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Answer:
A Bronsted acid acts as a reversible proton donor in aqueous solution by undergoing a dissociation reaction. If the acid is monoprotic, then each particle of the acid donates one proton each. This also forms a conjugate base product. If the equilibrium state of the reaction is very product favored, then the acid is described as being strong. In general, complete dissociation of the starting acid molarity is assumed here, so both the reversibility and the equilibrium state can be ignored during pH calculations.
Answer and Explanation: 1
The formula shown is nitric acid. It is a strong monoprotic acid. It will completely dissociate in aqueous solution to provide the same molarity of hydrogen ion:
HNO3(aq)→H+(aq)+NO−3(aq)HNO3(aq)→H+(aq)+NO3−(aq)
Before dissociation we have:
[HNO3]=0.010 M[HNO3]=0.010 M
After dissociation we have:
[H+]=0.010 M[H+]=0.010 M
The solution pH will be:
pH=−log[H+]pH=−log(0.010 M)pH=2.0
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