**Question:**What concentration of Br⁻ results when 847 mL of 0.403 M KBr is mixed with 961 mL of 0.447 M FeBr₂?**Solution Box:**\[ \text{[Br⁻]} = \]______ M**Explanation:**This problem involves calculating the concentration of bromide ions (\[ \text{Br}^- \]) after mixing two solutions:1. **KBr Solution:** - Volume = 847 mL - Concentration = 0.403 M - \[ \text{KBr} \longrightarrow \text{K}^+ + \text{Br}^- \] - 1 mole of KBr gives 1 mole of Br⁻.2. **FeBr₂ Solution:** - Volume = 961 mL - Concentration = 0.447 M - \[ \text{FeBr}_2 \longrightarrow \text{Fe}^{2+} + 2 \text{Br}^- \] - 1 mole of FeBr₂ gives 2 moles of Br⁻.The box is left blank to fill in the final calculated concentration of \[ \text{Br}^- \].

Molarity of KBr is 0.403 M. Volume of KBr is 847 mL. Molarity of FeBr2 is 0.447 M. Volume of FeBr2 is 961 mL.Number of moles of solute present is equal to the product of molarity and volume of solution. Calculate the number of moles of solute of KBr. nKBr=0.403 M×847 mL×0.001 L1 mL=0.341 mol So, the number of moles of KBr are 0.341 mol. Calculate the number of moles of solute of FeBr2. nFeBr2=0.447 M×961 mL×0.001 L1 mL=0.429 mol So, the number of moles of FeBr2 are 0.429 mol. On the dissociation of KBr, one mole of Br-are obtained while from FeBr2, two moles of Br- are formed. KBr→K++Br-FeBr2→Fe2++2Br- Calculate the total number of moles of Br-. nBr-=0.341 mol +2×0.429 mol=1.199 mol So, the number of moles of Br- is 1.199 mol. Total volume of the solutions is 1808 mL. Calculate the concentration of Br-. MBr-=1.199 mol1808 mL×0.001 L1 mL=0.663 mol/L=0.663 M Therefore, the concentration of Br- is 0.663 M.

Answered: What concentration of Br results when…

Science

Chemistry

What concentration of Br results when 847 mL of 0.403 M KBr is mixed with 961 mL of 0.447 M FeBr, ? [Br] = 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

What concentration of Cl¯ results when 859 mL of 0.519 M LİCI is mixed with 675 mL of 0.299 M MgCl,? [CI¯] = M
If 0.500 mL of an 0.219 M NaCl solution is added to 100.0 mL of pure water. what is the concentration of the new solution? Your answer should have 3 sig figs
1.) What volume in mL of 0.220 M HBr solution is required to produce 0.0185 moles of HBr? 2.) If 11.3 g of KBr (MM = 119.00 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of KBr in the resulting solution? 3.) If 25.0 mL of a 7.90 M HCl solution is diluted to 2.00 L, what is the molarity of the new solution? 4.) What quantity in moles of KBr are there in 225.0 mL of 0.155 M KBr?
Calculate the mass of the solid product in grams that the student can recover
A student combined 45.3 mL of a 0.549 M calcium nitrate Ca(NO,), solution with 83.55 mL of a 1.321 M Ca(NO,), solution. Calculate the concentration of the final solution. 3/2
A 450.0 mL sample of a 0.257 M solution of silver nitrate is mixed with 400.0 mL of 0.200 M calcium chloride. What is the concentration of Cl' in solution after the reaction is complete? [CI]= M
If 40.7 g of CH₃OH (MM = 32.04 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of CH₃OH in the resulting solution?
Analysis shows that a 2.750 mL sample of a diprotic acid reacts completely with330.0 mL of 0.2000 M KOH solution. What is the molar mass of the unknown acid? (density of unknown diprotic acid = 1.200 g/mL)
What NaCl concentration results when 269 mLof a 0.790 M NaCl solution is mixed with 462 mLof a 0.310 M NaCl solution?
Please help me answer this question. → Calculate the concentration of all the ions present when 15.0 mL of 0.225 M CaCl2 is mixed with 10.0 mL of 0.150 M NaCl. Thank you.
Rb
What is the concentration of nitrate ions in a solution made by mixing 839 mL of 0.2 M potassium nitrate and 854 mL of 0.4 M calcium nitrate?