A 0.5008-g sample that assayed 95.9% Na₂SO₄ required 48.40 mL of a barium chloride solution.**Reaction:**\[ \text{Ba}^{2+} + \text{SO}_4^{2-} \rightarrow \text{BaSO}_4(s) \]Calculate the analytical molar concentration of BaCl₂ in the solution.Concentration = _______ M

Given: Mass of Na2SO4 sample = 0.5008 g. Percent by mass of Na2SO4 in sample = 95.9 % And volume of BaCl2 solution required = 48.40 mL = 0.04840 L (Since 1 L = 1000 mL) The mass of Na2SO4 in sample = Mass of sample × percent by mass of Na2SO4100=> Mass of Na2SO4 in sample =0.5008 × 95.9100 = 0.4802672 g. Molar mass of Na2SO4 = Atomic mass of Na × 2 + Atomic mass of S + Atomic mass of O × 4=> Molar mass of Na2SO4 = 23 × 2 + 32 + 16 × 4 = 142 g/mol.Hence moles of Na2SO4 = MassMolar mass = 0.4802672142 = 0.0033822 mol approx. The precipitation reaction taking place is given by, => Na2SO4 (aq) + BaCl2 (aq) → BaSO4 (s) + 2 NaCl (aq) From the above-balanced reaction, we can see that 1 mole of Na2SO4 requires 1 moles of BaCl2. Hence moles of BaCl2 required = moles of Na2SO4 taken = 0.0033822 mol. Therefore the analytical molar concentration of BaCl2 = Moles of BaCl2 requiredVolume of solution required in L = 0.00338220.04840 = 0.06988 M approx.

Science

Chemistry

A 0.5008-g sample that assayed 95.9% Na2 SO4 required 48.40 mL of a barium chloride solution. Reaction: Ba?+ + SO4²- → BaSO4(8) Calculate the analytical molar concentration of BaCl, in the solution. Concentration M

A 0.5008-g sample that assayed 95.9% Na2 SO4 required 48.40 mL of a barium chloride solution. Reaction: Ba?+ + SO4²- → BaSO4(8) Calculate the analytical molar concentration of BaCl, in the solution. Concentration 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

(TOPIC: Gravimetry multi-component analysis) A 0.8612-g sample of a mixture of sodium bromide, sodium iodide, and sodium nitrate is analyzed by adding silver nitrate and precipitating a 1.0186-g mixture of silver bromide and silver iodide. The precipitate is then heated in a stream of chlorine gas, which converts it to 0.7125 g of silver chloride. Calculate the %w/w nitrate in the sample.
All I need is an answer. Thank you very much.
A solution of 50.0 mL of 0.20 M H2SO4 is titrated with 1.0 M of LiOH. H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O What volume of LiOH is required to neutralize the acid completely? Vol LiOH = [?] mL Hint: Be careful of the mole ratios! Vol LiOH (mL) Enter
3NaOH= H3PO4----> Na3PO4+ 3H20 A 41.0ml sample of NaOH solution of unknown concentration requires 24.3 ml of .150M H3PO4 solution to neutralize. A) what is the Molarity of the NaOH solution? Please go step by step and include correct significant figures. Thank you!
4.2
edu.co Ce... O 4 F4 144 If 35.0 g of CH3OH (MM = 32.0 g/mol) are dissolved in 500.0 mL of solution, what is the concentration of CH3OH in the solution? $ R F F5 ► 11 % 5 T G F6 6 A) 0.0700 M B) 2.18 M C) 0.00218 M D) 0.458 M F7 Y H F8 & 7 F9 * Question 5 of 9 8 DELL S K F10 ( 9 F11 O * ) O F12 P € PrtScr 00 { 10 [ + 11 Insert Delete Backspace PgUp JI 1 Enter
10) How many miligrams of BaSO4 are dissolved in a 225 mL sample of BaSO4(aq)? (Hint: calculate the solubility of a slightly soluble solute) Ksp= 1.1x 10-10
Question 5 835. mL of 0.749 M KOH(aq) is mixed with 387. mL of 0.587 M NiSO4(aq). Calculate the mass (g) of the precipitate that forms. Enter your answer to 1 decimal place. 21.1 margin of error +/- 0.3 Question 6 796. mL of 0.986 M K3PO4 (aq) is mixed with 565. mL of 0.373 M NiSO4 (aq). Calculate the concentration (M) of phosphate ion in the resulting mixture. Enter your answer to 3 decimal places. 0.473 margin of error +/- 0.005
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?
Please don't provide handwritten solution ...
Can u solve all handwriting?
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?