For the diprotic weak acid H2A, Kal = 3.5 × 10-6 and K22 = 7.7 × 10-9. What is the pH of a 0.0400 M solution of H,A? pH = What are the equilibrium concentrations of H, A and A²- in this solution? [H,A] = M [A?-] = M

Water dissociates to a greater extent at 37 degrees celsius than 25 degrees celsius. Which of the following is true? H2O(l) <-----> H^+ (aq) +OH^-(aq)      Kw = 2.24x10^-14 A. The pH of a neutral solution is higher than 7 at 37 degrees celsius B. The pKw for water is larger at 37 degrees celsius than at 25 degrees celsius C. The pOH of a .01 M KOH solution is lower at 37 degrees celsius than at 25 degrees celsius D. The pH of a .01 M HNO3 solution is higher at 37 degrees than t 25 degrees E. At 37 degrees celsius, pH + pOH < 14 WHta is the correct answer and why?

If the K of a weak base is 2.5 × 10-6, what is the pH of a 0.23 M solution of this base? pH =

Payal

Calculate the OH concentration and pH of a 7.7 x 10-³ M aqueous solution of sodium cyanide, NaCN. Finally, calculate the CN concentration. ( K₂ (HCN) = 4.9 × 10-¹⁰) [OH-] M pH = [CN] = 3

A solution of vinegar corresponds to about 0.400 M. At this concentration, with Ka = 1.8 x10-5 , what is the pH of vinegar? Vinegar formula (CH₃COOH) Show the ICE table and your calculation to get to the pH value.

Calculate the pH of a 3.5 M solution and the equilibrium concentrations of the species H3PO4, H2PO4- , HPO4-2, and PO4-3          (Ka1= 7.5 x 10-3, Ka2= 6.2 x 10-8, Ka3= 4.8 x 10-13)

What is the pH of a 80.0 mL solution which is 0.23 M in IO and 0.49 M in HIO? The K₂ for HIO is 2.3 × 10-11. a pH =

A diprotic acid (H, A) has Ka1 = 4.27 x 10-7 and Ka2 = 5.98 × 10-11. What is the pH of a 0.437 M H, A solution? pH =

Antony determines the pH of a solution to be 5.9. What is the concen- tration of hydronium ions in this solution? Use (H*] = 10-PH A 7.7x10-5 M B 1.9x 10-6 M 5.9x 10-8 M D 2.6 x 10-7 M