For the diprotic weak acid H,A, Kal = 2.4 x 10-6 and K2 = 6.9 × 10-9. What is the pH of a 0.0500 M solution of H, A? pH What are the equilibrium concentrations of H,A and A²- in this solution? [H,A] = M [A?-] = M

For the diprotic weak acid H2A, Ka1 = 3.0 x 10-6 and K2 = 5.6 x 10-9. %3! What is the pH of a 0.0550 M solution of H, A? pH = What are the equilibrium concentrations of H, A and A?- in this solution? (H,A) = [A?-) =

NH3(aq) + H₂O(1) ⇒ NH‡ (aq) + OH- (aq) The equilibrium hydroxide concentration in a 0.0220 M NH3 solution at 25 °C is given below. [OH-] = 6.29 x 10-4 M What is the percent ionization of the NH3 at equilibrium? lonization = [?] % % lonization Enter

Calculate the pH of a sulfuric acid (H2SO4, Ka HSO4 = 1.2 x 10-2) solution that has a concentration of A) 5.00 M and B) 0.075 M

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Question 8 of 20 Sub Complete the balanced molecular reaction for the following weak base with a strong acid: NaCIO2(aq) + H2SO«(aq) – 3- 2. 2+ 3+ 4+ 04- 1 6 7 8. 9. 01 D 07 9. 2 3 4. 6. (s) (1) (g) (aq) -> Na H2O H3O* OHT H. CI • x H2O Delete Reset W ? Questions prep ok étv A 山 T。 OCT 4. MacBook Pro 8. 11

Which of the following 1.0 M solutions would have the highest pH? Weak Acid Ka Weak Base Kb HCN 4.9 x 10-10 HONH, 1.1 x 10-8 HNO2 4.5 x 104 NH3 1.8 x 10-5 HIO 2.3 x 10-11 CHINH, 4.3 x 10-10 HBrO 2.5 x 10-9 H¸NNH₂ 1.3 x 10-6 CHCOOH 6.3 x 105 CH N 1.7 x 10-9 A KCN B C CH NHCI Nalo + D NH Br

For the diprotic weak acid H2A, Kal = 3.0 × 10-6 and Ka2 = 7.1 x 10-9. What is the pH of a 0.0700 M solution of H, A? pH = What are the equilibrium concentrations of H, A and A?- in this solution? [H,A] = M [A?-] = M

Kc for formic acid dissociation in water is 1.8x10-4. What are the equilibrium concentrations  of H30+ HCOO- and HCOOH if the initial concentration of HCOOH is .15 mol?  HCOOH (aq) +H20 (L) >< H30 (aq) + HCOO (aq)

please help with these two