Hi, I'm not sure how to approach this problem:
A monoprotic weak acid, HA , is ionized according to the reaction
HA(aq)+H2O(l)↽−−⇀A−(aq)+H3O+(aq) pKa=4.26
where A− is the conjugate base to HA.
For this weak monoprotic acid, the predominant species present at pH 5.57 is
-charged
-neutral
-unknown
Sapling #13
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Re: Sapling #13
Hi! To determine whether it is charged or neutral, compare the pH and the pKa. If the pH is less than the pKa, then it is negatively charged, otherwise it's neutral.
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Re: Sapling #13
Hi! To get the answer, you need to compare the pH and pKa. If the pKa is lower than pH, which means the HA is more acidic than the solution, HA will be ionized into H+ and A-. Thus this acid is negatively charged. Otherwise, (pKa is higher than pH), it'll remain neutral.
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Re: Sapling #13
Like previous answers, you need to compare pH and pKa. If pKa is lower, then it is negatively charged. If pKa is higher, it is neutral
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