An unknown sample containing a mixture of NaCl and Na2CO3 was analyzed to determine the % composition of each compound. In the analysis for Na2CO3 (soda ash), the following data were obtained mass of unknown - 0.4436 g conc. of HCl used - 0.25 N initial volume - 0.5 mL final volume - 20.0 mL (MW soda ash) 106.12) 1.) What method was used to determine the concentration of HCI? 2.) What is the net volume of HCI used in the titration? 3.) What is the % Na2CO3 in the given sample? NOTE: Round off your answer to a whole number (2 sig fig)

An unknown sample containing a mixture of NaCl and Na2CO3 was analyzed to determine the % composition of each compound. In the analysis for Na2CO3 (soda ash), the following data were obtained mass of unknown - 0.4436 g conc. of HCl used - 0.25 N initial volume - 0.5 mL final volume - 20.0 mL (MW soda ash) 106.12) 1.) What method was used to determine the concentration of HCI? 2.) What is the net volume of HCI used in the titration? 3.) What is the % Na2CO3 in the given sample? NOTE: Round off your answer to a whole number (2 sig fig)

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 Ag2CO3 will precipitate when excess (NH4)2CO3solution is added to 74.0 mL of 0.748 M AgNO3 solution? 2AgNO3(aq) + (NH4)2CO3(aq) Ag2CO3(s) + 2NH4NO3(aq)g
A sample containing a mixture of CuCl2(s) and KCI(s) with a mole fraction of 13.8% KCI was dissolved in water. An excess of AgNO3(s) is added to the mixture, resulting in the chloride being precipitated as AgCl(s). The AgCl(s) is collected and dried, weighed to have a mass of 8.40g. Calculated the masses of KCI(s) and CuCl2(s) in the original mixture.
I need the answer as soon as possible
What volume of 0.0500 M CoCl2 times 6H2O is required to react completely with 75.0 mL of 0.0500 M K3PO4?
Consider the reaction: 2 NaBH4(aq) + H₂SO4(aq) → 2 H₂(g) + Na₂SO4(aq) + B₂H6(9) What volume, in mL, of a 0.529 M solution of NaBH4 is required to produce 0.591 g of B₂H6? H₂SO4 is present in excess. mL Submit The desired mass of the product, B₂H6, is 0.591 g. What is this amount of B₂H5, in units of moles? mol B₂H6 Submit
An impure sample of KHP had a mass of 1.520 g, It was dissolved in titrated with 38.5 ml of 0.155 M NaOH solution. Calculate the % putity.
A 0.678-g sodium carbonate sample with 98.6% purity requires 36.8 mL of sulfuric acid solution to complete neutralization. What is the molarity of the sulfuric acid solution? MW Na2CO3 = 106.0 g/mol
A student determined the concentration of NaOCI in a commercial bleach sample using the same technique described in section "F" of the Halogens and Their Compounds lab. The student required 18 drops of 0.01M Na,S203 to reach the end point. What is the concentration (reported in molarity) of NaOCI in the bleach sample?
5. Sodium acetate can be formed from the metathesis/double replacement reaction of sodium bicarbonate and acetic acid. (See the Supplemental Information concerning metathesis reactions.) Determine the percent yield when 0.537 g of sodium acetate is obtained from mixing 15.0 g of NaHCO3 with 125 mL of 0.15 M acetic acid.
How many grams of pure Na2CO3 must be weighed and dissolved in a solution, if you are to prepare a 0.1478 N HCl that utilized 61.75 mL of titrant? MW Na2CO3 is 106 g/mol.
Molarity of stock KMnO4 : (read from bottle in lab) 0.01994 M Volume of KMnO4 Stock Solution added via pipet 5.00ml Calculated Molarity of solution BI
A 50.0 ml solution contains only Na2SO4 (MW 142.04 g/mole). If 40.0 ml of 0.25 M BaCl2 is needed to precipitate all the SO42- as BaSO4, what mass of Na2SO4 was in the original solution? What is the concentration of Cl- in the final solution?