EDTA is a hexadentate ligand containing four carboxylic acid groups and two amines.Which is true for the acid-base properties of EDTA? I EDTA is a hexaprotic system,H6Y2+,when the amines are protonated. II Neutral EDTA,H4Y,is tetraprotic when the amines are not protonated. III Deprotonated EDTA,Y4−,is the only form of EDTA that binds to metal cations. IV The fraction of EDTA in any of the six EDTA species is pH dependent.

A) III and IV B) I and II C) I,III,and IV D) II,III,and IV E) I,II,and IV A) III and IV B) I and II C) I,III,and IV D) II,III,and IV E) I,II,and IV E

Calculate pBa when 35.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba2+.For the buffered pH of 10, = 0.30.Kf = 7.59 × 107 for BaY2−.

A) 1)39 B) 1)75 C) 4)56 D) 4)82 E) 4)70 A) 1)39 B) 1)75 C) 4)56 D) 4)82 E) 4)70

Calculate pBa when 75.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba2+.For the buffered pH of 10, = 0.30.Kf = 7.59 × 107 for BaY2−.

A) 7)06 B) 3)53 C) 4)33 D) 7)58 E) 4)59 A) 7)06 B) 3)53 C) 4)33 D) 7)58 E) 4)59

Calculate pBa when 35.00 mL of 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba2+ in the presence of 0.1 M nitrilotriacetate. = 1.48 × 10−4. = 0.30 for pH 10.Kf = 7.59 × 107 for BaY2−.

A) 4)82 B) 2)64 C) 1)75 D) 4)55 E) 3)53 A) 4)82 B) 2)64 C) 1)75 D) 4)55 E) 3)53

Calculate pBa when 50.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba2+.For the buffered pH of 10, = 0.30.Kf = 7.59 × 107 for BaY2−.

A) 1)30 B) 7)88 C) 4)59 D) 7)36 E) 4)33 A) 1)30 B) 7)88 C) 4)59 D) 7)36 E) 4)33

Exam 13: Edta Titrations

EDTA is a hexadentate ligand containing four carboxylic acid groups and two amines.Which is true for the acid-base properties of EDTA? I EDTA is a hexaprotic system,H₆Y²⁺,when the amines are protonated. II Neutral EDTA,H₄Y,is tetraprotic when the amines are not protonated. III Deprotonated EDTA,Y⁴⁻,is the only form of EDTA that binds to metal cations. IV The fraction of EDTA in any of the six EDTA species is pH dependent.

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(Multiple Choice)

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Question 1

Correct Answer:

Verified

Which is NOT an end point detection method used with EDTA titrations?

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

A____________________ titration is necessary for analytes that precipitates in the absence of EDTA,that reacts slowly with EDTA or that blocks the indicator.

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

Calculate pBa when 35.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba²⁺.For the buffered pH of 10, = 0.30.K_f = 7.59 × 10⁷ for BaY²⁻.

(Multiple Choice)

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Question 4

Calculate [Mn²⁺] when 50.00 mL of 0.1000 M Mn²⁺ is titrated with 17.00 mL of 0.2000 M EDTA.The titration is buffered to pH 11 for which = 0.81.K_f = 7.76 × 10¹³

(Short Answer)

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Question 5

Which statement is NOT true?

(Multiple Choice)

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Question 6

Calculate for a 0.2 M EDTA solution buffered at pH 10.00.For EDTA K₁ = 1.0,K₂ = 31.6,K₃ = 100,K₄ = 490,K₅ = 1.35 × 10⁶ and K₆ = 2.34 × 10¹⁰.

(Short Answer)

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Question 7

Calculate [Ba²⁺] when 35.00 mL of 0.2000 M EDTA is added to 50.00 mL of 0.1000 M Ba²⁺ in the presence of 0.1 M nitrilotriacetate. = 1.48 x 10⁻⁴. = 0.30 for pH 10.K_f = 7.59 × 10⁷ for BaY²⁻.

