In a solution kept constant by buffering to pH= 8.0, 50.0 mL of 0.0050M Ni2+ is 0,0100 In titration with M EDTA, find the pNi against the following EDTA volumes. (at pH =8.0 a4 5.4x10-3) a) 0.00 mL, b) 10.0 mL, In additions of 30.00 mL EDTA

In a solution kept constant by buffering to pH= 8.0, 50.0 mL of 0.0050M Ni2+ is 0,0100 In titration with M EDTA, find the pNi against the following EDTA volumes. (at pH =8.0 a4 5.4x10-3) a) 0.00 mL, b) 10.0 mL, In additions of 30.00 mL EDTA

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter14: Applications Of Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 14.6QAP: The accompanying data (1.00-cm cells) were obtained for the spectrophotometric titration 10.00 mL of...

See similar textbooks

Related questions

Q: If 200 ml of 0.01 M EDTA is added to 100 ml of 0.01 M Ni solution that is buffered at PH of 10.2,…

Q: A 140.0 mL sample of 0.070 M Ca²+ is titrated with 0.070 M EDTA at pH 9.00. The value of log Kf for…

A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: Consider the titration of 25.0 mL of 0.020 0 M MnSO4 with 0.010 0 M EDTA in a solution buffered to…

Q: A 50.00-mL aliquot of solution containing 0.358 of MgSO4 (FM 120.37) in 0.500 L required 38.08 mL of…

A: Solution - According to the question - Given - Total Moles of Mg2+ = moles of MgSO4 = mass/molar…

Q: For the titration of 50.00 mL of 0.000226 M Ba²* with 0.100 M EDTA at pH 10.00, ay = 0.30, and Kf =…

Q: A 50.00 ml aliquot solution containing 0.524 g of magnesium sulfate (FW 120.37 in 0.500 L required…

A: Given that - Volume of magnesium sulfate = 50.00 mL Mass of magnesium sulfate in 0.500 L Solution…

Q: (b) 50 mL of 0.005 M Pb2* solution buffered at pH 10 is to be titrated with 0.01 M EDTA solution.…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: 25.00 mL 0.01000 M Ni2+ is titrated with 0.01000 M EDTA in a solution buffered topH 5.0. Given that…

A: The formation constant can be described as the constant that is used to establish the relation…

Q: 150.0 mL sample of 0.080 M Ca is titrated with 0.080 M EDTA at pH 9.00. The value of log K for the…

Q: The Cr plating on a surface that measured 3.00 cm x 4.00 cm was dissolved in HCl. The pH was…

A: Given : molarity of EDTA : 0.01441M Volume of EDTA = 10.19mL Total amount of EDTA or milimole of…

Q: The Cr plating on a surface that measured 3.00 cm x 4.00 cm was dissolved in HCI. The pH was…

Q: An unknown solution containing 25.00 mL of Ni2* in dilute HCI is treated with a known excess of…

A: Introduction : This question is basically based on back titration concept . Given : Molarity of…

Q: (a) Sketch a titration curve for a 50.0 mL of 0.01M Sr2+ solution, buffered at pH 11 when 0.0,10.0,…

A: Answer is explained below.

Q: A 60.00 mL of buffered solution (pH 10) containing Zn2* and Ni2* ions (from a chip sample) is…

A: Metal ion combine with EDTA in 1 : 1 mole ratio. So we would calculate moles of both metal ions…

Q: 25.00 mL 0.01000 M Ni2+ is titrated with 0.01000 M EDTA in a solution buffered topH 5.0. Given that…

Q: 0.5 mg sample required 20.5 ml. EDTA for titration. The EDTA was standardized by titrating 25 ml. of…

A: The question is based on the concept of complexometric titration. we have to analyse the alumina…

Q: 2+ Calculate the mass of Cu (At.wt. 63) that titrated iodometrically with I ,then the liberated I,…

A: Molarity = no. of moles/ vol (Lt)

Q: What is the value of pMg for 50.0 ml of a 0.0500 M Mg*2 solution buffered at pH 10.00 and titrated…

A: Question is based on the concept of quantitative analysis. We have to calculate P value of magnesium…

Q: A 50.00-mL aliquot of solution containing 0.395 of MgSO4 (FM 120.37) in 0.500 L required 39.55 mL of…

Q: A 25.00 mL sample containing Fe3+ was treated with 10.00 mL of 0.03676 M EDTA to complex all the…

A: A 25.00 mL sample containing Fe3+ was treated with 10.00 mL of 0.03676 M EDTA to complex all the…

Q: To check the hardness of tap water by complexometric titration 50 mL of water sample is required for…

Q: A 100, 0mL containing Zn^ 2+ was treated with 50.0 of 0.0500 M EDTA complex all the Zn^ 2+ and leave…

A: We have given that 100mL containing Zn2+ was treated with 50.0ml of 0.0500 M EDTA complex excess…

