Answer:
0.084 M
Explanation:
Using the Henderson-Hasselbalch equation for a buffer ( a buffer is solution contain a weak acid and it conjugate base; the solution resist change in pH)
pH = pKa + log ( base/acid)
4.9 - 4.76 =log ( base / acid)
10^0.14 = ( base / acid)
1.38 = (base / acid)
since there is 0.2 M in the buffer solution
the concentration of acid = × 0.2 = 0.084 M
Answer:
M = 16.8 M
Explanation:
<u>Data:</u> HNO3
moles = 12.6 moles
solution volume = 0.75 L
Molarity is represented by the letter M and is defined as the amount of solute expressed in moles per liter of solution.
The data is replaced in the given equation:
The question is incomplete, here is the complete question:
Calculate the initial rate for the formation of C at 25°C, if [A]=0.50 M and [B]=0.075 M. Express your answer to two significant figures and include the appropriate units.Consider the reaction
A + 2B ⇔ C
whose rate at 25°C was measured using three different sets of initial concentrations as listed in the following table:
The table is attached below as an image.
<u>Answer:</u> The initial rate for the formation of C at 25°C is
<u>Explanation:</u>
Rate law is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.
For the given chemical equation:
Rate law expression for the reaction:
where,
a = order with respect to A
b = order with respect to B
....(1)
....(2)
....(3)
Dividing 2 by 1, we get:
Dividing 3 by 1, we get:
Thus, the rate law becomes:
......(4)
Now, calculating the value of 'k' by using any expression.
Putting values in equation 1, we get:
Calculating the initial rate of formation of C by using equation 4, we get:
[A] = 0.50 M
[B] = 0.075 M
Putting values in equation 4, we get:
Hence, the initial rate for the formation of C at 25°C is
