4. A 50.0 mL solution of 0.100 M Zr** is buffered to pH=5 and titrated with 0.150 M EDTA. a. EDTA titrations are usually carried out at super high pHs. Why is it less important to do that with this one? b. Even though it's not at a high pH, the solution is still buffered. Why? c. What is pZr* at the equivalence point? Does that number make sense?

4. A 50.0 mL solution of 0.100 M Zr** is buffered to pH=5 and titrated with 0.150 M EDTA. a. EDTA titrations are usually carried out at super high pHs. Why is it less important to do that with this one? b. Even though it's not at a high pH, the solution is still buffered. Why? c. What is pZr* at the equivalence point? Does that number make sense?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.6QAP

See similar textbooks

Similar questions

Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain your answer. (i) [HA] =0.100 M = [A] (ii) [HA] = 0.300 M = [A]
Consider the following two acids: pKa1 = 2.98; pKa2 = 13.40 HO2CCH2CH2CH2CH2CO2H Adipic acid pKa1 = 4.41; pKa2 = 5.28 In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results.
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Compare the two quantities based on the given condition: At the equivalence point in the titration of Ca2+ with EDTA at pH 10.0 I. [Ca2+] II. [Y4-] a. I < II b. The two quantities cannot be compared due to insufficient information. Ic. > II d. I = II
1. Which of the following metal ions could be determined using EDTA titration at pH 2.0? a. Fe3+ b. Ca2+ c. Ag+ d. Mg2+ 2. Which of the following is not an indicator for EDTA titration? a. Calmagite b. Murexide c. Maleic acid d. Eriochrome black T
Calculate the pCl during the titration of 50.0 mL of 0.0500 M NaCl with 0.100 M AGNO3 after the addition of the following volumes of reagent: a. 10.0 mL b. 25.0 mL c. 35.0 mL For AgCl, Ksp 1.8 x 10-10. Write answers up to 3 decimal places. a. pCl b. pCl C. pCI
A water was tested for water hardness. A 50.00 mL aliquot was prepared and buffered to pH 10.0, it required 23.55 mL of 0.0250 M EDTA. A second aliquot, prepared with NaOH, was titrated with 14.53 mL of the same EDTA titrant. A. Calculate the total hardness of the water (expressed in ppm CaCO₃). B. Calculate the calcium hardness of the water (expressed in ppm CaCO₃). C. Calculate the magnesium hardness of the water (expressed in ppm MgCO₃).
100.0 mL sample of drinking water was buffered with ammonia at pH 10 and after addition of EBT required 21.4 mL of 0.00512 M EDTA for titration. FW CaCO3 = 100.09 g/mol. What will be the change in color at the end point? What is the water hardness in terms of ppm CaCO3?. What is the role of ammonia buffer in the analysis?
3.) What is the pH at the equivalence point for the titration of 50.0 mL 0.20 M nitrous acid by 0.20 M NaOH (Ka for nitrous acid = 4.5 x 10-4) A. 5.83 B. 7.00 C. 8.17 D. 9.00 Keywords: titration, equivalence point, weak acid, pH, basic salt, hydrolysis, moles, dilution, titrant, Ka, Kb, conjugate base Concepts: pH at equivalence point, acid-base behavior of salts
In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. What is the KMnO4 concentration? A. 0.040B. 0.044C. 0.021D. 0.027
a. Calculate the molar solubility of AgI in pure water. Ksp for AgI is 1.5 × 10-16. Solubility = M b. Calculate the molar solubility of AgI in 1.1 M NH3. The overall formation constant for Ag (NH3), is 1.7 × 10'. Solubility = M c. Compare the calculated solubilities from parts a and b. The solubility from (a) is greater. The solubility from (b) is greater. O The solubilities from (a) and (b) are the same.
The titration of an unknown weak acid with 0.10M NaOH is carried out and the pH at the equivalence point was found to be 8.50. Which indicator is best suited for the analyte? pKa=4.2 a. phenolphthalein pKa=9.7 b. methyl red pKa=5.0 c. methyl orange pKa=4.2 d. cresol purple pKa=8.3