Using spectrophotometry, you determine αHA- to be 0.90 for a solution containing a diprotic weak acid, H2A, that has pK’s of 2.50 and 6.00. What is the pH of this solution?
Using spectrophotometry, you determine αHA- to be 0.90 for a solution containing a diprotic weak acid,...
For the diprotic weak acid H2A, ?a1=2.1×10−6 and ?a2=5.9×10−9.What is the pH of a 0.0800M solution of H2A?pH = ____________What are the equilibrium concentrations of H2A and A2− in this solution?[H2A]=M[A2−]=MNo referals please without an attempt for an answer.
For the diprotic weak acid H2A, Ka-3.6x10 and Ka2 8.6 x10 What is the pH of a 0.0700 M solution of H2A? What are the equilibrium concentrations of H2A and A in this solution? Number pH- Number H,A Number
For the diprotic weak acid H2A, Ka1 = 2.7 × 10-5 and Ka2 = 5.2 × 10-7. What is the pH of a 0.0550 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?
For the diprotic weak acid H2A, Ka1 = 3.1 × 10-5 and Ka2 = 8.2 × 10-7. What is the pH of a 0.0650 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?
For the diprotic weak acid H2A, Ka1 = 4.0 × 10-6 and Ka2 = 6.1 × 10-9. What is the pH of a 0.0800 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?
For the diprotic weak acid H2A, Ka1 = 3.8 × 10-6 and Ka2 = 5.8 × 10-9. What is the pH of a 0.0700 M solution of H2A? What are the equilibrium concentrations of H2A and A2- in this solution?
For the diprotic weak acid H2A, Ka1 = 3.8 × 10-6 and Ka2 = 6.9 × 10-9. What is the pH of a 0.0800 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?
For the diprotic weak acid H2A, Ka1 = 2.8 × 10-6 and Ka2 = 8.2 × 10-9. What is the pH of a 0.0500 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?
For the diprotic weak acid H2A, Ka1 = 3.5 × 10-6 and Ka2 = 6.2 × 10-9. What is the pH of a 0.0800 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?
For the diprotic weak acid H2A, Ka1 = 3.6 × 10-6 and Ka2 = 6.7 × 10-9. What is the pH of a 0.0500 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?