Q: Cd²+ forms a stable complex with EDTA. Consider the titration of 30.00 ml of 0.0525 M Cd with 0.125…

A: Titration of 30.00 mL of 0.0525 M Cd with 0.125 M EDTA solution at pH 9We have to calculate the…

Q: In the titration of 50.0 ml of 0.005 M Ca2+ with 0.01 M EDTA ,at pH 10 find the pCa at equivalence…

A: Given, Volume of Ca2+ = 50.0 mLMolarity of Ca2+ = 0.005 MMolarity of EDTA = 0.01 MpH = 10KCaY=…

Q: O What is the pM in a titration of 16.0 mL of 0.05 M Ca2+ with 0.05 M EDTA if the titration buffered…

Q: a. A 40.0 mL sample containing 0.0400 M Ni" was titrated with 0.0400 M EDTA at pH 11.0. Given pkyy…

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A 35.0 mL sample of 0.0200 M Cu2+ buffered at pH 8.00 is titrated with 0.0100 M EDTA. Calculate…

A: It's a multiple part question. Given information, Volume of EDTA (V1) = ? Concentration of EDTA…

Q: A 50.0 mL aliquot of solution contairing 0.450 g of MgSO4 (FM 120.37) in 0.500L required 37.6 mL of…

A: EDTA titration :- It is a complexometric titrations . EDTA is short form of…

Q: A sample is analyzed for chloride by the Volhard method. Calculate the %KCl from the following data:…

A: Calculation of no. of mol of AgNO3: n=Molarity×Volume=0.1157 mol/L×35.00×10-3 L=4.0495×10-3 mol…

Q: An EDTA solution was allowed to react with Pb²⁺ to produce 0.25 M PbY²⁻, 2.67×10⁻⁸ M Pb²⁺ and an…

A: The reaction is: Pb2++EDTA⇔PbY2-

Q: Q2: Consider the titration of 30.C ml of 0.015 0 M MnSO with 0.010 0 M EDTA in a salution butfered…

A: To solve the titration curve, we first need to calculate the conditional formation constant of the…

Q: 3. A solution contains 1.694 mg of CoSo. (155.0 g/mol) per milliliter. a. Calculate the volume of…

A: a) Amount of CoSO4 = 1.694 mg/mL Calculation of mass of CoSO4: Mass=1.694 mg mL-1×25 mL=42.35 mg…

Q: A cyanide solution with a volume of 12.99 ml was treated with 30.00 mL. of Ni solution (containing…

Q: Use a spreadsheet and construct curves for the follow- ing titrations. Calculate potentials after…

A: Solution a) Half-cell reactions involved are:

Q: A cyanide solution with a volume of 13.87 mL was treated with 24.00 mL of Ni+ solution (containing…

A: Concentration of CN- can be determined from the amount of Ni2+ used in the titration of CN-.

Q: Cd2* forms a stable complex with EDTA. Consider the titration of 30.00 mL of 0.0525 M Cd" with 0.125…

A: The reaction between Cd2+ and EDTA takes place in the following way :Cd2+ + EDTA →…

Q: using a buffer at pH 3.0, calculate the concentration of Ni2+ in a solution that was prepared by…

A: i)

Q: Triplicate samples of NaOH was found to have concentrations of 0.1444 M (Trial 1), 0.1107 M (Trial…

A: Introduction : Titration can be defined as the technique where a solution of known concentration is…

Q: What is the value of pMg for 50.0 ml of a 0.0500 M Mg*2 solution buffered at pH 10.00 and titrated…

A: In the given question we have to calculate the pMg value of the given titration Reaction. Given…

Q: How do I find Moles of EDTA required for a complexometric titration of Magnesium if I have the…

A: Molarity is defined as “the number of moles of solute present in per litre of solution”. It is…

Q: chip sample) is analyzed using EDTA titration with EBT as indicator. The following data were…

Q: Cd2* forms a stabie complex with EDTA. Consider the titration of 30.00 ml of 0.0525M Ca with 0125 M…

A: The reaction that takes place is: Cd2+ + EDTA → [CdEDTA]2− 30.00 mL of 0.0525 M Cd2+ reacts with…

Q: What is the value of pMg for 50.0 ml of a 0.0500 M Mg2 solution buffered at pH 10.00 and titrated…

A: The question is based on the concept of complexometric titration. We have to calculate P value of…

Q: Given the following data during the potentiometric titration of 75.00 mL unknown NaCl solution by…

Q: You are asked to titrate a Mn3+ solution with EDTA at pH 9.00. The overall ionic strength of the…

A: Solution- Log k = 25.2k =1025.2 nowαEDTA4−=5.4 ×10−2×1025.2 at pH=9(a) k'(conditional formation…

Q: To a 50.00-mL aqueous solution containing Pb2+ is added a total amount of 5.000 mmol EDTA. The pH…

