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Answer :
HClO4, it’s the strongest acid of the bunch therefore it would have the lowest ph.
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2.00 M HClO4 would have the lowest pH due to its complete dissociation into H+ ions, indicating higher acidity. H2SO4 and HBr would also have low pH, while NaOH and HNO2 would have higher pH values. Option A.
To determine which solution would have the lowest pH, we need to compare the acidity of each compound. pH is a measure of the concentration of hydrogen ions (H+) in a solution, and the lower the pH, the higher the concentration of H+ ions, indicating higher acidity.
Let's evaluate each option:
A.) 2.00 M HClO4:
HClO4 is a strong acid that dissociates completely in water to produce H+ ions and ClO4- ions. Since it is a strong acid, it will yield a high concentration of H+ ions, resulting in a low pH. Thus, option A has the lowest pH.
B.) 2.00 M H2SO4:
H2SO4 is also a strong acid that dissociates completely in water to produce 2H+ ions and SO4^2- ions. Similar to HClO4, it will have a high concentration of H+ ions and a low pH.
C.) 2.00 M NaOH:
NaOH is a strong base that dissociates into Na+ and OH- ions. While it contributes to the hydroxide ion (OH-) concentration, it does not directly contribute to H+ ions, so its pH will be high (alkaline), not low.
D.) 2.00 M HBr:
HBr is a strong acid like HClO4 and H2SO4, and it will have a low pH due to a high concentration of H+ ions.
E.) 2.00 M HNO2:
HNO2 is a weak acid that only partially dissociates in water to produce H+ ions and NO2- ions. Since it is a weaker acid compared to the options above, it will have a higher pH, not the lowest. So Option A is correct.
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