Sodium Formate HCOONa

Sodium acetate CH3COONa Sodium succinate (CHaCOONa), Sodium benzoate CeHjCOONa Sodium formate HCOONa i Sodium oxalate fCOONa) J Sodium salicylate HOCeH COONa... 

A solution is prepared by mixing 0.1 mol of formic acid (HCOOH) and 0.1 mol of sodium formate (HCOONa) and diluted to a 1 L. 

To study these reactions use a m solution of sodium formate, HCOONa. 

Describe the effect on pH (increase, decrease, or no change) that results from each of the following additions (a) potassium acetate to an acetic acid solution (b) ammonium nitrate to an ammonia solution (c) sodium formate (HCOONa) to a formic acid (HCOOH) solution (d) potassium chloride to a hydrochloric acid solution (e) barium iodide to a hy-droiodic acid solution. 

Use information from Appendix D to calculate the pH of (a) a solution that is 0.250 M in sodium formate (HCOONa) and 0.100 M in formic acid (HCOOH) (b) a solution that is 0.510 M in pyridine (C5H5N) and 0.450 M in pyridinium chloride (C5H5NHCI) (c) a solution that is made by combining 55 mL of0.050 M hydrofluoric acid with 125 mL of 0.10 M sodium fluoride. 

Calculate the pH of a buffer made by dissolving 1 mol formic acid (HCOOH) and 1 mol sodium formate (HCOONa) in 1 L of solution (see Table 9.9). 

Consider I L of a buffer that is 0.85 M in formic acid (HCOOH) and 1.4 M in sodium formate (HCOONa). Calculate the pH after the addition of 0.15 mol HCl. (Assume the addition causes no volume change.)... 

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