Answered: What volume (in mL) of 2.0 M NaOH must…

What volume (in mL) of 2.0 M NaOH must be added to 500 mL of 0.300 M acetic acid to produce a buffer solution with a pH of 4.2? (Ka = 1.75 x 10 -5) %3D Select one: 19.4 O 16.3 13.5 26.7 22.9

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

What volume (in ml) of 2.0 M NaOH
must be added to 500 ml of 0.300
M acetic acid to produce a buffer
solution with a pH of 4.2? (Ka = 1.75
x 10 -5)
Select one:
O 19.4
16.3
13.5
26.7
22.9
Clear my choice

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Please assist with this question. I am confused.
3 a) The Ka value for phenolphthalein is 8 x 10-10. What is the concentration of hydrogen ton when this indicator changes colour? b) What is the pH at end paint? c) From your pH curve, why is the assumption that end point equals equivalence point valid for phenolphthalein?
5:48 PM Wed Nov 16 Today 5:48 PM 目。 oint when 15.0 ml. of o. 75% Calculate the pH of a titration at the point when 15.0 mL of 0.15 M NaOH is added to 30.0 mL of 0.20 M HNO3 Edit G ¯¯¯
A 20.0 mL solution of 0.200M weak acid HA is titrated with a 0.400M NaOH solution.(Ka of HA = 5.0 x 10-6).Calculate the pH after the following addition of the NaOH solution:a) 0.00 mLb) 5.00 mLc) 10.00 mL d) 13.50 mL
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Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is best suited for preparing a buffer solution with pH of 4.74? Question 2 options: NH3 / NH4Cl (Ka = 5.6 × 10–10) NaNO2 / HNO2 (Ka = 4.5 × 10–4) CH3COONa / CH3COOH (Ka = 1.8 × 10–5) NaCl / HCl NaOCl / HOCl (Ka = 3.2 × 10–8)
You have 25.00 mL of a solution containing 0.1125 M benzoic acid (pKa = 4.20) in a flask that you titrate with 0.2250 M NaOH to a Phenolphthalein endpoint. What is the pH after the following additions of NaOH: a) 12.5 mL of NaOH b) 6.25 mL NaOH c) 15 mL NaOH
1. Calculate the pH change [CH3COOH]=3.5*10^-3M, Ka of NaH2PO4/Na2HPO4 = 6.2×10^-8 A) add 0.5mL acetic acid to pH 7 buffer(0.1M NaH2PO4 19.5mL + 0.1M Na2HPO4 30.5mL) B) add 0.5mL acetic acid to 0.1M NaH2PO4 C) add 0.5mL acetic acid to 0.1M Na2HPO4
Use Figure to find an indicator for these titrations:(a) 0.10 M CH₃NH₂ with 0.10 M HCl(b) 0.50 M HI with 0.10 M KOH