What is the pCl of the solution during the titration of 50.0 mL of 0.100 M NaCl with 0.100 M AgNO3 after the addition of 0.00 mL, 10.0 mL, 49.9 mL, 50.0 mL, and 60.0 mL.  And graph pCl vs mL of AgNO3 added.

16.0mL of a 0.750M solution of H>COz are titrated with a 1.0OOM solution of KOH. At what volume of base will the equivalence point be reached? 42.7 mL 12.0 mL O24.0 mL 20.0 mL 21.3 mL

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Consider the titration of a 25.0mL sample of 0.195M acetic acid (CH3COOH) with 0.300M NaOH. How many mL of NaOH is required to reach the equivalence point? The Ka of acetic acid is 1.8x10-5.

30.0 mL of 0.400 M KOH is titrated using 0.300 M H2SO4. What is volume of H2SO4 needed to reach the equivalence point? 30.0 mL 40.0 mL 20.0 mL 15.0 mL

Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N, with 0.1000 M HCl solution after the following additions of titrant. 10.00 mL: 21.00 mL: 28.00 mL:

Consider the titration of 80.0 mL of 0.0200 M NH3 (a weak base; Kb = 1.80e-05) with 0.100 M HIO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mLpH =  (b) 4.0 mLpH =  (c) 8.0 mLpH =  (d) 12.0 mLpH =  (e) 16.0 mLpH =  (f) 22.4 mLpH =

A Consider the pH titration curve above (pH vs volume in ml). The pk, of the weak base being titrated and the pH of the equivalence point are, respectively: 12 11 10 8 7 5 4 2 1 10 20 30 40 O 2.5 and 4.0 • 5.4 and 4.5 O 11.2 and 5.4 O 11.2 and 4.5 O 4.5 and 5.4 Based on the indicator information above, which of the following indicators could be used successfuly in the titration in Part A? (Select all correct responses. Indicator Colour (low pH – high pH) pK, methyl yellow red-yellow 3.1 methyl orange red-yellow 3.7 bromophenol blue yellow-blue 4.2 bromocresol green yellow-blue 4.7 methyl red pink-yellow 5.1 bromocresol purple bromothymol blue yellow-purple 6.3 yellow-blue 7.0 phenol red yellow-red 7.9 O phenol red cresol red yellow-red 8.3 O bromocresol purple thymol blue yellow-blue 8.9 O methyl yellow thymolphthalein colourless-blue 9.2 O bromothymol blue O thymol blue O thymolphthalein Part C Baseu on the table above, what colour is methyl orange at pH3? Submit Request Answer Part…

Consider the titration of 50.0 mL of 1.00 M H3ASO4(Ka1 = 5.6\times 10-3, Ka2 = 1.7\times 10-7, Ka3 = 4.0\times 10-12) with 1.00 MKOH. Calculate the pH after the addition of each of the following volumes of base. A) 25 mL B) 50 mL C) 75 mL D) 100 mL

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