Calculate the pH of a mixture containing 0.100M HONH3 and 0.100M HONH3Cl
Calculate the pH of a mixture containing 0.100M HONH3 and 0.100M HONH3Cl
Calculate the pH of an acid mixture that contains 0.200M HCl and 0.100M HCHO2. Formic acid has an acid ionization constant of Ka=1.8x10-4 and HCl is a strong acid. (5 points)
Calculate the pH during titration of 75.0mL of 0.100M benzoic acid by 0.100M NaOH before the addition of NaOH and after 20mL NaOH are added. Ka=6.3x10^-5
Calculate the pH at the equivalence point when 25.0mL of 0.100M NH3 is titrated with 0.100M HCl. The reaction is given as follows : NH3 + H30+ -> NH4+ + H20 Show complete solution . Will rate your answer. Draw titration curve and label first and second equivalence point.
Calculate the pH at the equivalence point when 25.0mL of 0.100M NH3 is titrated with 0.100M HCl. The reaction is given as follows : NH3 + H30+ -> NH4+ + H20 Show complete solution . Will rate your answer.
calculate the pH & POH of a mixture containing 20.0 mL of 0.150 m HBr mixed W/ 40.0 mL of water.
calculate the pH of a 0.100M solution in NH4+ ka=5.70x10^-10
Calculate the pKb for a substance given that a 0.100M solution has a pH of 10.65.
Titration of 50.0mL of 0.100M HX (Ka=1.5x10^-5) with 0.100M NaOH. Calculate the pH of 1) initial acid solution 2) buffer formed at the addition of 12.5mL NaOH 3) buffer formed at the addition of 25.0mL NaOH 4) buffer formed at the addition of 37.5mL NaOH 5) solution obtained at the endpoint
Calculate the values of the pH at the equivalence points (two) in the titration of 50.0 mL of a mixture containing HA at 0.080 M concentration (strong acid) and HB at 0.12 M concentration (pKHB = 8.4) with NaOH 0.200 M.
1.) Calculate the pH of a solution that is prepared by taking 20.0 mL of 0.100M NH3 (a weak base) and diluting it with 180.0 mL of water at 25 degrees C. (Ka of NH3 = 1.8 *10-5