(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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- A chemist wishes to prepare 121.00 mL of acetic acid/sodium acetate buffer solution with a pH of 4.55 and a total concentration of the components equal to 0.35 M. The pKa for acetic acid is 4.75. (a) What mass of acetic acid (molar mass 60.05 g/mol) is required? (b) What mass of sodium acetate (molar mass 82.03 g/mol) is required?arrow_forwardThe 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_forward
- Consider 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_forwardSuper 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_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
- Consider the titration of 36.0 mL of 0.123 M ammonia with 0.0766 M HCl. (See the Acid-Base Table attached.) (a) How many mL of HCl are required to reach the equivalence point?57.8 mL(b) What is the pH at the equivalence point? 5.29(c) What is the pH of the solution after the addition of 17.2 mL of acid? (d) What is the pH of the solution after the addition of 84.3 mL of acid? (only need help witn c and d)arrow_forwardA buffer contains 0.010 mol of lactic acid (pKa = 3.86) and 0.050 mol of sodium lactate per liter. (a) Calculate the pH of the buffer. (b) Calculate thechange in pH when 5 mL of 0.5 M HCl is added to 1 L of the buffer. (c) What pH change would you expect if you added the same quantity of HCl to 1 L of pure water?arrow_forward(a) Why is the pH at the equivalence point for the titration of a strong acid with a strong base equal to 7.00? (Select all that apply in this situation). The conjugate of a strong base is a weak acid. 000 At the equivalence point only water and a neutral salt are present. The conjugate of a weak acid is a weak base. The anions of strong acids are neutral. The cations of strong bases are neutral. (b) Why is the pH at the equivalence point of a titration generally not equal to 7.00 for the titration of a weak acid with a strong base? (Select all that apply in this situation). At the equivalence point only water and a neutral salt are present. The conjugate of a strong base is a weak acid. The cations of strong bases are neutral. The conjugate of a weak acid is a weak base. The anions of strong acids are neutral.arrow_forward
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