(a) Develop a logarithmic concentration versus pH diagram for propionic acid (CH3CH2COOH, Ka 1.34*10-5). Assume a...
Consider the titration of 15.00 mL of 0.1800 M propionic acid (CH3CH2COOH), with 0.1555 M NaOH. Ka for propionic acid is 1.34 X 10-5 a. What volume of base is required to reach the equivalence point? b. When the equivalence point is reached, sodium propionate ionizes in water. Write the equation for the reaction. C. What is the pH at the equivalence point? (20 points) Consider the titration of 15.00 mL of 0.1800 M propionic acid (CH3CH2COOH), with 0.1555 M...
Propionic acid, C2H5CO2H (Ka = 1.34 × × 10^−5), is used in the manufacture of calcium propionate, a food preservative. What is the pH of a 0.698-M solution of C2H5CO2H?
1. 50.00 mL of 0.1000 M propanoic acid (CH3CH2COOH – Ka = 1.34 X 10-5) is titrated with 0.2000 M KOH. Calculate the pH at the following points in the titration: 1) Initial pH – no KOH has been added. 2) 5.00 mL of KOH has been added. 3) 12.50 mL of KOH has been added. 4) At the equivalence point. (Calculate the volume of KOH to reach the equivalence point & identify a good indicator.) 5) Provide a sketch...
The Ka of propanoic acid (C2H5COOH) is 1.34 × 10-5. Calculate the pH of the solution and the concentrations of C2H5COOH and C2H5COO– in a 0.421 M propanoic acid solution at equilibrium.
The Ka of propanoic acid (C2H5COOH) is 1.34 × 10-5. Calculate the pH of the solution AND the concentrations of C2H5COOH AND C2H5COO– in a 0.323 M propanoic acid solution at equilibrium. Please explain each step in detail.
1. Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice with a pH of 2.0. Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 2. What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52? Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 3. Which is the stronger acid, NH4+ or HBrO? Hint: Compare...
HA is a weak acid. Its ionization constant, Ka, is 2.4 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.046 M.
HA is a weak acid. Its ionization constant, Ka, is 4.7 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.062 M.
HA is a weak acid. Its ionization constant, Ka, is 4.7 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.062 M.
HA is a weak acid. Its ionization constant, Ka, is 4.7 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.062 M.