Answer:
72.2 ml
Explanation:
The neutralization equation between HBr (acid) and NaOH (base) is the following:
HBr(aq) + NaOH(aq) → NaBr(aq) + H₂O(l)
We can see that 1 mol of HBr reacts with 1 mol of NaOH. At the equivalence point, the total number of moles of HBr reacts with the total number of moles of NaOH. The number of moles can be calculated as the product between the molarity (M, in mol/L) and the volume (V). So, we can equal the quantities of acid and base, as follows:
moles HBr = moles NaOH
M(HBr) x V(HBr) = M(NaOH) x V(NaOH)
Now, we calculate the volume of NaOH with the data:
V(NaOH)= M(HBr) x V(HBr)/M(NaOH)
= (2.60 mol/L x 50.0 ml)/(1.80 mol/L)
=72.2 ml
1cm = 0.01m
1cm x 172 = 0.01 x 172
172cm = 1.72m
Answer:
Benzoic acid is the stronger acid
Explanation:
Weak acids do not dissociate completely in the solution. They exists in equilibrium with their respective ions in the solution.
The extent of dissociation of the acid furnising hydrogen ions can be determined by using dissociation constant of acid ().
Thus for a weak acid, HA
The is:
The more the , the more the acid dissociates, the more the stronger is the acid.
Also,
is defined as the negative logarithm of .
So, more the , less is the and vice versa
All can be summed up as:
The less the value of , the more the is and the more the acid dissociates and the more the stronger is the acid.
Given,
of acetic acid = 54.7
of benzoic acid = 54.2
of benzoic acid < of acetic acid
So, benzoic acid is the stronger acid.
"Increasing the temperature" is the one factor among the factors given in the question that <span>increases the rate of dissolution in an unsaturated solution. The correct option among all the options that are given in the question is the first option or option "A". I hope the answer has come to your help.</span>