(a)
Interpretation:
The acid with larger Ka value should be detected and reason of larger value should be explained.
Concept Introduction:
The value of
(b)
Interpretation:
pH should be estimated for each acid and difference between their values should be explained.
Concept Introduction:
Equivalence point is the point of titration curve where, the amount of titrant added is stoichiometrically enough to neutralize the amount of sample. It is detected at halfway of the steep curve.
The pH at this point will be the equivalent pH.
(c)
Interpretation:
If volume of acids A and B are taken equal then, acid with higher initial concentration should be determined.
Concept Introduction:
pH gives the concentration of
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Chapter 12 Solutions
Chemistry for Engineering Students
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- The drawing below represents a buffer composed of equal concentrations of a weak acid, HX, and its conjugate base, X-'. The heights of the columns are proportional to the concentrations of the components of the buffer. (a) Which of the three drawing (1), (2), or (3) represents the buffer after the addition of a strong acid? Explain. (b) Which of the three represents the buffer after the addition of a strong base? Explain. HX X HX X- HX X HX X (1) (2) (3) Copyright © 2006 Pearson Prentice Hall, Inc.arrow_forwardExplain (molecularly) why in the titration of a weak base with strong acid, the titration curve is flat once some titrant has been added but before the equivalence point is reached?arrow_forwardConsider the titration of 36.0 mL of 0.117 M ammonia with 0.0752 M HCl. (See the Acid-Base Table.) (a) How many mL of HCl are required to reach the equivalence point?5.60 mL(b) What is the pH at the equivalence point? 5.30(c) What is the pH of the solution after the addition of 15.7 mL of acid? (d) What is the pH of the solution after the addition of 82.9 mL of acid? only need part c and d pleasearrow_forward
- Super Ninja has a 10.00 mL sample of 0.15 M of chlorous acid, HClO2(aq). 1)This acid is titrated with 0.20 M sodium hydroxide, NaOH. (i) Calculate the initial pH of the acid before titrating. (ii) Calculate the pH at the equivalence point. (iii) what indicator would you choose for this titration? explain why?arrow_forwardSuper Mario has a 10.00 mL sample of 0.10 M of nitrous acid, HNO2(aq) This acid is titrated with 0.20 M sodium hydroxide, NaOH. (i) Calculate the initial pH of the acid prior to titrating. (ii) Calculate the pH at equivalence point. (iii) Calculate the pH after 10.00 mL of NaOH is added. (iv) Would a buffer ever form in this titration? Explain.arrow_forwardCalculate pH for a weak base/strong acid titration. Determine the pH during the titration of 35.9 mL of 0.286 M methylamine (CH3NH₂, Kp = 4.2x10-4) by 0.286 M HCIO4 at the following points. (a) Before the addition of any HCIO4 (b) After the addition of 13.2 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 54.9 mL of HCIO4arrow_forward
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