When one student did this experiment, he started with 19.5 mL of 0.118 M monoprotic acid. The endpoint was reached when 17 mL of base was added. What was the concentration of the base?
.002301 moles because .0195 L x .118
.002301/.017 =molarity(concentration)
Answer 0.135mol/L concentration
alison is assuming also a monoprotic base.
To find the concentration of the base, we need to use the concept of stoichiometry and the volume and concentration information provided.
First, let's determine the number of moles of acid used in the experiment:
moles of acid = volume of acid (in liters) × concentration of acid
Given that the volume of acid used is 19.5 mL (or 0.0195 L) and the concentration of acid is 0.118 M, we can calculate the moles of acid:
moles of acid = 0.0195 L × 0.118 M
Next, since the acid and base react in a 1:1 ratio according to the balanced chemical equation, the number of moles of base is also equal to the number of moles of acid.
Now, we can find the concentration of the base by dividing the moles of base by the volume of base used:
concentration of base = moles of base / volume of base (in liters)
Given that the volume of base used is 17 mL (or 0.017 L), we can substitute the values to find the concentration of the base:
concentration of base = moles of acid / 0.017 L
By using the calculated moles of acid and the provided volume of base, we can find the concentration of the base.