The equivalence point is reached when 25.00 mL of 0.100 M EDTA is titrated with 25.00 mL of 0.100 M Mg²⁺. Calculate the pMg²⁺ if the titration is buffered to pH 10.00, α_Y⁴⁻ = 0.30 at that pH, and K_f = 10^8.79 for the MgY²⁻ complex.Options:- ( ) 1.00- ( ) 5.05- ( ) 7.69- ( ) 5.43- ( ) 9.57

Answered: Image /qna-images/answer/9544764e-44fb-48b0-88af-c7039ee8ed45.jpg

The equivalence point is reached when 25.00 mL of 0.100 M EDTA is titrated with 25.00 mL of 0.100 M Mg2*. Calculate the pMg2* if the titration is buffered to pH 10.00, ayt = 0.30 at that pH, and Kf = 108.79 for the MgY2- complex. O 1.00 5.05 O 7.69 O 5.43 O 9.57

The equivalence point is reached when 25.00 mL of 0.100 M EDTA is titrated with 25.00 mL of 0.100 M Mg2. Calculate the pMg2 if the titration is buffered to pH 10.00, ayt = 0.30 at that pH, and Kf = 108.79 for the MgY2- complex. O 1.00 5.05 O 7.69 O 5.43 O 9.57

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

Related questions

Q: 13. A sample contained Cr(III) species. A 25.00 mL portion of this sample is combined with 10.00 mL…

A: Given data : Volume of Cr(III) sample = 25.0 mL = 25×10-3 L Concentration of CDTA = 0.0875 M Volume…

Q: What is the concentration of NH3 needed to form a soluble complex with 0.001 M AGB (Ksp = 5.0 x…

Q: Calculate the equilibrium concentration of Zn2 + in a solution that was prepared by mixing 75.0 mL…

A: Zinc is determined by EDTA titration in almost the same way magnesium is - in the pH 10 against…

Q: 5.00 mL of 7.00 x 10¯³ M Fe(NO3)3 (7.00 times 10 to the minus 3rd power MFe (NO3)3) is added to 7.00…

A: Molarity of Fe3+ ions = 7.00 × 10-3 M Total Volume = 5 + 7 + 5 = 17 ml = 0.017 L

Q: [CLO-6] Calculate the pMg in the reaction of 50 mL of 0.1 M Mg2* (buffered to plH 10) with 25.5 ml…

Q: A 25.00 mL mixture of 0.01000 M Fe(CN)6 4– and 0.01000 M Sn2+ is titrated with 0.01000 M Ce4+ .…

A: The oxidation half reaction for the reaction of Fe(CN)64- with Ce4+ can be written as, Fe(CN)64- +…

Q: A. A solution is prepared by adding 0.05 M CaF2, 0.10 M NaF and 0.10 M9F2 to water. If all of these…

A: Hello. Since your question has multiple parts, we will solve the first question for you. If you want…

Q: The titration of Zn+2 and EDTA is carried out in the same manner as the Mg+2-EDTA titration. In this…

A: It is explained as given below :

Q: Demonstrate that Cu2+ can be titrated by EDTA in the presence of [CH3COO-] = 0.17 M and pH 9.5. b.…

A: The objective of this question is to show the concentration of Cu2+ ions in a sample using EDTA…

Q: Using the graph given, which metal can be titrated better with EDTA and why? Fe3+ Fe2+ Ca2+ Hg2+

A: This is a method of quantitative estimation of concentration of unknown solution by titrating it…

Q: The higher the ammonia concentration, the less sharper the end point for the EDTA-Zn²+ complex.

A: No. Of moles of KOH in 26.66ml of 0.15M KOH = (0.15/1000)*26.66 =0.0039 mol No. Of moles of…

Q: 50.00 ml of a 0.0500 M Ni2+ solution, whose pH is adjusted to pH=11 and the solution is additionally…

A: The titration of 50.00 mL solution of 0.0500 M Ni2+ is carried out with 0.100 M EDTA solution while…

Q: A solution is prepared by mixed 50.0 mL of 0.0400 M Ni2+ with 50.00 mL of 0.0400 M EDTA. Calculate…

A: The objective of this question is to calculate the concentration of Ni2+ when a solution is prepared…

Q: Should the equivalent of 0.01 M AgBr [Ksp=5*10^-13] dissolve in 6 M NH3 [Kf for…

Q: 47.6 mL aliquot from a 0.5 L solution that contains 0.45g of MnSO4 (MW is 151 g/mol) required 41.9…

Q: Which of the following statements regarding complexometric titrations is incorrect ? OIn the pH…

A: Complexometric titration : It's a type of volumetric analysis in which the end point of the…

Q: Calculate the pZn value after the addition of 25 mL of titrant in the titration of 50 mL of 0.01 M…

Q: Equilibrium Concentration Fe[SCN]?* Vol of Fe* Vol of SCN- 0.05 M HNO, (mL) (mL) (mL) 10.00 0.00…

A: The molarity of Fe(NO3)3 solution is 0.200 M. The molarity of NaSCN solution is 0.002 M.

