1. What is a âback-titrationâ?

2. Why is a back titration necessary in this experiment?

3. Calculate the number of moles of base equivalents in: a) 675 mg CaCO3 b) 135 mg Mg(OH)2 - Base equivalents = number of moles of acid (H+ ) consumed

4. Calculate the number of moles of acid (H+ ) in 33.6 mL of (a) 0.10 M HCl and (b) 0.10 M H2SO4.

5. Calculate the pH of each of the following solutions: a) 0.10 M HCl b) 2.0 x 10-4 M HNO3 c) 0.015 M NaOH d) 12 M HCl

6. Suppose that the pH meter indicates that the pH of three solutions is 2.00, 7.15, and 10.50, respectively. Calculate the [H3O+ ] of each of these solutions in molarity.

7. What quantities are plotted on the x- and y-axes of an acid-base titration curve?

8. What do the rapid changes or âbreaksâ in a titration curve represent?

9. What does the equivalence point in a titration represent?

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Lelia LubowitzLv2

31 Dec 2019

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Using the pKa values in Appendix G and activity coefficients from Table 8-1, calculate the pH of each of the following buffer solutions without activity and with activity. 0.025 M NaHCO_3 and 0.0030 M NaHCO_3 0.050 M NaHCO_3 and 0.015 M Na_2CO_3 0.0050 M disodium hydrogen citrate and 0.050 M sodium dihydrogen citrate. 0.050 M citric acid and 0.0050 M sodium dihydrogen citrate 0.050 M NaF and 0.040 M HF For each buffer system from problem #4, calculation the pH of the resultant solution when 15.00 mL of 0.005000 M HCl are added, 15.00 mL of 0.0400) M NaOH is added, and 5.00 mL of 0.02500 M HCl and 8.00 mL of 0.03500 mL of NaOH are added. Assume a 100 mL sample of your buffer, made fresh for each part. Plot a titration curve of a 30.00 mL aliquot of 0.05000 M sodium hypochlorite with 0.07250 M HCl. Your plot should include a minimum of 10 points prior to the equivalence point and 10 points after the equivalence point. Plot a titration curve of a 25.00 mL aliquot of 0.1000 M diprotic weak acid (pK_1 = 2.00, pK_2 = 6.50) with 0.05000 M NaOH. Your plot should include a minimum of 10 points in each variable range of the titration curve and both equivalence points. Do NOT calculate the 1^st (acid only in solution) point (0.00 mL NaOH added). This plot has the same issue as the one in class. When titrating a weak, unknown base with HCl, you performed the following series of standardizations. Initially, you made a solution of approximately 0.1000 M NaOH and standardized this solution with KHP. You then diluted slock HCl to make a solution of approximately 0.1000 M. In an acid/base titration, you took a 25.00 mL aliquot of your HCl solution and titrated it with the standardized NaOH. Due to a bad day in lab, this standardization took more than 4 trials. Throw out any outliers. Finally, a pH titration was performed with a 25.00 mL aliquot of your unknown weak base. This solution was made by dissolving 3.4581 grams of your unknown in 250.0 mL of water. Determine the pKb of your weak base (Don't worry about error in this value!). In addition, determine the molecular mass of the base and the error in this value. This error will be slightly flawed, you only did ONE titration of your unknown, so all of your error will come from the standardizations. Data will be provided in an Excel file emailed from the Instructor after this exam has been assigned.

advance study assignment molar mass of an acid.
1. 7.2ml of 6.0M NaOH there are in 7.2ml of 6.0 M NaOH are diluted with water to a volume of 400.0ml. you are asked to find the molarity of the resulting must be solution.
a. first find out how many moles of NaOH there are in 7.2ml of 6.0 M NaOH. use equation 1. note that the volume must be in liters.
b. since the total number of moles of NaOH is not changed on dilution, the molarity after dilution can also be found by equation 1. using the final volume of the solution. calulate the molarity.
2. in an acid base titration, 21.16ml of an NaOH solution are needed to neutralize 20.04ml of a 0.0997M HCL solution. to find the molarity of the NaOH solution, we can use the following procedures.
a. first note the value of MH+ in HCL solution.
b. find MOH- in NaOH solution equation 3
c. obtain M NAOH from M OH
3. a 0.3012g sample of an unknown monoprotic acid requires 24.13ml of 0.0944 M NaOH of neutralization to a phenolpthalein end point. there are 0.32ml of 0.0997 M HCL used for back titration.
a. how many moles of OH- are used?
how many moles of H+ from HCL?
_____moles OH- _______ moles H+
b. how many moles of H+ are there in the solid acid? use eq 5.
____moles H+ in solid
c. what is the molar mass of the unknown acid? use equation 4.
______g/mol

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