How many grams of HCOOH are needed to make 2.0 liters of aqueous solution of pH=3.8?Be...
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 C6H5COOH are needed to make 3.9 liters of aqueous solution of pH 3.4?Be sure to back correct from equilibrium molecular acid molarity to starting molecular acid molarity How many grams of C6H5COOH are needed to make 3.9 liters of aqueous solution of pH 3.4?Be sure to back correct from equilibrium molecular acid molarity to starting molecular acid molarity
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.
+-/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 0.0167 M aqueous solution of formic acid (HCOOH, K, = 1.8x10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH [HCOOH)equilibrium [HCOO equilibrium
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?
Problem 3 (8 points). The pH of an aqueous solution of formic acid (HCOOH) is 2.771. What is the initial molar concentration of HCOOH, if its acid ionization constant is K = 1.78*10*? Enter your answer in the box provided with correct units and sig. figs.: Answer: The initial molar concentration of : [HCOOH) = formic acid is
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).
Five cubic feet of an aqueous hydrochloric acid (HCl) having a molarity of 2.0 is to be prepared. Assuming the SG of the solutions is 1.02, determine: (a) How many gram of pure HCl is needed? (b) How many liters of pure water is needed? (c) What is the mole fraction of HCl in the solution? (d) What is the mass fraction of HCl in the solution?