Q: 4. A 50.0 mL solution of 0.100 M Zr** is buffered to pH=5 and titrated with 0.150 M EDTA. a. EDTA…

A: This is a method of quantitative estimation of concentration of unknown solution by titrating it…

Q: 8.00 mL of 6.00 x 10-3 M Fe(NO3)3 (6.00 times 10 to the minus 3rd power M Fe (NO3)3) is added to…

A: Given that : Given that :Initial volume of Fe(NO3)3 = 8.00 mLMolarity of Fe(NO3)3 =…

Q: At what pH does EDTA become a strong complexing agent? * 04 06 8 10 Which best describes the…

A: Ethylenediaminetetraacetic acid (EDTA) is a metal-chelating agent and binds metals such as chromium,…

Q: Consider the titration of 25.00 mL of 0.03555 M Co2+ by 0.02784 M EDTA at pH 10.00. Kf is 1045.…

A: The amount of EDTA required to reach the endpoint of the titration is determined as shown below.…

Q: Calculate the solubility of Ca3(PO4)2 (a) in pure water and (b) in a solution in which [PO4³-] 0.112…

Q: What are the molar solubilities of Cu(OH)2 [Ksp = 2.2e-20] and Pb(OH)2 [Ksp = 1.2e-15]?

A: Given: Cu(OH)2 and Pb(OH)2

Q: equivalent point, 25.00 mL of 0.10 M EDTA is required to titrate 50.00 mL of calcium in body fluid…

A: Calcium react with EDTA to form calcium EDTA complex in stoichiometry ratio of 1:1.

Q: Scientists conducted EDTA titration to check for water hardness, they used two 150 mL samples for…

A: Mg+2 + EDTA = Mg-EDTA Ca+2 + EDTA =…

Q: Determine the molar concentration of free Cu2+ in a solution prepared by combining 50.00 mL of…

A: When complex formation occurs between an analyte and titrant, the formation is measured with the…

Q: Which of the following statements regarding complexometric titrations is incorrect O The higher the…

A: Complexometric titrations: It is a kind of Volumetric analysis , where formation of colored complex…

Q: Which of the following statements regarding complexometric titrations is Incorrect O The higher the…

A: Complexometric titrations: It is a kind of Volumetric analysis , where formation of colored complex…

Q: 50.00 mL of 0.0524 M Pb(NO3)2 is titrated with 0.0419 M EDTA. The pH is buffered to 8.57. Find the…

A: At the equivalence point the initial moles of Pb2+ and the moles of EDTA added are equal. The total…

Q: vity/Student Guide Big Idea Assessments A certain brand of zinc cold medicine is marketed as…

A: The students know when the end point is achieved because the color of the solution changes.…

Q: 1.) A sample containing 0.175 g of Cl- is dissolved in 50 mL of deionized H20. The solution is…

A: Let us solve.

Q: 8. A 24-hr urine specimen was diluted to exactly 2.000 L. After buffering to pH 10.0, a 50.00 mL…

A: The objective of the question is to calculate the amount of calcium and magnesium ions.The titration…

Q: Calculate for the molar concentration of the Mg-EDTA complex during the titration of 48.0 ml of…

A: αY4- = 4.8*10-4 The balanced equation for the formation of Mg-EDTA complex is: Mg2+(aq) +…

Q: If a solution of 0.30 M Mn2 and 0.30 M Cd² is gradually made basic, what will the concentration of…

A: Answer: For a sparingly soluble compound, at the saturation point, reaction quotient becomes equal…

Q: Solid KSCN was added to a 2.93 M Co²+ solution so that it was also initially 2.93 M SCN¯. These ions…

A: Let us consider the volume of the solution is 1 L. Hence it contains initially 2.93 moles of Co2+…

Q: The formation constant for [Cu(CN)2]` is 1.0 × 1016, what is the value of the dissociation constant…

Q: What is the maximum concentration of Mg2+ that can exist in solution at pH 12 considering a…

A: The question is based on the concept of solubility product principle.It states that when a weak…

Q: A standard solution of EDTA (0.08 M) is being used to titrate 50 ml of a 0.04 M Ca 2+ solution.…

A: Q.1: Before the addition of EDTA solution, [Ca2+] = 0.04 M pCa2+ = - log[Ca2+] = - log(0.04) =…

Q: C. Sketch the photometric titration curve for the reaction of Fe (100 mL, colorless, 10 ppm) with…

A: Photometric Titration: This is a titration in which the absorbance of the solution is used to…

Question

The equivalence point is reached when 25.00 mL of 0.100 M EDTA is titrated with 25.00 mL of 0.100 M Mg²⁺.

