16.792 g of Ba(OH)2 (171.342 g.mol') is weighed out and carefully dissolved to make a 500.00cm³ solution. A 25.00 cm³ of this solution is pipette then transfer into a 100.00 mL volumetric flask, filling up to the mark with water. A 40.00 mL sample of this diluted solution is then reacted with a 0.753 M solution of HNO3. Ba(OH)2(aq) + 2HNO3(aq) → Ba(NO3)2(aq) + 2H20(1) The moles of Ba(OH)2 transferred to the beaker is: 1.96 x 10-3 mol 5.21 x 10-3 mol 4.90 x 102 mol 1.96 x 10-1 mol O 3.92 x 10-3 mol O None of the above

16.792 g of Ba(OH)2 (171.342 g.mol') is weighed out and carefully dissolved to make a 500.00cm³ solution. A 25.00 cm³ of this solution is pipette then transfer into a 100.00 mL volumetric flask, filling up to the mark with water. A 40.00 mL sample of this diluted solution is then reacted with a 0.753 M solution of HNO3. Ba(OH)2(aq) + 2HNO3(aq) → Ba(NO3)2(aq) + 2H20(1) The moles of Ba(OH)2 transferred to the beaker is: 1.96 x 10-3 mol 5.21 x 10-3 mol 4.90 x 102 mol 1.96 x 10-1 mol O 3.92 x 10-3 mol O None of the above

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 following reaction H2S (g) + FeS(s) + CO2(g) →FeS2(s) + HCO2H(aq) If 2.00 g of each reactant is each dissolved in 250.0 mL of water and all the solutions are mixed together. The final volume was measured to be 750.0 mL. a)How many grams of CO2 left unreacted? b) What is the concentration of HCO2H in this solution?
A solution contains Al3+ and Co2+. The addition of 0.3808 L of 1.706 M NaOH results in the complete precipitation of the ions as Al(OH)3 and Co(OH)2. The total mass of the precipitate is 22.87 g. Find the masses of Al3+ and Co2+ in the solution.
A student pipets 13 mL of a 0.0115 M solution of CaCl2 into a 100.00 mL volumetric flask and dilutes to the mark. What is the concentration of the resulting solution?
A student weighs out a 3.79 g sample of potassium nitrate, transfers it to a 250 mL volumetric flask, adds enough water to dissolve it and then adds water to the 250 mL tic mark. What is the molarity of KNO3 in the resulting solution? M
You are asked to determine the percentage of the components of a mixture containing sodium iodide, NaI, magnesium hydroxide, Mg(OH)2, and barium sulfate, BaSO4. The total mass of your mixture sample is 4.82g. First you extracted the NaI from the mixture with water and filtered insoluble Mg(OH)2and BaSO4 from the solution, containing the NaI. After evaporating and drying the filtrate, you find that you have recovered 0.95g of NaI. When you react the insoluble residue of Mg(OH)2 and BaSO4 with 3M HCl, the Mg(OH)2 dissolves. After decanting the supernatant liquid containing aqueous MgCl2 from the insoluble BaSO4 and drying the solid, you recover 2.04g of BaSO4. Finally you add 3M KOH solution to the aqueous solution to precipitate the Mg(OH)2. After filtering thesolution and drying the precipitate, you recovered 1.21g of Mg(OH)2. Calculate the percent NaI in the original sample mixture.
A student weighs out a 11.4 g sample of AI(CH3COO)3, transfers it to a 250. mL volumetric flask, adds enough water to dissolve it and then adds water to the 250. mL tick mark. What is the molarity of aluminum acetate in the resulting solution? Molarity = M
A student pipets 18 mL of a 0.0459 M solution of CaCl2 into a 100.00 mL volumetric flask and dilutes to the mark. What is the concentration of the resulting solution?
A mixture contains only NaCl and Al2(SO4)3. A 2.67-g sample of the mixture is dissolved in water and enough amount of NaOH is added, producing a precipitate of Al(OH)3. The precipitate is filtered, dried, and weighed. The mass of the precipitate is 0.754 g. What is the mass percent of Al2(SO4)3 in the sample? Assume that all aluminum is precipitated as Al(OH)3.
What mass of solid product is formed when 50.0 mL of 0.10 M Pb(NO3)2 (aq) is mixed with 75.0 mL of 0.10 M NaCl (aq)? Assume a 100% yield. Thank you!
You are given a solid that is a mixture of Na2SO4 and K₂SO4. A 0.205g sample of the mixture is dissolved in water. An excess of an aqueous solution of BaCl₂ is added. The BaSO4 that is formed is filtered, dried, and weighed. Its mass is 0.298g. What are the percent compositions by mass of Na₂SO4 and K₂SO4 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
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 12.40 g PbCl2(s) is obtained from 200.0 mL200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution.