Use stoichiometric methods to analyze a mixture. A mixture of BaCl₂ and inert material is analyzed to determine the Ba content. First the mixture is dissolved in water. Then all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. BaCl₂(aq) + 2AgNO3(aq) →→→2AgCl(s) + Ba(NO3)2(aq) In one experiment, a 0.6280 g sample of the mixture resulted in 0.6470 g of AgCl. Determine the percent (by mass) of Ba in the mixture. % Ba

Use stoichiometric methods to analyze a mixture. A mixture of BaCl₂ and inert material is analyzed to determine the Ba content. First the mixture is dissolved in water. Then all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. BaCl₂(aq) + 2AgNO3(aq) →→→2AgCl(s) + Ba(NO3)2(aq) In one experiment, a 0.6280 g sample of the mixture resulted in 0.6470 g of AgCl. Determine the percent (by mass) of Ba in the mixture. % Ba

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

Consider the reaction: Ag* (aq) + Cl(aq) → AgCl(s) How many grams of NaCl would be needed to precipitate the Ag* ions from 2.900 x 102 mL of a 0.0115 M AgNO3 solution? The molar mass of NaCl is 58.44 g/ mol. Tap here or pull up for additional resources
Consider the reaction: Al(NO3)3 (aq) + MgCl2 (aq) ➝ AlCl3 (aq) + Mg(NO3)2 (aq). You mix together 25.0 mL of 0.85 M Al(NO3)3 and 25.0 mL of 0.90 M MgCl2 in the lab. What will the final concentration of aluminum chloride be?
You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 32.35 mL of HCl solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCl solution?
Please explain
25. A 25 mL sample of Ca(OH)2 was analyzed with a 0.10 M HCl standard. If 30 mL of the acid standard were consumed during the titration, determine the grams of calcium hydroxide Ca(OH)2 present. in the sample. Ca(OH)2(aq) + 2 HCl(aq) → CaCl2(aq) + 2 H2O(l) What is the molarity of the calcium hydroxide solution, Ca(OH)2? A) 0.05 B) 0.50 C) 0.06 D) 0.40 E) 0.34
When 50.0 mL of a 0.3000 M AgNO3 solution is added to (4.65x10^1) mL of a solution of MgCl₂, an AgCl precipitate forms immediately. The precipitate is then filtered from the solution, dried, and weighed. If the recovered AgCl is found to have a mass of (1.2x10^-1) g. what was the concentration in molarity of chloride ions in the original MgCl₂ solution? 2AgNO3(aq) + MgCl₂(aq) → 2AgCl(s) + Mg(NO3)2(aq) Use the correct number of significant figures and type in the unit abbreviation for the answer. Answer: 8.0x10^-1 M.
For the reaction of the precipitation of sulfate ions in water as BaSO4;a) Write the net ionic equation.b) What is the initial sulphate ion concentration since 0.320 g BaSO4 is precipitated as a result of the treatment with excessive amount of BaCl2 for 3500 ml of water? (Ba = 137.3 g / mol, O = 16.0 g / mol, S = 32.0g / mol, Cl = 35.45 g / mol)
n student worker in the Cal Poly chemistry stockroom is asked to determine the concentration of an aqueous solution of Ca(OH), by titration with an aqueous HNO, standard. Given that the student started with 16.4 mL of Ca(OH)2 and reached the end point with 0.9021 mL of the HNO, 20.9 M standard, what is the concentration of the Ca(OH)2 solution? Report your answer to THREE decimal places. Type your answer.
Consider the following chemical reaction. 3 Zn(C₂H₃O₂)₂(aq) + 2 Na₃PO₄(aq) → 6 NaC₂H₃O₂(aq) + Zn₃(PO₄)₂(s) A chemist makes a solution of zinc acetate by dissolving 20.5 g Zn(C₂H₃O₂)₂ in 105 mL H₂O. What is the concentration of this zinc acetate solution?
Exp # 2: suppose you have a {Zn2+(aq), Fe3+(aq)} solution, and you’re asked to separate the two ions, how do you seperate the ions and form a precipitate?
A 57.0 mL sample of a 0.118 M potassium sulfate solution is mixed with 38.0 mL of a 0.122 M lead(II)acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 1.01 g. Determine the limiting reactant, the theoretical yield, and the percent yield.
The bromide ion concentration in a solution may be determined by the precipitation of silver bromide. Ag+ (aq) + Br- (aq) yields AgBr (s) A student finds that 24.32 mL of 0.7010 M silver nitrate is needed to precipitate all of the bromide ion in a 50.00-mL sample of an unknown. What is the molarity of the bromide ion in the student's unknown?