Calculate the pMg²⁺ if the titration is buffered to pH 10.00, α_Y⁴⁻ = 0.30 at that pH, and K_f = 10^8.79 for the MgY²⁻ complex.

Options:
- ( ) 1.00
- ( ) 5.05
- ( ) 7.69
- ( ) 5.43
- ( ) 9.57

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Taking the Ksp of Zn(OH)2 as 4.0 x 10-3 and the Kf of [Zn(NH3)6] 2+ as 9.9 x 108 , determine how many moles of Zn(OH)2 can dissolve in 0.6 L of 1.2 M NH3.
11) Will a 0.15 M solution of NH3 be sufficient to keep Zn2+ from precipitating from a solution of 45.0 mL at a concentration of 1 mM before any EDTA is added if the solution is buffered to pH 11? Zn(OH)2 Zn(NH3)+ Zn(NH3)2* Zn(NH3);²* Zn(NH3)2* Ksp-6.0x10-16 (Bi=102.18) (B2=10443) (B3=10%.75) (Be=10%.70)
4. Calculate the molar solubility of MnS (Ksp 3.0 x 10-14) in a solution buffered to a pH of 5.00? (HS, Kar 9.6 x 10, Kar=1.3 x 10-¹4)
The % (w/w) I- in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of 0.05619 M AgNO3 and allowing the precipitate to form, the remaining silver was back-titrated with 0.05322 M KSCN, requiring 35.14 mL to reach the endpoint. Report the %(w/w) I- in the sample. [Ans. 17.76 % (w /w)]
3. Calculate the pZn of solutions prepared by adding 15.0, 25.0, and 35.0 mL of 0.100M EDTA to 50.0 mL of 0.00500M Zn²+ in 0.100M NH3 and 0.175M NH4Cl buffered to a pH of 9.0.
Spotify - 2Pa X2 www.shakes x * OWLV2 | Onli x + .com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [References] Cu2+ ions from copper(II) sulfate combine with Br ions from potassium bromide to form the yellow CuBra complex ion in the equilibrium shown below: (aq) + 4 Br" (aq)CuBr (aq) + 4 H,O (1) yellow Cu(H,O),+ blue When the blue diluted solution was heated, it turned yellow. This color change indicates that the are favored, K v with increased temperature, and the reaction is
A 130.0 mL sample of 0.060 M Ca²+ is titrated with 0.060 M EDTA at pH 9.00. The value of log Kf for the Ca²+ —EDTA complex is 10.65 and the fraction of free EDTA in the Y4- form, ay, is 0.041 at pH 9.00. What is K, the conditional formation constant, for Ca²+ at pH 9.00?
Kk.468.
What should be the pH of the environment for 50% of Ag+ ions to complex in the cyanide (CN¯) anion equivalent to a solution containing 10-3 M Ag+ ions? pKa for HCN = 9,3 ; logß2 for Ag(CN)2 - = 20,0 How can we INCREASE the complexity rate? Please help.
At 40.0 mL 0.0050 M Sr2 + pH 10, 0.0100 M EDTA is titrated. Calculate the pSr for the equivalence point. Kol(SrY) = 4,3x108 , α4 = 0,35
What should be the pH of the environment for 50% of Ag+ ions to complex in the cyanide (CN¯) anion equivalent to a solution containing 10-3 M Ag+ ions? pKa for HCN = 9,3 ; logß2 for Ag(CN)2 = 20,0 How can we INCREASE the complexity rate?
A 1.00 mL aliquot of a solution containing Cu and Ni is treated with 25.00 ml. of a 0.03468 M EDTA solution. The solution is then back titrated with 0.02308 M Zn+ solution at a pH of 5. A volume of 20.28 ml. of the Zn solution was needed to reach the xylenol orange end point. A 2.000 mL aliquot of the Cu* and Ni* solution is fed through an ion- exchange column that retains Ni?*. The Cu?+ that passed through the column is treated with 25.00 mL of 0.03468 M EDTA. This solution required 23.18 mL of 0.02308 M Zn* for back titration. The Ni extracted from the column was treated witn 25.00 mL of 0.03468 M EDTA. How many milliliters of 0.02308 M Zn+ is required for the back titration of the Ni solution? volume: ml.