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 with 0.0500 m EDTA when 50.0 mL of EDTA is added (Kf = 6.2x108)(ay4. = 0.30 )? 1. O5.77 2. O2.88 3. 4.94 4. 1.39 5. 07.96
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,…
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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…
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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 =…
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Q: 3. An EDTA solution is standardized against high purity CaCO3 by dissolving 0.3982 g CaCO3 in…
A: Given data,Mass of CaCO3=0.3982gVolume of EDTA=38.26mLpH=10.0
Q: A 49.10 mL aliquot from a 0.500 L solution that contains 0.530 g of MnSO4 (MW=151.00 g/mol) required…
A: Solution -
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 50.00 mL solution containing Ni2+ and Fe2+ was treated EDTA to bind all the metal ions. After…
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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…
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Q: What is the value of pMg for 50.0 ml of a 0.0500 M Mg solution buffered at pH 10.00 and titrated…
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Q: A 10.0 mL of 0.02M MgCl2 solution is titrated with 0.02 M EDTA. If the conditional constant K4 is 1…
A: The complexation reaction between Mg2+ ions and EDTA ions can be summed as: Mg2++EDTA2-=[Mg-EDTA]…
Q: 11) What is the pM in a titration of 20.0 mL of 0.05 M Ca2 with 0.05 M EDTA if the titration is…
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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: An EDTA solution is standardized against high-purity CaCO3 by dissolving 0.3982 g CaCO3 in…
A: Given, CaCO3=0.3982 g Volume of EDTA =38.26 mL molecular weight of EDTA= 292.24 g/mol
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 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: In order to titrate EDTA into a water sample of unknown water hardness, the EDTA of known…
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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: Balanced equilibrium for the reaction of EDTA(Y4-) with Pb2+ is: Pb2+(aq) + Y4-(aq) ⇌ PbY2-(aq) ;…
Q: A 120.0 mL sample of 0.040 M Ca²+ is titrated with 0.040 M EDTA at pH 9.00. The value of log Kf for…
A: COMPEXOMETRIC TITRATION Complexometric titration reactions are those reactions in which coloured…
Q: A water was tested for water hardness. A 50.00 mL aliquot was prepared and buffered to pH 10.0, it…
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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 pZn2+ for solutions prepared by adding 0.00, 5.00, 10.00, 15.00, 20.00, 25.00 and…
A: The concentration of Zn2+ can be determined as: M1V1(Zn2+)=M2V2(EDTA) pZn2+ can be determined by:…
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…
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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: What will be the equilibrium concentration of Cu²+ if a 50.0 mL of 0.0400 M EDTA was added to 20.0…
A: The solution is given below:
Q: Calculate the concentration of Ni²+ and pNi in a solution that was prepared by mixing 50.0 mL of…
A: Solution: We have to calculate the unknown concentration of Ni2+
Q: 02) Consider the titration of 20.00mL of a Ca2+0.0250mol/L solution with 0.0500mol/L EDTA. The Ca2+…
A: 2)given, initially the volume of Ca2+ = 20.00 mL concentration of Ca2+ = 0.0250 mol/L concentration…
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: Calculate a titration curve for 10.0 mL of 1.00 mM Ca?* with 1.0 mM EDTA at pH 9.0.
