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

so Please don't provide handwritten solution,

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

A buffer is prepared by adding 4.8 g of (NH4)2SO4 to 425 mL of 0.258 M NH3. Assuming that the volume stays constant, what is pH of the buffer solution? Consider: Kb (NH3) = 1.8×10–5, and Molar Mass of (NH4)2SO4 = 132.14 g/mol. (A) 10.04 (B) 5.22 (C) 9.44 (D) 4.93 (E) 1.75

For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than 7. (a) Equal volumes of 0.10 M acetic acid, CH3CO2H, and 0.10 M KOH are mixed. (b) 25 mL of 0.015 M NH3 is mixed with 25 mL of 0.015 M HCl. (c) 150 mL of 0.20 M HNO3 is mixed with 75 mL of 0.40 M NaOH.

Be sure to answer all parts. Tris [tris(hydroxymethyl)aminomethane] is a common buffer for studying biological systems. (K = 5.01 × 10 and pK = 8.3) (a) Calculate the pH of the Tris buffer after mixing 11.0 mL of 0.20 M HCl solution with 25.0 mL of 0.10 M Tris. (b) This buffer was used to study an enzyme-catalyzed reaction. As a result of the reaction, 0.00019 mol of H* was produced. What is the pH of the buffer at the end of the reaction? (c) What would be the final pH if no buffer were present?

t ent Determine the pH during the titration of 64.4 mL of 0.443 M acetic acid (K₂ = 1.8x10-5) by 0.443 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 96.6 mL of KOH

TUTOR Analysis of a Weak Acid-Strong Base Titration Curve Determine the pH during the titration of 63.3 mL of 0.465 M formic acid (K₂ = 1.8×10) by 0.465 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 95.0 mL of KOH