grams of C6H5COOH = 1.4
Explanation
pH = 3.4
[H+] = 10-pH
[H+] = 10-3.4
[H+] = 4.0 x 10-4 M
initial concentration of benzoic acid = ([H+]2 / Ka) + [H+]
initial concentration of benzoic acid = [(4.0 x 10-4 M)2 / (6.3 x 10-5)] + (4.0 x 10-4 M)
initial concentration of benzoic acid = 2.91 x 10-3 M
moles benzoic acid = (initial concentration of benzoic acid) * (volume of solution in Liter)
moles benzoic acid = (2.91 x 10-3 M) * (3.9 L)
moles benzoic acid = 0.0114 mol
mass benzoic acid = (moles benzoic acid) * (molar mass benzoic acid)
mass benzoic acid = (0.0114 mol) * (122.12 g/mol)
mass benzoic acid = 1.4 g
How many grams of C6H5COOH are needed to make 3.9 liters of aqueous solution of pH 3.4?Be sure to...
How many grams of C6H5COOH are needed to make 2.5 liters of aqueous solution of pH=4.0? Be sure to back correct from equilibrium molecular acid molarity to starting molecular acid molarity.
How many grams of CH3COOH are needed to make 2.0 liters of aqueous solution of pH=3.1?Be sure to back correct from equilibrium molecular acid molarity to starting molecular acid molarity.
How many grams of HCOOH are needed to make 2.0 liters of aqueous solution of pH=3.8?Be sure to back correct from equilibrium molecular acid molarity to starting molecular acid molarity.
+-/4 points My Not How many grams of CHCOOM are needed to make 3.1 liters of aqueous solution of pH-3.5730 sure to back correct from equorum molecular acid molarity to starting molecular acid molarity Submit Answer Practice Another Version
Calculate the pH of a 0.496 M aqueous solution of benzoic acid (C6H5COOH, Ka = 6.3×10-5) and the equilibrium concentrations of the weak acid and its conjugate base. pH = _____ [C6H5COOH ]equilibrium = _____M [C6H5COO- ]equilibrium = _____M
How many grams of HCl are needed to make 250. mL of a strong acid solution having a pH equal to 1.00
2) How many grams of sodium hypochlorite (NaClo) are needed to make 250 mL of 0.700 M NaClO solution? 3) How many grams of KCO, would be needed to make 4.55 mL of a 15.00 (m/v) solution? 4) A 34.0 % (m/m) sulfuric acid (H2SO4) solution has a density of 1.25 g/mL. What is the molarity of this solution?
1. How many liters of 3.4 M HI will be required to reach the equivalence point with 2.1 L of 2.0 M KOH? 2. How many liters of 1.75 M HCl will be required to reach the equivalence point with 1.25 L of 2.5 M KOH 3. Titration reveals that 11.6 mL of 3.0 M sulfuric acid is required to neutralize the sodium hydroxide in 25.00 mL of NaOH solution. What is the molarity of the NaOH solution? 4. Titration...
1. You need to prepare 10.0 liters of an acid aqueous solution with a pH of 1.25. Calculate the mass of sulfuric acid that you need (in grams).
43. An aqueous solution of methylamine (CH3NH2) has a pH of 10.65. How many grams of methylamine are there in 100.0 mL of the solution? Calculate the pH and percent ionization of a 0.990 M HNO2 solution. pH = %