Why space acids weak or strong?Every acid reacts through water. When it loser a proton, it transfers that proton to water. Water acts together a base as soon as it solvates the proton. The conjugate acid is protonated water and it is represented as (H3O)+, (H5O2)+, (H2nOn)+, or just as H+(aq). The conjugate base is the mountain minus the proton.A strong acid is fully dissociated in water when a weak acid is in equilibrium with its conjugate base in water. Let"s look at the reaction the a strong acid, nitric mountain or HNO3, and a weaker acid, nitrous mountain or HNO2, in water.
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Nitric acid is a more powerful acid than nitrous acid because its conjugate basic is more stable. The NO3- ion has excess negative charge spread out out end 3 oxygen atom while the excess an adverse charge in NO2- is spread out out over on 2 oxygen atoms.A conjugate base is an ext stable when the an adverse charge is on one electronegative element and also when the charge is delocalized end multiple atoms. The more stable the conjugate base, the stronger the acid. A steady conjugate base is not really basic. A very solid acid has a really weak conjugate base and a an extremely weak acid has actually a very strong conjugate base.
Weak acid EquilibriumNitrous acid is in equilibrium with a proton and also its conjugate base, NO2-. Because the concentration that water is constant, us can define a consistent equal come the product of the concentration of water and also the equilibrium constant. This constant, the Ka is 10-3.29 for HNO2.
We deserve to use the Ka to identify the pH that a solution of nitrous acid. For example, let"s identify the pH the a equipment made indigenous 0.01 mole that HNO2 in 1.0 together of water. Few of the acid will dissociate into H+ and also NO2- but we don"t recognize w=how much. We"ll contact the molar concentration that solvated proton x for this reason
It is always possible to fix for x by making use of the quadratic equation yet most of the time we can solve it making use of an approximation. If we assume that the level of dissociation is small, then the equilibrium concentration of acid doesn"t change really much from its original concentration. We can then use the original acid concentration in the Ka expression.The approximation is a good one in this case due to the fact that we obtain the very same pH value using it together we walk from the quadratic equation.
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