Consider the following acids: H2S, H3PO4.
Write the formula of the conjugate base for H≥S.
Express your answer as an ion.
The conjugate base for H2S is HS-.
To determine the formula of the conjugate base for H2S, we need to remove a hydrogen ion (H+) from H2S.
H2S loses one hydrogen ion to form its conjugate base. The chemical formula for the conjugate base of H2S is HS^-.
To determine the formula of the conjugate base for H−S, we need to understand the concept of conjugate acids and bases.
A conjugate base is formed when an acid donates a proton or H+ ion. In this case, H−S is the acid since it can donate a proton.
To write the formula of the conjugate base, remove the acidic hydrogen (H+) and keep the remaining part of the formula intact. Thus, the conjugate base of H−S would be S2−. This is because when H+ from H−S is removed, it leaves behind S2−, which has gained two electrons to maintain charge neutrality.
Therefore, the formula of the conjugate base for H−S is S2−.