(Essay)

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Question 8

The reaction between Al³⁺ and EDTA is too slow for direct titration.To a 25.00 mL Al³⁺ sample 50.00 mL of 0.2000 M EDTA is added and allowed to react for 30 minutes.The excess EDTA was titrated with 21.23 mL of 0.1000 M Zn²⁺.What is the concentration of Al³⁺ in the sample?

(Short Answer)

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Question 9

Calculate pBa when 75.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba²⁺.For the buffered pH of 10, = 0.30.K_f = 7.59 × 10⁷ for BaY²⁻.

(Multiple Choice)

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Question 10

Calculate [Mn²⁺] when 50.00 mL of 0.1000 M Mn²⁺ is titrated with 25.00 mL of 0.2000 M EDTA.The titration is buffered to pH 11 for which = 0.81.K_f = 7.76 × 10¹³

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Question 11

The____________________ is the ability of multidentate ligands to form more stable metal complexes than those formed by similar monodentate ligands.

(Multiple Choice)

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Question 12

A____________________ is a reagent that protects a component of the analyte from reaction with EDTA.

(Multiple Choice)

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Question 13

Which statement is NOT true for auxiliary complexing agents?

(Multiple Choice)

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Question 14

A metal that does not freely dissociate from an indicator is said to____________________ the indicator.

(Multiple Choice)

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Question 15

Calculate pBa when 35.00 mL of 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba²⁺ in the presence of 0.1 M nitrilotriacetate. = 1.48 × 10⁻⁴. = 0.30 for pH 10.K_f = 7.59 × 10⁷ for BaY²⁻.

(Multiple Choice)

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Question 16

For EDTA titrations the titration reaction is Mⁿ⁺ + EDTA ⇋ MY^n-4.Which statements are true for EDTA titration curves? I At the equivalence point,there is exactly as much EDTA in solution as metal.[Mⁿ⁺] is calculated from the dissociation of MY^n-4 formed. II After the equivalence point,the concentration free EDTA equals excess EDTA and virtually all metal ion is in the form MY^n-4.[Mⁿ⁺] is calculated from the dissociation of MY^n-4. III Before the equivalence point,free [Mⁿ⁺] equals excess unreacted Mⁿ⁺ after EDTA has been consumed.Dissociation of MY^n-4 is negligible. IV pM is plotted on the y-axis and milliliters EDTA solution added on the x-axis.

(Multiple Choice)

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Question 17

Which statement is incorrect for conditional formation constants,K_f^′?

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Question 18

Ammonia,0.10 M,is used as an auxiliary complexing agent for a Co²⁺ titration with EDTA.There are 6 s for the complex between ammonia and Co²⁺.Which equation is used to calculate ?

(Multiple Choice)

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Question 19

Calculate pBa when 50.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba²⁺.For the buffered pH of 10, = 0.30.K_f = 7.59 × 10⁷ for BaY²⁻.

(Multiple Choice)

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Question 20

Showing 1 - 20 of 20

Exam 13: Edta Titrations

Which is NOT an end point detection method used with EDTA titrations?

A____________________ titration is necessary for analytes that precipitates in the absence of EDTA,that reacts slowly with EDTA or that blocks the indicator.

Calculate pBa when 35.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba2+.For the buffered pH of 10, = 0.30.Kf = 7.59 × 107 for BaY2−.

Calculate [Mn2+] when 50.00 mL of 0.1000 M Mn2+ is titrated with 17.00 mL of 0.2000 M EDTA.The titration is buffered to pH 11 for which = 0.81.Kf = 7.76 × 1013

Which statement is NOT true?

Calculate for a 0.2 M EDTA solution buffered at pH 10.00.For EDTA K1 = 1.0,K2 = 31.6,K3 = 100,K4 = 490,K5 = 1.35 × 106 and K6 = 2.34 × 1010.

Calculate [Ba2+] when 35.00 mL of 0.2000 M EDTA is added to 50.00 mL of 0.1000 M Ba2+ in the presence of 0.1 M nitrilotriacetate. = 1.48 x 10−4. = 0.30 for pH 10.Kf = 7.59 × 107 for BaY2−.

The reaction between Al3+ and EDTA is too slow for direct titration.To a 25.00 mL Al3+ sample 50.00 mL of 0.2000 M EDTA is added and allowed to react for 30 minutes.The excess EDTA was titrated with 21.23 mL of 0.1000 M Zn2+.What is the concentration of Al3+ in the sample?

