7. Write the charge balance for the following solutions and list the equations that would have to be solved to determine the equilibrium solution composition. (a) 103 M benzoic acid (b) 10-3 M Na₂S (c) 103 M (NH4)2CO3 (d) 10-3M (NH4)2CO3 plus 5 × 10-3 M (NH4)3PO4 plus 10-3 M CaCO3

Determine the pH during the titration of 57.0 mL of 0.347 M nitrous acid (K₂ = 4.5x10-4) by 0.347 M NaOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any NaOH (b) After the addition of 14.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 85.5 mL of NaOH

Calculate the pH after 0.020 mol NaOH is added to 1.00 L of each of the solutions below, (a) 0.123 M HONH2 (Kp 1.1 x 10 8) %3! (b) 0.123 M HONH3CI (c) pure H20 7 (d) a mixture containing 0.123 M HONH2 and 0.123 M HONH3CI

Write the charge balance and material balance(s) that are needed to determine the equilibrium solution composition for each of the following aqueous solutions:   (a) 10-3 M benzoic acid   (b) 10-3 M Na2S   (c) 10-3 M (NH4)2CO3   (d) 10-3 M (NH4)2CO3 plus 5 × 10-3 M (NH4)3PO4 plus 10-3 M CaCO3

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How many moles of HCOONA must be added to 1.0 L of 0.10 M HCOOH to prepare a buffer solution with a pH of 3.4? (HCOOH K = 2 × 10 ) (A) 0.01 (B) 0.05 (C) 0.1 (D) 0.2 What is the percent ionization of a 0.10 M solution of formic acid at 25°C? Formic acid, HCOOH, has a Ka value of 1.9 x 104 at 25°C. (A) 0.19% (B) 1.4% (C) 4.4% (D) 14%

Which is the best solution to buffer at pH = 10.50?           (A) A buffer solution containing 0.25 M H2CO3 and 0.45 M Na2CO3; (Ka (H2CO3) = 4.3 x 10–7)          (B) A buffer solution containing 0.25 M NaHCO3 and 0.45 M Na2CO3; (Ka (HCO3–) = 5.6 x 10–11)          (C) A buffer solution containing 0.12 M NaHCO3 and 0.22 M Na2CO3; (Ka (HCO3–) = 5.6 x 10–11)          (D) A buffer solution containing 0.12 M NH4Cl and 2.2 M NH3; (Ka (NH4+) = 5.6 x 10–10)

Determine the pH during the titration of 69.1 mL of 0.366 M benzoic acid (Ka = 6.3×10-5) by 0.366 M NaOH at the following points. (Assume the titration is done at 25 °C.)(a) Before the addition of any NaOH (b) After the addition of 16.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint)  (d) At the equivalence point  (e) After the addition of 104 mL of NaOH

Determine the pH during the titration of 26.8 mL of 0.447 M hypochlorous acid (K, = 3.5x103) by 0.467 M NAOH at the following points. (a) Before the addition of any NaOH 3.90 (b) After the addition of 6.20 mL of NaOH 6.95 (c) At the half-equivalence point (the titration midpoint) 6.90| (d) At the equivalence point (e) After the addition of 38.5 mL of NaOH