1) Calculate the pH for the titration of 60.00 mL of a 0.1500 M methylamine with 45.00 mL of 0.1000 M HCl. Kb = 4.42 × 10−4
2) One liter of a pH 5.00 propionic acid buffer with a total concentration of 60 mM must be prepared. Calculate the mmols propionic acid and sodium propionate needed to prepare the buffer. Ka = 1.34 x 10-5 for propionic acid
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1) Calculate the pH for the titration of 60.00 mL of a 0.1500 M methylamine with 45.00 mL of 0.1000 M HCl. Kb = 4.42 × 1...
QUESTION 10 Calculate the pH during the titration of 30.00 mL of 0.1000 M methylamine, (CH3)NH2(aq), with 0.1000 M HCl(aq) after 12 mL of the acid have been added. Kb of methylamine - 3.6 x 10-4
A 50.00 ml aliquot of 0.1000 M NaOH is titrated with 0.1000 M HCL. Calculate the pH of the solution after the addition of 0.00, 10.00, 25.00, 40.00, 45.00, 49.00, 50.00, 51.00, 55.00, and 60.00 ml of acid and prepare a titration curve from the data.
QUESTION 10 Calculate the pH during the titration of 30.00 mL of 0.1000 M methylamine, (CH3)NH2(aq), with 0.1000 M HCl(aq) after 12 ml of the acid have been added. Kp of methylamine - 3.6 x 10-4 1 points Save Answe
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Calculate the pH during the titration of 20.00 mL of 0.1000 M trimethylamine, (CH3)3N(aq), with 0.1000 M HCl(aq) after 21 mL of the acid have been added. Kb of trimethylamine = 6.5 x 10-5.
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...
In the titration of 50.00 mL of 0.1000 M sodium formate (NaCO2H, whose conjugate acid is HCO2H, and Kb of CO2H- = 1.8 x 10-5) with 0.1000 M HCl at 25.0 C, calculate the pH of the solution when the 25.00 mL of HCl has been added.
Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (Kb = 5.2 × 10−4), with 0.1000 M HCl solution after the following additions of titrant. (a) 15.00 mL: pH = (b) 20.40 mL: pH = (c) 29.00 mL: pH =
Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (Kb = 5.2 × 10−4), with 0.1000 M HCl solution after the following additions of titrant. (a) 15.00 mL: pH = (b) 20.40 mL: pH = (c) 29.00 mL: pH =
Calculate the hypothetical pH AFTER addition of 15.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with 0.1000 M HCl at 25°C. QUESTION 7 10 poir Calculate the hypothetical pH AFTER addition of 40.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with 0.1000 M HCl at 25°C. Calculate the hypothetical pH AFTER addition of 46.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with...