For the previous reaction write the balanced net ionic equation and identify the spectator ions & their colors. Also indicate the type of underlying chemical process {redox (R), acid-base (AB),precipitation (P)} that occurs in the reaction. Additionally, if the reaction is redox identify the oxidizing & reducing agents.{ NOTE: For the equations belowi)Put answers in the spaces to balance the equations.ii)Do NOT use subscripts or superscripts in formula answers. Put parentheses around any polyatomic species only if there is more than one of it in the formula. Put numbers on same levelas symbols (e.g.s, the ion "NO3" should be written as (NO3)-1 or (NO3)1-; Na2CO3 should be written as Na2CO3 & Ca(NO3)2 as Ca(NO3)2.)iii) Input all numerical coefficients even if it is the number "1". }i) Net ionic equation:(aq) +(ag) --->(s)(Place #s or coefficients and formulas in the spaces)ii) Spectator ions: ( remember these have charges )lon formulaColoriii) Underlying chemical process:iv) Oxidizing agent: (no coefficients, just the complete formula; if there isn't one, write none.)Reducing agent: (no coefficients, just the complete formula; if there isn't one, write none.) Predict the products then write the balanced molecular and total ionic equations for the reaction that occurs when the aqueous contents of the two beakers below are added together. Sodium(Na") ions are gray.Co2+CIONa*OHcobalt(II) chloridesodium hydroxide+------->{ NOTE: For the equations belowi)Put answers in the spaces to balance the equations.ii)Do NOT use subscripts or superscripts in formula answers. Put parentheses around any polyatomic species only if there is more than one of it in the formula. Put numbers on same levelas symbols (e.g.s, the ion "NO3"should be written as (NO3)-1 or (NO3)1-; Na2cO3 should be written as Na2CO3 & Ca(NO3)2 as Ca(NO3)2.)iii) Input all numerical coefficients even if it is the number "1". }(i) Molecular equation:(aq) +(aq)(s) +(aq)--->(Place #s or coefficients and formulas in the spaces)(ii) Total ionic equation:1 Co2*(aq) +(aq) +(aq) +(ag) --->(s) +(aq) +(aq)(Place #s or coefficients and formulas in the spaces)

Predict the products then write the balanced molecular and total ionic equations for the reaction that occurs when the aqueous contents of the two beakers below are added together. Sodium (Na") ions are gray. OCI Na* OH cobalt(II) chloride sodium hydroxide -------> + {NOTE: For the equations below i) Put answers in the spaces to balance the equations. ii) Do NOT use subscripts or superscripts in formula answers. Put parentheses around any polyatomic species only if there is more than one of it in the formula. Put numbers on same leve as symbols (e.g.s, the ion "NO3" should be written as (NO3)-1 or (NO3)1-; Na2co3 should be written as Na2CO3 & Ca(NO3)2 as Ca(NO3)2.) iii) Input all numerical coefficients even if it is the number "1". } (i) Molecular equation: (aq) + (aq) --> (s) + (aq) (Place #s or coefficients and formulas in the spaces) (ii) Total ionic equation: 1 Co2*(aq) + (aq) + (aq) + (aq) -> (s) + (aq) + (aq) (Place #s or coefficients and formulas in the spaces)

Predict the products then write the balanced molecular and total ionic equations for the reaction that occurs when the aqueous contents of the two beakers below are added together. Sodium (Na") ions are gray. OCI Na* OH cobalt(II) chloride sodium hydroxide -------> + {NOTE: For the equations below i) Put answers in the spaces to balance the equations. ii) Do NOT use subscripts or superscripts in formula answers. Put parentheses around any polyatomic species only if there is more than one of it in the formula. Put numbers on same leve as symbols (e.g.s, the ion "NO3" should be written as (NO3)-1 or (NO3)1-; Na2co3 should be written as Na2CO3 & Ca(NO3)2 as Ca(NO3)2.) iii) Input all numerical coefficients even if it is the number "1". } (i) Molecular equation: (aq) + (aq) --> (s) + (aq) (Place #s or coefficients and formulas in the spaces) (ii) Total ionic equation: 1 Co2*(aq) + (aq) + (aq) + (aq) -> (s) + (aq) + (aq) (Place #s or coefficients and formulas in the spaces)

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 42CR: 42. a. Fill in the following table as if it is a well plate and you are mixing two aqueous compounds...

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In the spectroscopic analysis of many substances, a series of standard solutions of known concentration are measured to generate a calibration curve. How would you prepare standard solutions containing 10.0, 25.0, 50.0, 75.0, and 100. ppm of copper from a commercially produced 1000.0-ppm solution? Assume each solution has a final volume of 100.0 mL. (See Exercise 123 for definitions.)
ummarize the simple solubility rules for ionic compounds. How do we use these rules in determining the identity of the solid formed in a precipitation reaction? Give examples including balanced complete and net ionic equations.
4.88 A quality control technician needs to determine the percentage of arsenic (As) in a particular pesticide. The pesticide is dissolved and all of the arsenic present is converted to arsenate ions (AsO43-). Then the amount of AsO43- is determined by titrating with a solution containing silver ions (Ag+). The silver reacts with the arsenate according to the following net ionic equation: 3Ag+(aq)+AsO43(aq)Ag3AsO4(s) When a 1.22-g sample of pesticide was analyzed this way, it required 25.0 mL of 0.102 M Ag+ solution to precipitate all of the AsO43-. What was the mass percentage of arsenic in the pesticide?