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 pHof (a) a solution that is 0.060 M in potassium propionate(C2H5COOK or KC3H5O2) and 0.085 M in propionic acid(C2H5COOH or HC3H5O2); (b) a solution that is 0.075 M in trimethylamine, (CH3)3N, and 0.10 M in trimethylammoniumchloride, (CH3)3NHCl; (c) a solution that is made bymixing 50.0 mL of 0.15 M acetic acid and 50.0 mL of 0.20 Msodium acetate.

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Does the pH increase or decrease, and does it do so to a largeor small extent, with each of the following additions?(a) 5 drops of 0.1 M NaOH to 100 mL of 0.5 M acetate buffer(b) 5 drops of 0.1 M HCl to 100 mL of 0.5 M acetate buffer(c) 5 drops of 0.1 MNaOH to 100 mL of 0.5 MHCl(d) 5 drops of 0.1 MNaOH to distilled water

Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.145 M 4-chlorobenzoic acid (Ka = 1.0 ✕ 10−4) with 0.145 M KOH. (Assume Kw = 1.01 ✕ 10−14.) (a no KOH added????   (b)20. mL of KOH solution added????   (c)39 mL of KOH solution added????   (d)40. mL of KOH solution added????   (e)41 mL of KOH solution added????

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.

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)

PR: (a) Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 800. mL of solution. (10). (b) Calculate the pH after 0.050 moles of NaOH are added to the buffer solution (assume no volume change) (10). Ka (HCNO) = 2.0 × 10-4