A 50.00 mL aliquot of 0.1000 M acetic acid is titrated with a 0.0500 M KOH. Calculate the pH when 25.00 mL of base is added. Ka = 1.75 x 10â5
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In a titration experiment, 50.00 mL of 0.10 M acetic acid (formal concentration, (Ka = 1.75 x 10^-5 at 25 C) was titrated with a 0.10 M NaOH (formal concentration ) at 25 C. The pH of the solution at 50.00 mL of this titrant will be this
1. A 25.00 mL aliquot of a 0.050 M weak acid (Ka = 1.0 x 10-4) is titrated with 0.100 M KOH. What is the pH after the addition of the following volumes of base:
a) 10
b) 13
2. What mass of lead chloride (278.10 g/mol; Ksp = 1.7 x 10-5) dissolve in 500.0 mL of 0.550 M NaCl solution?
Calculate the pH during the titration of 30.00 mL of 0.1000 M C6H5OH(aq) with 0.1000 M KOH(aq) after 18 mL of the base have been added. Ka of phenol = 1.0 x 10-10.