What would the effect on your molarity of NaOH be if you had added 35 mL of water to dissolve the KHP (acid) instead of 25 mL? Explain.
My answer so far is that adding more water shouldn't affect the molarity at all because water does not account for the reaction between NaOH and KHP.
This explanation seems rather simple, am I missing something or am I completely wrong? Thanks in advance!
I think the question MAY (that's MAY) not be worded properly. Two scenarios.
1. IF the question is stated properly, then the molarity of the KHP solution created by added 35 mL water instead of 25 mL water is decreased. As Mia notes, M = mols/L and if L is larger than M is smaller. BUT, I don't think that's the question because the question is about the M of NaOH and not M KHP.
2. I think the question REALLY is that of a titration of NaOH vs KHP. If in that titration, one adds 35 mL water to the KHP solid, adds NaOH and titrates the KHP solution formed, then the calculated value for M NaOH is the same no matter what volume of water is added to the KHP before titrated with NaOH. The reason is that the KHP, as weighed, contains mols KHP = grams/molar mass KHP. That will take so many mols NaOH and that determines the M of the NaOH. The volume of water added prior to titration doesn't matter. The indicator in the titration changes when mols KHP = mol NaOH. Water not entering into the reaction is part of a good explanation of what is going on but the crucial answer is that mols KHP = mols NaOH and the amount of water added is that required for the convenience of the operator.
Btw, KHP is Potassium hydrogen phthalate
C8H5KO4
Molarity is another way of saying molar concentration. If you know the formula for molarity you will see that the change in volume will affect the molarity of a solution. The more water you add the more you will dilute the solution.
Yes I know the formula of molarity M=mol/L but the volume of water is not accounted for in this calculation specifically since the volume we're using is the volume of NaOH solution dispensed into the flask. Therefore, water shouldn't have an effect on the molarity of the NaOH.
DrBob222 you're exactly right on 2! Sorry my teacher didn't really clarify exactly what was being asked but I took on the question like how #2 is stated, and therefore said that the molarity of the NaOH wouldn't be affected by the amount of water added prior to the reaction.
Well, my chemistry knowledge may be a bit rusty, but let me try to put a humorous twist on this for you!
Adding more water to your solution of NaOH and KHP is like bringing in a bunch of extra party guests to your chemistry party. The molarity, or concentration, of NaOH is determined by the amount of NaOH present in a given volume of solution. So, if you add more water without adding more NaOH, it's like diluting the size of the party crowd, but not changing the number of clowns.
In simpler terms, adding more water doesn't affect the molarity of NaOH because the amount of NaOH doesn't change. It's like inviting more people to a party but not ordering more pizza – the pizza to partygoer ratio stays the same. So, in this case, don't worry about the extra water. Just make sure you have enough funny clowns (NaOH) to keep the chemistry party going!
Keep up the good work, and remember, chemistry can always use a little humor to lighten the mood!
Your answer is partially correct. Adding more water to dissolve the KHP (acid) does not directly affect the molarity of NaOH. However, when you perform a titration using NaOH and KHP, the volume of water you add to dissolve the KHP can indirectly affect the molarity.
During the titration, you are adding a known volume and concentration of NaOH to neutralize a known mass of KHP. The molarity of NaOH is calculated by dividing the moles of NaOH by the volume of NaOH used in the titration.
Adding more water to dissolve the KHP will result in a larger total volume of solution in the flask. This can affect the volume of NaOH required to reach the endpoint, as it may take more NaOH to completely neutralize the KHP due to dilution.
The molarity of NaOH is calculated using the formula:
Molarity (M) = moles of NaOH / volume of NaOH used (in liters)
If you added more water, the volume of NaOH used may be larger than if you had added less water. This would result in a lower molarity of NaOH because the moles of NaOH would be divided by a larger volume, resulting in a smaller value.
In conclusion, adding more water to dissolve the KHP during a titration can indirectly affect the molarity of NaOH, as it can change the volume of NaOH used in the titration calculation.