Interpretation:
p-nitrophenol is a stronger acid than phenol. This statement has to be accounted.
Concept Introduction:
Stronger and weaker acids:
Stronger acids are more reactive because of their less stability whereas weaker acids are less reactive because of their more stability. Stronger acids have high
Acidity with respect to resonance contributors:
The compounds with more resonance contributors are meant to be more acidic than those with less resonance contributors. It is because, the effective delocalization of electrons among more resonance contributors enables the acidic proton to be easily removed and hence the compounds with more resonance contributors are meant be more acidic whereas the less effective delocalization of electrons among less resonance contributors does not enable the acidic proton to be easily removed and hence the compounds with less resonance contributors are meant be less acidic.
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Organic Chemistry
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- Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name formula C;H,N |1.7 × 10~9 4 hydrofluoric acid HF 6.8 × 10 pyridine 10 4.9 x 10 alo 4 hydrocyanic acid НCN ethylamine C2H,NH, | 6.4 × 10 Ar Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the sofution t will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M C2H5NH3B choose one 0.1 M C5H5NHCI choose one v 0.1 М KI choose one v 0.1 M KF choose onearrow_forwardCalculate the pH at 25°C of a 0.68 M solution of potassium butanoate (KC3H7CO2). Note that butanoic acid (HC3H7CO2) is a weak acid with a pKa of 4.82.arrow_forwardHow is SO3 more acidic than MgO? SO3 + H2O = H2SO4 so it can give two (H+) but MgO + H2O = Mg(OH)2, wouldn't it therefore also be able to give 2 (H+) making it just as acidic as SO3? can someone explain?arrow_forward
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