A chemist titrates 30.0 mL of a sample solution containing CI-(aq) ions with a 0.0489 mol/L KMNO4(aq) solution. The light purple-coloured end point is attained after the addition of 22.5 ml of the KMNO4(aq) (solution in the buret). The KMnO4faq) dissolve, and the balanced net ionic equation is: 2MNO4 (aq) + 10CI-(aq) + 16H*(aq) → 2Mn²+ (aq) + 5C12(g) + 8H2O( 2 ) The molar concentration of CI-(aq) ions in the sample solution is: a. 0.0489 mol/L 0.300 mol/L С. b. 0.225 mol/L d. 0.183 mol/L

A chemist titrates 30.0 mL of a sample solution containing CI-(aq) ions with a 0.0489 mol/L KMNO4(aq) solution. The light purple-coloured end point is attained after the addition of 22.5 ml of the KMNO4(aq) (solution in the buret). The KMnO4faq) dissolve, and the balanced net ionic equation is: 2MNO4 (aq) + 10CI-(aq) + 16H*(aq) → 2Mn²+ (aq) + 5C12(g) + 8H2O( 2 ) The molar concentration of CI-(aq) ions in the sample solution is: a. 0.0489 mol/L 0.300 mol/L С. b. 0.225 mol/L d. 0.183 mol/L

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section12.3: Determining Equilibrium Constants

Problem 12.3PSP

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