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

Q: Question attached

Q: A 15.0 mL sample of 0.0100 M Cu²+ buffered at pH 9.00 is titrated with 0.0300 M EDTA. Calculate…

A: Given: Volume of Cu2+ = 15.00 mL Concentration of Cu2+ = 0.0100 M pH=9.00 To Calculate pCu2+ for…

Question

In a solution kept constant by buffering to pH= 8.0, 50.0 mL of 0.0050 M Ni2+ is 0,0100
In titration with M EDTA, find the pNi against the following EDTA volumes. (at pH =8.0
a4 = 5.4x10-3)
a) 0.00 mL,
b) 10.0 mL,
C) In additions of 30.00 mL EDTA

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step by step

Solved in 4 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The accompanying data (1.00-cm cells) were obtained for the spectrophotometric titration 10.00 mL of Pd(II) with 2.44 10-4 M Nitroso R(O. W Rollins and M. M. Oldham, Anal. chem .,1971, 43, 262, DOI: 10.1021/ac60297a026). Calculate the concentration of the Pd(II) solution, given that the ligand-to-cation ratio in the colored product is 2:1
c. An EDTA solution is standardized against high-purity CaCO3 by dissolving 0.3982 g CaCO3 in hydrochloric acid, adjusting the pH to 10 with ammoniacal buffer, and titrating. If 38.26 mL was required for the titration, calculate the molarity of the EDTA. (Molecular weight EDTA = 292.24 g mol-1)
A 60.00 mL of buffered solution (pH 10) containing Zn and Nit ions (from a chip sample) is analyzed using EDTA titration with EBT as indicator. The following data were recorded: M of EDTA = 0.05204 V of EDTA for Zn2+ =D41.97 V of EDTA for Ni2+ mL = 15.16 mL How many mmoles of Zn and Ni were present in the solution? If the weight of the chip is 1.000 g, give the % Zn and % Ni in the original sample.
To a 50.00-mL aqueous solution containing Pb2+ is added a total amount of 5.000 mmol EDTA. The pH is made alkaline, and the excess EDTA is back-titrated with 0.0100 M Mg2+, requiring 15.2 mL. Calculate the molar concentration of Pb in the sample. A.0.100 M B. 0.0970 M C. 0.0486 M D. 2.94 x 10-3 M
A foot powder sample containing Zn was dissolved on 50.00 mL water and was titrated to the end point color with 22.57 mL of 0.01639 M EDTA at pH=4. (α= 3.61x109, KKzny2 = 3.2 x 1016). The pZn in the sample is:
You are asked to titrate a Mn3+ solution with EDTA at pH 9.00. The overall ionic strength of the solution is 0.10 M. Mn3+ +EDTA4- ⇌ MnEDTA- log K = 25.2 a. Calculate the conditional formation constant for MnEDTA- at pH 9.00 b. Calculate the equilibrium [Mn3+] at pH 9.00 for total Mn3+ = 2.0 mM i) total EDTA = 0.50 mM ii) total EDTA = 5.00 mM
A 50.00-mL aliquot of solution containing 0.358 of MgSO4 (FM 120.37) in 0.500 L required 38.08 mL of EDTA solution for titration. How many milligrams of CaCO3 (FM 100.09) will react with 1.00 mL of this EDTA solution?
b. EDTA cannot be used as a primary standard always. When can EDTA be used as a primarystandard ? Give reason why EDTA is used in complexometric titrations.
1. How much volume (mL) is needed to standardize 0.05M of EDTA using 180mg of magnesium ribbon? MW: 24g/mol2. How many grams of EDTA is required to prepare 250mL of a 0.05M solution? MW: 292g/mol3. What is the Molarity of the EDTA solution if 35mL of the titrant was added to 0.2g of calcium carbonate? Round off to four decimal places
A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient dryness and quantitatively transferred to a 250 mL volumetric flask, and diluted to mark. A 10 mL of aliquot was then transferred to an Erlenmeyer flask, together with 5mL buffer and 5 drops of EBT indicator, and was used to standardize the EDTA titrant. The solution turned blue after the addition of 24.10 mL of EDTA. A blank correction was performed and was determined to be 0.4 mL. What is the concentration of EDTA obtained (MW CaCO3 = 100.0869 g/mol)?
C1. A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible. What is the molar concentration of the standardized EDTA solution? (use C1 as reference)* 0.08m 0.8M 0.08N 0.08M How many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?* 0.1825 0.1852 1.825 1.1852
Calculate the pZn2+ for solutions prepared by adding 0.00, 5.00, 10.00, 15.00, 20.00, 25.00 and 30.00 mL of 0.0100 M EDTA to 25.00 mL of 0.00250 M Zn2+. Assume that both the Zn2+ and EDTA are 0.0100 M in NH3 to provide a constant pH of 9.0