Reactions within equations and properties of acidity

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A reaction occurs for each of the following below. How do you differentiate between the different driving forces? (a driving force can either be the transfer of electrons; the formation of a precipitate, etc.)

2Na(s) + 2H2O(l) --> 2NaOH(aq) + H2

KOH(aq) + HF(aq) --> KF(aq) + H2O(l)

NaF(aq) + HCl(aq) --> NaCl(aq) + HF(aq)

Pb(NO3)2(aq) + Na2CrO4(aq) --> PbCrO4(s) + 2NaNO3(aq)

NaNO3(aq) + HCl(aq) --> NaCl(aq) + HNO3(aq)

How exactly would I go about finding which one of the following listed solutions below is the most acidic?

1.0 molar HClO3(aq)
1.0 molar HC2H3O2(aq)
1.0 molar HCN(aq)
1.0 molar HNO2(aq)
1.0 molar HF(aq)

Is HC2H3O2(aq) a strong acid?

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See the attachment.

Reactions within equations and properties of acidity
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A reaction occurs for each of the following below. How do you differentiate between the different driving forces? (a driving force can either be the transfer of electrons; the formation of a precipitate, etc.)

2Na(s) + 2H2O(l) --> 2NaOH(aq) + H2

KOH(aq) + HF(aq) --> KF(aq) + H2O(l)

NaF(aq) + HCl(aq) --> NaCl(aq) + HF(aq)

Pb(NO3)2(aq) + Na2CrO4(aq) --> PbCrO4(s) + 2NaNO3(aq)

NaNO3(aq) + HCl(aq) --> NaCl(aq) + HNO3(aq)

For each of the above reactions, you must use the solubility rules to determine ...

Solution Summary

This solution is provided in 449 words in an attached .doc file. It discusses solubility in terms of differentiating driving forces, and using the equilibrium Ka value to determine acidity of substances.

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