The concentration of H3ASO3 in a solution is determined by titration with a 0.1495 M Ce** solution. The balanced net ionic equation for the reaction is: 3+ 2Ce*(aq) + H3ASO3(aq) + 5H,O()- 2Ce*(aq) + H3ASO4(aq) + 2H3O*(aq) (a) If 19.80 mL of the 0.1495 M Ce** solution are needed to react completely with 40.00 mL of the H3ASO3 solution, what is the concentration of the H3ASO3 solution? (b) Which of the two solutions was in the buret during the titration? (c) Suppose at the end of the titration, the solution containing the Ce* ion is transferred to a volumetric flask and diluted to 250. mL. What is the concentration of Ce3+ in the diluted solution? M

The concentration of H3ASO3 in a solution is determined by titration with a 0.1495 M Ce** solution. The balanced net ionic equation for the reaction is: 3+ 2Ce(aq) + H3ASO3(aq) + 5H,O()- 2Ce(aq) + H3ASO4(aq) + 2H3O*(aq) (a) If 19.80 mL of the 0.1495 M Ce** solution are needed to react completely with 40.00 mL of the H3ASO3 solution, what is the concentration of the H3ASO3 solution? (b) Which of the two solutions was in the buret during the titration? (c) Suppose at the end of the titration, the solution containing the Ce* ion is transferred to a volumetric flask and diluted to 250. mL. What is the concentration of Ce3+ in the diluted solution? 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

The concentration of H₂AsO3 in a solution is determined by titrating it with a 0.1722 M Ce solution. The balanced net ionic equation for the reaction is: 2Ce+ (aq) + H₂AsO3(aq) + 5H₂0 (1) 2Ce³+ (aq) + H₂AsO4(aq) + 2H30+ (aq) In one experiment, 21.40 ml of the 0.1722-M Ce4+ solution is required to react completely with 40.00 mL of the H₂AsO, solution. Calculate the concentration of the H₂AsO solution. Submit Show Approach Show Tutor Steps
A CHM 125 student performed the "Redox Titration" procedure as given in the laboratory manual. In this experiment, the titrant solution of potassium permanganate (KMNO4) was used to determine the percentage of sodium oxalate (NazC2O4) in an unknown sample. The net ionic equation for the titration carried out was: 2MnO4 (aq) + 5C20,7(aq) + 16H*(aq) → 2MN²*(aq) + 10CO2(g) + 8H2O(£) The data provided in the table below was acquired. Complete the table and determine the percent of sodium oxalate in the unknown sample based on this one titration. Molarity of KMNO, Titrant Solution: 0.0203 M Trial 1 Weight of Oxalate 0.954 g Unknown Starting Buret Reading: 0.65 mL Ending Buret Reading: 34.85 mL of permanganate sl order to use 35.00 mL of Titrant Used: mmol of MnO4 mmol of 2- Weight of NazC204 in Unknown: Percent of Na,C204 in Unknown: You wer 4-
You are performing an experiment in lab that involves the titration of 25.0 mL of H2SO4 solution. You titrate the acidic solution with 0.8067 M NaOH and the equivalence point is reached by the addition of 17.31 mL of NaOH solution. Using the balanced equation below, calculate the molartity of H2SO4 in the flask. Do NOT include units. 2NaOH(aq) + H2SO4(aq) --> 2H2O(l) + Na2SO4(aq)
How to write a balance equation from H2C3H5O3 (aq) + KOH (aq)
Can you help me with the attached probelm?
Complete the following reaction and balance it. Fe(OH)3(aq) + HCl(aq) → a) FeCl3(aq)+ 3 H2O(l) b) FeCl(aq) + H2O(l) c) Fe(aq) + HOCl(aq) d) FeCl(aq) + 3 OH–(aq) e) H2O(l) + FeCl2(aq)
calculate the standard emf for each of tne following reactions: (a) H2(8) + F(8) → 2H*(aq) + 2 F (aq) (b) Cu2" (aq) + Ca(s) → Cu(s) + Ca²*(aq) (c) 3 Fe2*(aq) → Fe(s) + 2 Fe³*(aq) (d) 2 CIO, (aq) + 10 Br (ag) + 12 H*(aq) → Cl2(8) + 5 Br2(1) + 6 H20(I)
Nitesh
a Ammonium chloride and rubidium acetate, RbCH, CO₂, are mixed in water. Choose a balanced equation for the acid-base reaction that could, in principle, occur. O RbCH3CO₂ (s)+NH, Cl(s) + H₂O() = Rb+ (aq) + CH3CO₂¯(aq) +NH, +(aq) +Cl¯(aq) OCH3CO₂ (aq) + NH4+ (aq) CH3CO₂H(aq) + NH3 (aq) RbCH, CO₂ (aq) + NH4Cl(aq) NH₂CH3 CO₂ (aq) + RbCl(aq)
Balance this equation Mn²+ (aq) +O,(g) Mn0,(s) in basic solution.
Which of the following reactions is (are) redox reaction? (a) Zn (s) + HCI(aq) -----> ZnCl2 (aq) + H2(g) (b) Na (s) + H2SO4 (aq) -----> Na2SO4 (aq) +H2(g) (c) AGNO3(aq)+ KCI(aq) ----> AgCl(s) + KNO3(aq) (d) NaHCO3 (aq) + HBr (aq) ----> NaBr (aq) + H2O (I) + CO2 (g) 3411-- A (1) (II) C (III) None of above
please answer only d and e in question