator ions:
Ca and CO

6. Write the two equations that show the two stage ionization of sulfurous acid in water:

H2SO3+H20-> H3O+ SO

I really donít know how to do this one..


Thanks...but that doesn't really help..

1. Explain how strong acid solutions conduct an electric current:

-Strong acids readily release ions creating electro negativity.

Yes, they release ions and it is the ions that conduct the electric current from one electrode to the other. The positive ions travel to the negative electrode and the negative ions travel to the positive electrode. Creating electronegativity, whatever that means, doesn't have anything to do with it. It's all with the ions.

2. Will a strong acid or weak acid conduct electricity better? Why?

-A strong acid because the readily releasing ions have more energy.

A strong acid is correct but not for that reason. Strong acids are 100% ionized; weak acids are only partially ionized (less than 100% and many in the range of < 1% to 5%). Therefore, strong acids produce more ions and more ions can conduct more electricity.

3. Balance:
CaCO3+HCl->CaCl2+H2O+CO2

I got CaCO3+2HCl->CaCl2+H2O+CO2
very good

4. Write the net ionic equation of the above reaction:

I got 2HCl->Cl2+H2O

No. You have the molecular equation written and balanced correctly. Now convert to the ionic equation. Strong electrolytes ionize completely, solids and gases as well as weak electrolytes are written as the molecule.
Ca^+2 + CO3^-2 + 2H^+ + 2Cl^- ==>Ca^+2 + 2Cl^- + H2O + CO2
Next, cancel those ions that appear on both sides of the equation.
Ca^+2 cancels. 2Cl^- cancels. What is left is the net ionic equation.
CO3^-2 + 2H^+ ==> H2O + CO2


5. Identify spectator ions:
Ca and CO
The spectator ions are those that canceled.


6. Write the two equations that show the two stage ionization of sulfurous acid in water:

H2SO3+H20-> H3O+ SO

H2SO3 ==> H^+ + HSO3^-
HSO3^- ==> H^+ + SO3^-2



6. Write the two equations that show the two stage ionization of sulfurous acid in water:

H2SO3+H20-> H3O+ SO

H2SO3 ==> H^+ + HSO3^-
HSO3^- ==> H^+ + SO3^-2

With this one, we then have to say which stage is favored. I think it's stage 2 because the bonds are stronger. That's what it means, right?

First, I wrote the ionization equation but I didn't show the water. This is how it would look including the water.

H2SO3 + H2O ==> H3O^+ + HSO3^-
HSO3^- + H2O ==> H3O^+ + SO3^-2

Second, look up the ionization constants for H2SO3 in your text. There is a k1, for the first ioniation, and a k2, for the second ionization. As I remember, k1 is about 10^-2 and k2 is about 10-7 (just ball park numbers). The ionization with the larger k is the one that occurs first and most. Using your answer, the bond IS stronger between H and SO3 in the HSO3^-; therefore, that is the one that does not want to take place and that means the OTHER one is favored.

d

write net ionic equations that represent the following reactions:
a. the ionization of HClO3 in water

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