Write down the correct alpha equation needed to determine the fraction of the total generic diprotic acid H2A in a solution that is in A2- form.
Write down the correct alpha equation needed to determine the fraction of the total generic diprotic acid H2A in a solution that is in A2- form.
For the diprotic weak acid H2A, ?a1=2.0×10−6 and ?a2=8.8×10−9. What is the pH of a 0.0650 M solution of H2A? pH= What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]= M[A2−]=
For the diprotic weak acid H2A, ?a1=3.0×10−6 and ?a2=7.3×10−9 . What is the pH of a 0.0500 M solution of H2A ? pH= What are the equilibrium concentrations of H2AH2A and A2−A2− in this solution? [H2A]= [A2−]=
For the diprotic weak acid H2A, Ka1=4.0×10−6 and ?a2=5.9×10−9 What is the pH of a 0.05500.0550 M solution of H2A? pH= What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]= [A2−]=
For the diprotic weak acid H2A, ?a1=3.5×10−6 and ?a2=7.8×10−9 What is the pH of a 0.07000 M solution of H2A? pH= What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]= [A2−]=
For the diprotic weak acid H2A, ?a1=2.9×10−6 and ?a2=8.4×10−9 What is the pH of a 0.07000.0700 M solution of H2A? What are the equilibrium concentrations of H2A and A2− in this solution?
A diprotic acid, H2A,H2A, has acid dissociation constants of ?a1=4.15×10−4Ka1=4.15×10−4 and ?a2=3.73×10−12.Ka2=3.73×10−12. Calculate the pH and molar concentrations of H2A,H2A, HA−,HA−, and A2−A2− at equilibrium for each of the solutions. A 0.176 M0.176 M solution of H2A.H2A. pH = [H2A]=[H2A]= MM [HA−]=[HA−]= MM [A2−]=[A2−]= MM A 0.176 M0.176 M solution of NaHA.NaHA. pH= [H2A]=[H2A]= MM [HA−]=[HA−]= MM [A2−]=[A2−]= MM A 0.176 M0.176 M solution of Na2A.Na2A. pH= [H2A]=[H2A]= MM [HA−]=[HA−]= MM [A2−]=[A2−]= M
is this correct ? 5.(5 points) A 0.10-mal sample of a diprotic acid, H2A, is dissolved in 250 mL of water. Kaq for this acid is 1.0 10-5 and Kaz is 1.0 10-10. Calculate the concentration of A2- in this solution 1.0 x 10-12 M 1.0 x 10-10M 1.0 x 10-7M 1.0 x 10-3M
A diprotic acid, H2A has acid dissociation values, with pKa1-1.85 and pKa2-7.17. What is the Kb1 of its base form, A2? Note: -Report final answer only without subscript and unit. - Round your final answer to correct sig fig.
Given a diprotic acid, H2A , with two ionization constants of ?a1=2.0×10−4 and ?a2=3.1×10−12 , calculate the pH for a 0.120 M solution of NaHA.
A diprotic acid, H2A, has kan = 6.7x10-8 and Ka2 = 3.1x10-20. Determine the concentration of HA and A2-ions in a 0.20 M H2A solution. HA concentration is 0.20 M and A2- concentration is 6.7x10-8 M ОА. HA concentration is 1.2x10-4 M and A2- concentration is 6.7x10-8 M ОВ. HA concentration is 2.6x10-4 M and A2- concentration is 3.1x10-20 M Ос. OD. HA concentration is 1.2x10-4 M and A2- concentration is 3.1*10-20 M HA-concentration is 2.6x10-4 M and A2-concentration is...