The acid dissociation constant is defined as Ka = [H+][A-]/[HA] where [H+], [A-] and [HA] are the concentrations of protons, conjugate base, and acid in solution respectively. Assuming this is a weak acid as the pH is quite high for a 1.35 M solution, we can assume that the change in [HA] is negligible and therefore [HA] = 1.35 M.
To calculate [H+] we can use the relationship pH = -log[H+], rearranging to give: [H+] = 10^(-pH) = 10^(-2.93) = 1.17 x 10^(-3).
Since the acid is relatively concentrated we can assume therefore that [H+] = [A-] as for each proton dissociated, a conjugate base is formed.
Therefore, we can calculate Ka as:
Ka = [H+]^2/[HA] = (1.17 x 10^-3 M)^2/1.35 = 1.01 x 10^-6 M
Answer:
Formula of the compound = 
Explanation:
Given,
No. of mole of O = 8.20 mol
No. of mole of P = 3.30 mol
Chemical formula = 
Ratio of P and O = 
formula of the compound =
the Percentage yield for the reaction = 48.8%
What is Percentage yield ?
The % ratio of the theoretical yield to the actual yield is known as the percent yield. It is calculated as the theoretical yield multiplied by 100% divided by the experimental yield. The percent yield is 100% if the theoretical and actual yields are equal. Because the real yield is frequently lower than the theoretical value, percent yield is typically lower than 100%. This may be due to incomplete or conflicting reactions or sample loss during recovery. If the percent yield is more than 100%, more sample than expected was retrieved from the reaction.
4 P + 3 O2 = P4O6
moles P = 75.3 g / 30.9738 g/mol= 2.43
moles O2 required = 2.43 x 3 / 4=1.82
actual moles O2 = 38.7 g /32 g/mol=1.21 so O2 is the limiting reactant
theoretical moles P4O6 = 1.21 / 3=0.403
theoretical mass P4O6 = 0.403 mol x 219.895 g/mol=88.6 g
% yield = 43.3 x 100/ 88.6 = 48.8 %
the Percentage yield for the reaction = 48.8%
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