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

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

Hh.39.

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

so Please don't provide handwritten solution,

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 of the following combination of solutions will form a buffer solution?            (A)  50.0 mL of 0.20 M NH3 + 50.0 mL of 0.10 M HCl;          (B)  50.0 mL of 0.20 M NH3 + 50.0 mL of 0.10 M NaOH;          (C)  50.0 mL of 0.20 M HCl + 50.0 mL of 0.10 M NH3;          (D)  50.0 mL of 0.20 M NaOH + 50.0 mL of 0.10 M HCl.

(7) Calculate the pH of each of the following solutions: (a) 0.1000M Propanoic acid( HC H O,,K=1.3x105) (b) 0.1000M sodium propanoate (Na C HỎ) (c) 0.1000M HC₂H₂O, and 0.1000M Nа С¸¸0₂ 3 5 52 (d) After 0.020 mol of HCl is added to 1.00 L solution of (a) and (b) above. (e) After 0.020 mol of NaOH is added to 1.00 L solution of (a) and (b) above.

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)

Calculate pH for a weak base/strong acid titration. Determine the pH during the titration of 38.5 mL of 0.236 M ammonia (NH3, K₂ = 1.8x10-5) by 0.236 M HBr at the following points. (a) Before the addition of any HBr 4.9 (b) After the addition of 16.4 mL of HBr (c) At the titration midpoint (d) At the equivalence point (e) After adding 58.9 mL of HBr