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A 20.0-mL sample of 0.200 M HBr solution is titrated with
Chapter , Problem 17.43(choose chapter or problem)
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added: (a) 15.0 mL, (b) 19.9 mL, (c) 20.0 mL, (d) 20.1 mL, (e) 35.0 mL.
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QUESTION:
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added: (a) 15.0 mL, (b) 19.9 mL, (c) 20.0 mL, (d) 20.1 mL, (e) 35.0 mL.
ANSWER:Problem 17.43 A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added: (a) 15.0 mL, (b) 19.9 mL, (c) 20.0 mL, (d) 20.1 mL, (e) 35.0 mL. Step-by-step solution Step 1 of 20 +(A) To determine the moles of H ion from 0.200M HBr; +Moles of H ion = Molarity (M) x Volume (L) = 0.200M x 0.020L H ion = 4 x 10 mol 3