A 0.4108-g sample of primary-standard Na2 CO3 was treated with 46.50 mL of dilute perchloric acid. The solution was boiled to remove CO2, following which the excess HClO4 was back-titrated with 9.90 mL of dilute NaOH. In a separate experiment, it was established that 26.90 mL of the HC1O4 neutralized the NaOH in a 24.00-mL portion. Calculate the molarities of the HC104 and NaOH. Molarity of the HC1O4 = M Molarity of the NaOH = M

A 0.4108-g sample of primary-standard Na2 CO3 was treated with 46.50 mL of dilute perchloric acid. The solution was boiled to remove CO2, following which the excess HClO4 was back-titrated with 9.90 mL of dilute NaOH. In a separate experiment, it was established that 26.90 mL of the HC1O4 neutralized the NaOH in a 24.00-mL portion. Calculate the molarities of the HC104 and NaOH. Molarity of the HC1O4 = M Molarity of the NaOH = M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

How many grams of (CH3)2NH2CI must be added to 1.00 L of 0.200 M (CH3)2 NH to produce a buffer with pH = 10.65? Assume no change in volume. pKp of (CH3)2 NH = 3.27 molar mass (CH3)2NH2CI = 81.6 g/mol O 6.91 g O 0.11 g O 19.6 g 0.34 g O 24.0 g 0.22 g
A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution. Dimethylamine is a weak base with K₁=5.4 × 10-4. What mass of (CH3)NH₂Br should the student dissolve in the (CH3) NH solution to turn it into a buffer with 2 pH = 11.05? You may assume that the volume of the solution doesn't change when the (CH3)NH₂Br is dissolved in it. Be sure your answer has a 2 unit symbol, and round it to 2 significant digits.
7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. H3C6H5O7 (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?
A pipette is used to add 41 mL of 0.2 M Pb(NO3)2 to a 268.0 mL solution of 0.2 M NaF. Determine the equilibrium concentration of Pb2+(aq) in the final solution. Ksp(PbF2)=3.6E-8Include at least 3 significant figures in your answer.
An alkaline earth hydroxide, M(OH)2, was taken to lab for analysis. The unknown powder was poured into a flask and swirled in room temperature DI water until a saturated solution formed. This solution was then slowly filtered to remove the undissolved solid hydroxide. 11.9 mL of this saturated solution was titrated with 0.148 M HCI (ag). Endpoint required 15.6 mL of the HCl (ag) solution. Calculate the Kan for this alkaline earth hydroxide.
7.) A saturated solution of M(OH)2 is prepared and then filtered to remove any undissolved solid M(OH)2. 15.0 mL of the filtered, saturated solution was titrated with a 0.035 M HCI solution. Examination of the pH titration curve indicated that it took 11.60 mL of the HCl solution to reach the equivalence point. What is the [M2+] in the saturated solution? [M2+] =
(a) Lactic acid, (CH3CH(OH)COOH) is a common biomolecule which can accumulate in muscles during intense exercise. A chemist prepares a buffer using 225 mL of 85 M lactic acid (Ka = 1.38 x 10-4) and 435 mL of 0.68 M sodium lactate. What is the pH of the buffer? What is the pH of the lactate buffer if 0.25 moles of gaseous HCl is added?
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
You used the back-titration method to experimentally determine the amount of CaCO3 in an Ultra Strength Tums antacid tablet. You calculated that you used 21.5 mmol HCl to complete the titration of a 2.139 g Tums tablet. What is the mass (in mg) of the active ingredient in the Tums tablet? (CaCO3 = 100.1 g/mol)
Calculating the pH of a weak acid titrated with a strong base 0/5 Izabella An analytical chemist is titrating 127.4 mL of a 0.4200M solution of nitrous acid (HNO 2) with a 0.2400M solution of KOH. The pK of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 260.9 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = 0 ☑ G 000 18 Ar B
P
In the titration of 25.00 mL of a water sample, it took 20.590 mL of 3.150x 10−3 M EDTA solution to reach the endpoint. The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures)