A 190.0 mL solution of 2.765 M strontium nitrate is mixed with 215.0 mL of a 3.581 M sodium fluoride solution. Calculate the< Feedbackmass of the resulting strontium fluoride precipitate.The sodium ion concentration youcalculated is incorrect.When calculating the Na+concentration, you may have used the48.30mass:volume of the original NaF solution.Instead, use the total volume of bothAssuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 forsolutions to calculate the concentrationthe concentration.in the final solution.3.576[Na*] =MIncorrect2.763[NO,] =MIncorrect0.739[Sr**] =MIncorrect1.788[F=] =MIncorrect

Answered: Image /qna-images/answer/74d42509-6a39-4c94-bfeb-599449db7f5b.jpg

A 190.0 mL solution of 2.765 M strontium nitrate is mixed with 215.0 mL of a 3.581 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. 48.30 mass: g Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration. 3.576 [Na*] =| M Incorrect 2.763 [NO,] = M Incorrect 0.739 [Sr*] = M Incorrect 1.788 [F=] = M Incorrect

A 190.0 mL solution of 2.765 M strontium nitrate is mixed with 215.0 mL of a 3.581 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. 48.30 mass: g Assuming complete precipitation, calculate the final concentration of each ion. If the ion is no longer in solution, enter a 0 for the concentration. 3.576 [Na] =| M Incorrect 2.763 [NO,] = M Incorrect 0.739 [Sr] = M Incorrect 1.788 [F=] = M Incorrect

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

formula in the last column. dyueuus SUlutions A ahd B are mixed. If a precipitate will form, enter its empirical Does a precipitate form when A and B empirical formula of solution A solution B are mixed? precipitate potassium chloride lead (II) nitrate O yes O no sodium hydroxide zinc chloride O yes O no copper(II) sulfate potassium sulfide O yes O no
0.8888 g a mixture contains calcium chloride and potassium nitrate. To determine the % of each compound, silver nitrate was added to these solutions to precipitate all the chlorine in a form of silver chloride. 1.885 grams of silver chloride was precipitated, washed and dried. Calculate the % of calcium chloride in the sample.
What mass of precipitate is formed when 100. mL of 0.350 M NaCl reacts with 100. mL of 0.175 M Pb(NO3)2? g
Solid sodium hydroxide is slowly added to 75.0 mL of a 0.238 M iron(III) sulfate solution until the concentration of hydroxide ion is 0.0576 M. The mass of iron(III) ion remaining in solution is grams.
A 21.25 g of a mixture of the solid salts, sodium chloride and lead II nitrate, is added to distilled water and stirred. The precipitate that is formed is filtered and dried. Its mass was determined to be 11.06 g. Analysis of the remaining solution shoed that the following ions were present: Pb2+, Na+ and NO3". Determine the percent (by mass) of lead (II) nitrate in the mixture. Assume 100 % yield.
Suppose 31.0 mL of 0.510 M CoCl2 solution is added to 72.0 mL of 0.180 M NiCl2 solution. Calculate the concentration, in moles per liter, of each of the ions present after mixing. Assume that the volumes are additive. Concentration of Co2+ = mol/L Concentration of Ni2+= mol/L Concentration of Cl- = mol/L
d) A 38.5mL sample of 0.875M AgNO, solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate the limiting reactant, the theoretical yield, and percent yield. AGNO3(aq) + NaClaq) → AGCI6) + NaNO3(aq)
A 0.7011-g mixture of sodium chloride and sodium nitrate is completely dissolved in water. When silver nitrate is added to the solution, 0.9805 g of solid precipitate. What is the percent by mass of chloride in the initial mixture? 65.41 % 71.50 % 34.59 % 13.99 % 28.50 %
A 185 mL sample of 1.20 M Pb(NO₃)₂ is mixed with 99.5 mL of 1.50 M NaCl, and the PbCl₂ precipitate is filtered from the solution. Then 200 mL of 3.00 M NaBr is added to the remaining solution, and the PbBr₂ precipitate is also collected and dried. What is the mass of the PbBr₂ precipitate, assuming the yield in each precipitation step is 100%?