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28) a) What is the pH of a 0.159 M aqueous solution of ammonium iodide, NHAI pH- This Solution is...
What is the pH of the solution obtained by mixing 30.00 mL of 0.250 M HCl and 30.00 mL of 0.125 M NaOH? We assume additive volumes. What is the pH of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid? (ka for acetic acid is 1.3x10-5.) Calculate the pH of a solution prepared by mixing 15.00 ml of 0.10 M NaOH and 30.00 mL of 0.10 M benzoic acid solution. (Benzoic acid is monoprotic; its...
The substance phenol (CH3OH) is a weak acid (K = 1.0x10-19). What is the pH of a 0.159 M aqueous solution of sodium phenoxide, NaC,H,? This solution acidic basic neutral
a) What is the pH of a solution that consist of 0.20 M ammonia, NH3, and 0.20 M ammonium choride, NH4Cl? (Kb for ammonia is 1.8 x 10-5) b) 1.25 g of benzoic acid (C6H5CO2H) and 1.25 g of sodium benzoate (NaC6H5CO2) are dissolved in enough water to make 250 mL solution. Calculate the pH of the solution using the Handerson-Hasselbach equation (Ka for benzoic acid is 6.3 x 10-5). c) What is the pH after adding 82 mg of...
Please Help! A)BThank you! The pH of an aqueous solution of 0.249 M ammonium iodide, NH4I (aq), is This solution is B The pH of an aqueous solution of 0.579 M triethanolamine (a weak base with the formula CsHisO3N) is
Calculate the pH of a 0.159 M aqueous solution of hydroxylamine (NH20H, Kt 9.1x109) and the equilibrium concentrations of the weak base and its conjugate acid. pH [NH2OHequilibrium М [NH3OHlequilibrium М
What is the amount of ammonium chloride that has to be dissolved in 190 mL of 0.189 M NH3(Kb= 1.8×10‒5) to make it a buffer with a pH of 8.96, in grams? A mixture contains 0.250 M benzoic acid, a monoprotic acid (Ka = 6.28 × 10‒5), and 0.400 M sodium benzoate. How many mL of a HCl solution whose pH is 0.523 should be added to 500 mL of this buffer to change its pH from what it is...
The pH of an aqueous solution of 0.203 M sodium acetate, NaCH3COO(aq) is what?
Calculate the pH of a 0.020 M benzoic acid solution, K = 6.3x10^-5 Calculate the pH of a 0.015 M solution of sodium acetate, where the K of acetic acid is 1.8x10^-5
Calculate the pH of a buffer solution that results from combining 37.5 mL of a 0.450 M in benzoic acid (HC7H5O2) and 82.5 mL of a 0.250 M in sodium benzoate (NaC7H5O2). For benzoic acid, Ka = 6.5 × 10–5 .
1. Calculate pH of CH3COOH. The concentration of this species is O.33 M. Ka = 1.8x10^-5 (six decimal places) 2. Calculate pH of NH4OH. The concentration kf this species is 0.49 M. Ka= 1.8x10^-5 (six decimal places) 3. How do I figure out is an aqueous solution of a salt is acidic, basic, or neutral? Can you explain it by using this as an example; Sodium acetate, NaCH3COO?