Calculate pBa when 75.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba2+.For the buffered pH of 10, = 0.30.Kf = 7.59 × 107 for BaY2−.

Calculate [Mn2+] when 50.00 mL of 0.1000 M Mn2+ is titrated with 25.00 mL of 0.2000 M EDTA.The titration is buffered to pH 11 for which = 0.81.Kf = 7.76 × 1013

The____________________ is the ability of multidentate ligands to form more stable metal complexes than those formed by similar monodentate ligands.

A____________________ is a reagent that protects a component of the analyte from reaction with EDTA.

Which statement is NOT true for auxiliary complexing agents?

A metal that does not freely dissociate from an indicator is said to____________________ the indicator.

Calculate pBa when 35.00 mL of 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba2+ in the presence of 0.1 M nitrilotriacetate. = 1.48 × 10−4. = 0.30 for pH 10.Kf = 7.59 × 107 for BaY2−.

Which statement is incorrect for conditional formation constants,Kf′?

Ammonia,0.10 M,is used as an auxiliary complexing agent for a Co2+ titration with EDTA.There are 6 s for the complex between ammonia and Co2+.Which equation is used to calculate ?

Calculate pBa when 50.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba2+.For the buffered pH of 10, = 0.30.Kf = 7.59 × 107 for BaY2−.

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Let the Titrations Begin

Activity and the Systematic Treatment of Equilibrium

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Advanced Topics in Equilibrium

Fundamentals of Electrochemistry

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Calculate pBa when 35.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba²⁺.For the buffered pH of 10, = 0.30.K_f = 7.59 × 10⁷ for BaY²⁻.

Calculate [Mn²⁺] when 50.00 mL of 0.1000 M Mn²⁺ is titrated with 17.00 mL of 0.2000 M EDTA.The titration is buffered to pH 11 for which = 0.81.K_f = 7.76 × 10¹³

Calculate for a 0.2 M EDTA solution buffered at pH 10.00.For EDTA K₁ = 1.0,K₂ = 31.6,K₃ = 100,K₄ = 490,K₅ = 1.35 × 10⁶ and K₆ = 2.34 × 10¹⁰.

Calculate [Ba²⁺] when 35.00 mL of 0.2000 M EDTA is added to 50.00 mL of 0.1000 M Ba²⁺ in the presence of 0.1 M nitrilotriacetate. = 1.48 x 10⁻⁴. = 0.30 for pH 10.K_f = 7.59 × 10⁷ for BaY²⁻.

The reaction between Al³⁺ and EDTA is too slow for direct titration.To a 25.00 mL Al³⁺ sample 50.00 mL of 0.2000 M EDTA is added and allowed to react for 30 minutes.The excess EDTA was titrated with 21.23 mL of 0.1000 M Zn²⁺.What is the concentration of Al³⁺ in the sample?

Calculate pBa when 75.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba²⁺.For the buffered pH of 10, = 0.30.K_f = 7.59 × 10⁷ for BaY²⁻.

Calculate [Mn²⁺] when 50.00 mL of 0.1000 M Mn²⁺ is titrated with 25.00 mL of 0.2000 M EDTA.The titration is buffered to pH 11 for which = 0.81.K_f = 7.76 × 10¹³

Calculate pBa when 35.00 mL of 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba²⁺ in the presence of 0.1 M nitrilotriacetate. = 1.48 × 10⁻⁴. = 0.30 for pH 10.K_f = 7.59 × 10⁷ for BaY²⁻.

Which statement is incorrect for conditional formation constants,K_f^′?

Ammonia,0.10 M,is used as an auxiliary complexing agent for a Co²⁺ titration with EDTA.There are 6 s for the complex between ammonia and Co²⁺.Which equation is used to calculate ?

Calculate pBa when 50.00 mL 0.1 M EDTA is added to 50.00 mL of 0.1 M Ba²⁺.For the buffered pH of 10, = 0.30.K_f = 7.59 × 10⁷ for BaY²⁻.