Question

Calculate the pH of a solution made by adding 42 g of sodium acetate, NaCH3COO, to 22 g of acetic acid, CH3COOH, and dissolving in water to make 300. mL of solution. Hint given in feedback. The K, for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. Answer: Calculate the pH of a solution made by adding 59 g of sodium acetate, NaCH3COO, to 22 g of acetic acid, CH3COOH, and dissolving in water to make 500 mL of solution. Answer: Calculate the pH of a solution made by adding 35.0 g of sodium formate, NaHCOO, to 100 mL of 0.21 M formic acid, HCOOH. Hint what kind of solution is made? The Ka for HCOOH is 1.8 x 10-4 M. As usual, report pH to 2 decimal places. Answer:

Answer 1

kindly post different questions separately. please rate

meu al NO CH3 000 - 429 molar mans of NaCH3COO = 82103 g/mol moles of NH3COO = man 42 g - 0.512 mol molar mas 82.03 g/mol mans of CH3COOH = 229 molar man of CH3COOH = 60.05 g/mol. moles of CH3COOH = mas – 229 molarmas 60105 g/mol volume of solution 300 ml = 0.3L (1000 mL = 1L) = 0,3664 mol concentration (N) = moles Volume (L) [NA CH3 100 ] = 6.512 mol = 0.3L - 1.707M [CH3 CUCH] = 0.3664 mol = 03L 1.221 m ka of acetic acide 1.8 *10-5 pka = -log ko = -log (1.8810-5) = 41.744 Using Henderson Hanal batch equation pH = pka + log [NOCH3 cool (CH3 C00H] - 4.744 + log (1907) 1221M bH = 4.89 answer