HA and HB are both weak acids although HB is the
stronger of the two. Will it take a larger volume of
a 0.10 M NaOH solution to neutralize 50.0 mL of
0.10 M HB than would be needed to neutralize 50.0
mL of 0.10 M HA?
Absolutely not.
50 mL 0.1M HA or 50 mL of 0.1M HB will take exactly the same amount of 0.1M NaOH to neutralize each.
ddwds
To determine whether a larger volume of a 0.10 M NaOH solution is required to neutralize 50.0 mL of 0.10 M HB compared to 50.0 mL of 0.10 M HA, we need to consider the concept of acid strength and the neutralization reaction. Here's the step-by-step breakdown:
1. Acid strength: In this scenario, it is mentioned that HB is the stronger acid compared to HA. This indicates that HB has a higher tendency to dissociate and release H+ ions in solution.
- Strong acid: completely dissociates in water, releasing all its H+ ions.
- Weak acid: partially dissociates in water, releasing only a small fraction of its H+ ions.
2. Neutralization: The neutralization reaction involves the reaction between an acid and a base. In this case, a strong base (NaOH) will react with the weak acids (HA and HB).
- NaOH (sodium hydroxide) is a strong base that dissociates completely in water, releasing OH- ions.
- The reaction between an acid and a base results in the formation of water and a salt.
3. Volume of NaOH solution needed: The volume of NaOH solution required to neutralize an acid is directly proportional to the amount of H+ ions present in the acid solution.
- Since HB is the stronger acid, it will have a higher concentration of H+ ions compared to HA.
Based on these factors, it will indeed take a larger volume of a 0.10 M NaOH solution to neutralize 50.0 mL of 0.10 M HB compared to neutralizing 50.0 mL of 0.10 M HA. This is because HB is the stronger acid and has a higher concentration of H+ ions.
To determine if it will take a larger volume of a 0.10 M NaOH solution to neutralize 50.0 mL of 0.10 M HB compared to neutralizing 50.0 mL of 0.10 M HA, we need to consider the concept of acid strength and the concept of molar ratios in a neutralization reaction.
1. Acid Strength: HA and HB are both weak acids, but HB is stronger. This means that HB will ionize more in water compared to HA, resulting in a higher concentration of hydrogen ions (H+).
2. Neutralization Reaction: When an acid reacts with a base, they undergo a neutralization reaction, resulting in the formation of water and a salt. In this case, the base is NaOH, which dissociates in water to form Na+ and OH- ions.
In a neutralization reaction between an acid and a base, the moles of hydrogen ions (H+) from the acid are equal to the moles of hydroxide ions (OH-) from the base. This forms water.
In both cases, 50.0 mL of 0.10 M HB and 50.0 mL of 0.10 M HA correspond to the same number of moles of acid.
3. Molar Ratios: Since the concentration of the NaOH solution is given as 0.10 M, it means that in every 1 liter of solution, there are 0.10 moles of NaOH. Therefore, the molar ratio between NaOH and H+ (or OH-) is 1:1.
Given that the number of moles of acid is the same for both HB and HA, and the molar ratio between NaOH and H+ (or OH-) is 1:1, it will take the same volume of 0.10 M NaOH solution to neutralize both 50.0 mL of 0.10 M HB and 50.0 mL of 0.10 M HA.
In summary, even though HB is a stronger acid than HA, it will not require a larger volume of 0.10 M NaOH to neutralize since the molar ratios and number of moles for both acids are the same.