(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
- What accounts for the discrepancy in pH? When you have already dissolved the computed masses of reagents for the buffer in an ample amount of distilled water, and upon checking the pH using the pH meter the pH is less than the target pH.arrow_forwardDefine and explain the significance of the equivalence point of a titration. Identify the role of the indicator in this context.arrow_forwardDescribe the changes in pH that take place during the titration of: (a) a weak acid with a strong base, (b) a weak base with a strong acid .arrow_forward
- b) In the development of a method for the determination of formic acid by neutralization volumetry, the pH was calculated as a function of the addition of NaOH for the titration of 25.00 mL of 0.1280 mol/L formic acid with NaOH standardized with concentration of 0.0670 mol/L. With reference to this titration curve, determine the pH of the solution after the addition of 5.00 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two places after the comma and show your calculations. c) Based on the table below, indicate which indicators could be used to determine the end point of this titration.arrow_forward134 grams of potassium sorbate KCH3 (CH)4CO2 is fully dissolved in 100.00 mL of water, which is carefully transferred to a conical flask. Then 100.00 mL of 0.240 M HNO3 is added dropwise to this solution from a burette. Given: Ka (sorbic acid) = 1.7 × 1O^-5 Showing all your calculations and reasoning, determine the pH of the solution that results after the addition of all the acid mentioned above. Suppose that the titration continues. Determine the pH of the solution in the flask at theequivalence pointarrow_forwardA buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00 ml of this buffer solution contains 0.025 moles of HA and 0.066 moles NaA, and has a measured pH of 4.61, what is the pKa of the unknown weak acid?arrow_forward
- Cd+2 and Fe+2 (starting concentration 10 mol/L) should be separated by fractionated precipitation using H₂S. Does a pH range exist allowing to completely precipitate one metal (i.e. the remaining concentration of the precipitated ion has to be 10 mol/L or less) whereas the other stays in solution at its initial concentration? Please calculate this pH range whereby pH values below zero are set to zero! Please illustrate the situation graphically by plotting pH versus in solution/precipitating/fully precipitated for the two ionsarrow_forwardAn approximately 0.1-molar solution of NaOH is to be standardized by titration. Assume that the following materials are available. Clean, dry 50 mL buret •Analytical balance 250 mL Erlenmeyer flask •Wash bottle filled with distilled water Phenolphthalein indicator solution Potassium hydrogen phthalate, KHP, a solid monoprotic acid (to be used as the primary standard) Briefly describe the steps you would take, using the materials listed above, to standardize the NaOH solution. Describe (the set up) the calculations necessary to determine the concentration of the NaOH solution.arrow_forwardSketch the general appearance of the curve for the titration of a weak acid with a strong base. Explain (in words) what chemistry governs the pH in each of the four distinct regions of the curve.arrow_forward
- Lakes have a natural buffering capacity, especially in regions where limestone gives rise to dissolved calcium carbonate. Write an equation for the effect of a small amount of acid rain containing sulfuric acid if it falls into alake containing carbonate (CO3-2 ) ions. Discuss how the lake will resist further pH changes. What happens if a large excess of acid rain is deposited?arrow_forwardHow the pH at the equivalence point is determined by the species present; why the pH at the midpoint of the buffer region equals the pKa of the acidarrow_forwardIn a titration, 10.543 mL of a 1.112 M weak acid solution are placed in a 125 mL Erlenmeyer flask. A 1.249 M solution of NaOH (aq) is placed in the buret and filled to the 0.00 mL mark. NaOH solution is added to the flask and the buret reading is now 18.119. What is the pH of the solution? Enter your answer with at least 4 sig figs. The pKa of the weak acid is 4.954. (please type answer not write by hend)arrow_forward