3. How much 0.10 M Base (in mL) is required to neutralize 8.00 mL of the 0.10 M acid?
Base Acid Base Volume (mL)
NaOH HCl ____________
NaOH HC2H3O2 _____________
4. How would the volume of base change from problem three if the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water (like it will be in the experiment you perform in lab)?
A. The volume would decrease.
B. No change.
C. The volume would increase.
D. Not enough information is given to predict what would happen.
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I need help with a chemistry problem. Here it is A quantity of gas has a volume of 14L at STP. What is the volume (in L) at 9.7 atm and 94 C? Can you help me set up the equation?
The base/acid problem was answered above.
PV = nRT. Don't forget to use temperature in Kelvin, which is Kelvin = 273 + C.
In the future, note that you probably can get help a little faster if you go to the top of the page, click on Ask a New Question, and post your own question instead of piggy-backing on another post.
actually nobody even bothered to answer it...i just see the same person giving an explanation that might not exactly be comprehended by others...
To answer question 3, we need to use the concept of stoichiometry. The balanced chemical equation for the neutralization reaction between a base and an acid is:
Base + Acid -> Salt + Water
First, we need to determine the stoichiometry of the reaction. From the balanced chemical equation, it can be observed that the ratio of base to acid is 1:1. This means that for every 1 mole of base, we require 1 mole of acid.
Next, we can use the concentration and volume of the acid to calculate the moles of acid present. The concentration of the acid is given as 0.10 M, which means there are 0.10 moles of acid present in 1 liter (or 1000 mL) of solution. Therefore, in 8.00 mL of the acid, there would be:
Moles of Acid = (0.10 M) x (8.00 mL / 1000 mL)
To neutralize the acid, we need an equal number of moles of base. Since the base and acid have a 1:1 stoichiometry, the moles of base required would be the same as the moles of acid:
Moles of Base = Moles of Acid
Now, we can calculate the volume of the base required using the concentration of the base. The concentration of the base is also given as 0.10 M, so we can use the following equation to determine the volume:
Volume of Base = (Moles of Base) / (Concentration of Base)
Plug in the value of the moles of base (which is equal to the moles of acid) and the concentration of the base (0.10 M) to calculate the volume of base required to neutralize the acid.
To answer question 4, if the 8.00 mL of 0.10 M acid is diluted with 100 mL of water, the total volume of the acid solution will increase. However, the amount of acid present in the solution remains the same, as it is just being distributed in a larger volume. Therefore, the volume of base required to neutralize the acid will remain the same. So the answer would be B. No change.