Na2CO3 is used to standardize a solution of HCl. What is the concentration of HCl if 0.1970 g of pure Na₂CO3 dissolved in 50.00 mL of water took 29.41 mL of HCl to reach the end point in the titration? Next, 0.4242 g of an unknown sample containing Na2CO3 was dissolved in 50.00 mL of water. It took 18.92 mL of the standardized HCl solution to reach the end point in the titration of the unknown sample. What is the wt% of Na₂CO3 in the unknown? M HCI wt % Na₂CO3

Na2CO3 is used to standardize a solution of HCl. What is the concentration of HCl if 0.1970 g of pure Na₂CO3 dissolved in 50.00 mL of water took 29.41 mL of HCl to reach the end point in the titration? Next, 0.4242 g of an unknown sample containing Na2CO3 was dissolved in 50.00 mL of water. It took 18.92 mL of the standardized HCl solution to reach the end point in the titration of the unknown sample. What is the wt% of Na₂CO3 in the unknown? M HCI wt % Na₂CO3

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.14QAP

See similar textbooks

Similar questions

Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
8-47 A sample of 27.0 mL of 0.310 M NaOH is titrated with 0.740 M H2SO4. How many milliliters of the H2SO4 solution are required to reach the end point?
13,How many milliliters of 0.0854 M NaOH are required to titrate 25.00 mL of 0.1250M HI to the equivalence point? Group of answer choices A, 17.08 B, 17.1 C, 36.6 D, no correct answer E, 36.593
A 25.00 mL sample of HCl of unknown concentration is titrated with 21.12 mL of 0.1201 M KOH to the phenolphthalien endpoint. What is the molar concentration of the HCL solution? Group of answer choices 0.1015 M 0.05073 M 0.102 M 0.051 M
. A 4.59 mL sample of HCl, specific gravity 1.3, required 50.5 mL of 0.9544N NaOH in a titration. Calculate the % w/w HCl.
A student prepared a 0.0750 M NaOH solution for a titration experiment. If it took 25.52 ml of the NaOH to turn the H2SO4 solution faint pink, how many moles of NaOH were required to reach the end point? What was the mole of H2SO4 used from 3a. question?
Consider the following infermation about sulfurous acid, a diprotic acid (11,S0,L LSO3=HSO, +1I* pK=1.81 HSO, S0,+H pK2-691 The titration curve for sodism sulfite, Na SO, with standard HCl is shown below PH VI V2 ml, HO added What are the major species present al point 3? O No
How many milliliters of 8.50x10-2 M NaOH are required to titrate each of the following solutions to the equivalence point? Show Transcribed Text V = 45.0 mL of 9.00x10-² M HNO3 Submit ▾ Part B V = —| ΑΣΦ 35.0 mL of 8.50x10-2 M CH3COOH Show Transcribed Text V = Request Answer IVE ΑΣΦ P Pearson Submit C IVE ΑΣΦ Ĉ Request Answer 55.0 mL of a solution that contains 1.80 g of HCl per liter www ? SW ? ? mL mL mL
A solution of HCl was titrated against sodium carbonate. What is the titer for Trial 1 in the given data? T2 0.3562 0.3479 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (ml) Vol HCI used (ml) 35.10 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L) A
Which of the following chemicals would be the best buffer for a pH 9.00 solution: NH3 (Kb = 1.75x10-5), C6H5NH2 (Kb = 3.99x10-10), H2NNH2 (Kb = 3.00x10-6), C5H5N (Kb = 1.69x10-9)? A) H2NNH2 B) C6H5NH2 C) NH3 D) C5H5N
1.876 g of the sample containing H2C2O4requires 38.84 mL of 0.1032 M of NaOH for titration: H2C2O4+ 2 NaOH →Na2C2O4+ 2 H2OA 1.38 mL of 0.0992 M HCl is used in the back –titration. (a)Calculate the percentage of H2C2O4in the sample.(b)Calculate the percentage expressed as the dihydrate, H2C2O4•2H2O.