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Sagot :
From the list, the FIRST option, is much more acidic, Since Cl are reppealing, pair is the stronger acid
Let's first define acid: Acids and Bases of Bronsted Lowery, Let's define the terms "Bronsted Lowry acid/base" first. Anything that will donate H+ (protons) to a solution and lowers pH is considered a Bronsted Lowry acid (i.e HCl) Any species that accepts H+ (protons) in solution and raises pH (NH3 accepts H+ to produce NH4+) is referred to as a Bronsted Lowry base. Commonly, acid/bases are displayed in the left (reactants), when we scribe the goods: When the B.L. acid contributes its H+ proton (HCl to Cl-), a base known as a Bronsted Lowery conjugate is created. The acid produced when a base accepts its H+ proton, such as NH4+, is known as a Bronsted Lowery conjugate acid. The right (product) side is normally where conjugate bases and acids are displayed.For this case the only acidic proton is that of OH group Then we need plenty of negative species , such as Cl near the OH to favour donation of H+ the long chain will maintain far away the electronegativity so avoid long chains
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