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
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: 11. A solution of 0.0500M Ca²* and 0.00500M Mg* was titrated against EDTA at pH = 10 (K'r for CaY2…
A: EDTA is ethylenediaminetetraacetic acid which is an indicator. It has 2 amino and 4 carboxyl groups.…
Q: A 1.509-g samle of a Pb/Cd alloy was dissolved in acid and diluted to exactly 250.0 mL in a…
A: The explanation is given below-
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: 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: The Telluride ion was determined by indirect titration with EDTA. To a solution conta 50.00 mL of…
A: Given Concentration of Zn(ClO4)2= 0.08664 M Given Telluride Solutions = 50 ml We have to calculate…
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: The question is based on the concept of equilibrium . we have to calculate P value of magnesium ion…
Q: chip sample) is analyzed using EDTA titration with EBT as indicator. The following data were…
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Q: In a solution kept constant by buffering to pH= 8.0, 50.0 mL of 0.0050M Ni2+ is 0,0100 In titration…
A: The question is based on the concept of complexometric titrations. We have to calculate pNi at…
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: Calculate pMn² when 50.00 mL of 0,100 0 M Mn² is titrated with 25.00 mL of 0.200 0 M EDTA. The…
A: Given: 50.00 mL of 0.1000 M Mn2+ is titrated with 25.00 mL of 0.2000 M EDTA Kf = 7.76 × 1013 α =…
Q: In the titration of MgSO4.2H2O (2g per litre) against a 0.01 M solution of the disodium salt of…
A: Given 0.01 M solution of EDTA the reaction involving titration of MgSO4.2H2O and EDTA can be…
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: Calculate the pCa for the titration of 100 ml of 0.050 M Ca²+ at pH = 8 with 0.1 M EDTA After…
A: The balanced equation for the reaction of Ca2+(aq) and EDTA, Y4-(aq) is: Ca2+(aq) + Y4-(aq) ⇌…
Q: An unknown solution containing 25.00 mL of Ni2+ in dilute HCl is treated with a known excess of…
A: Given, Ni2+=25.0 mLEDTA= 25.0 mLConcentration of EDTA =0.05382 MZn2+=0.02299 MVolume= 17.0 mL
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- A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0474 M EDTA. The endpoint volume was 40.99 ml. A second aliquot of the same mixture was made strongly basic by the addition of NaOH – this causes the Mg2+ to precipitate as Mg(OH)2. The solution was then titrated with the 0.0474 M EDTA and the endpoint volume was found to be 30.04 ml.(a) Sketch a titration curve for a 50.0 mL of 0.01M Sr2+ solution, buffered at pH 11 when 0.0,10.0, 24.0, 25.0, 26.0, 30.0, and 40.0 mL of 0.02 M EDTA are added. Given the KSrY2- is 4.3X108 and α4 is 0.85.A solution containing Mg2+ was buffered to pH 9.81 and titrated with EDTA. Eriochrome black T, with p?a1 = 6.3 and p?a2 = 11.6 was used as the indicator. It is a diprotic acid, H2E What is the fraction of the predominant form of eriochrome black T in solution at this pH? (To answer this, report the alpha fraction of the indicator’s most prevalent species at this pH)
- A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0493 M EDTA. The endpoint volume was 42.15 ml. A second aliquot of the same mixture was made strongly basic by the addition of NaOH – this causes the Mg2+ to precipitate as Mg(OH)2. The solution was then titrated with the 0.0493 M EDTA and the endpoint volume was found to be 35.65 ml. Calculate the molar concentration of MgConsider the titration of 25.0mL 0.020M of Co(NO3)2 with .0100M EDTA in a solution buffered to pH 10.00. Calculate pCo^2+ at the following volumes of added EDTA. a. 0.0 mL b. 20.0 mL c. 40.0 mL d. 49.0 mL e. 50.0 mL f. 50.1 mL g. 55.0 mL h. 60.0 mLChromel is an alloy composed of nickel, iron and chromium. A 0.6553-g sample was dissolved and diluted to 250.0 mL. When a 50.00-mL aliquot of 0.05173 M EDTA was mixed with an equal volume of the diluted sample, all three ions were chelated, and a 5.34-mL back titration with 0.06139 M copper (II) was required.The chromium in a second 50.0-mL aliquot was masked through the addition of hexamethylenetetramine; titration of the Fe and Ni required 36.98 mL of 0.05173M EDTA. Iron and chromium were masked with pyrophosphate in a third 50.00-mL aliquot, and the nickel was titrated with 24.53 mL of the EDTA solution. Calculate the percentage of Cr in the alloy. Express your answer in 2 decimal places.
- For the complexiometric titration of Ca2 + ions in the shell of the egg sample weighing 62,576 g, the necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL of the prepared sample was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The prepared solution was titrated with 23.6 mL of 0.0095 M EDTA solution. What is the value of the amount of calcium in the sample in terms of% CaCO3? (Ca: 40, C: 12, O: 16 g / mol)25.0 mL of an unknown Ni2+ solution was treated with 25.00 mL of 0.05283 M Na2EDTA. The pH of the solution was buffered to 5.5 and then back-titrated with 17.61 mL of 0.02299 M Zn2+. What was the unknown Ni2+ M?A 25.0025.00 mL solution of 0.088300.08830 M NaINaI is titrated with 0.051500.05150 M AgNO3AgNO3. Calculate pAg+pAg+ following the addition of the given volumes of AgNO3AgNO3. The KspKsp of AgIAgI is 8.3×10−178.3×10−17. 37.40 mLpAg+=37.40 mLpAg+= VepAg+=VepAg+= 47.30 mLpAg+=47.30 mLpAg+=
- A 0.2431 g sample of CaCO3 is dissolved in 6 M HCl and the resulting solution is diluted to 250.0 mL in a volumetric flask. Titration of a 25.00 mL sample of the solution requires 28.55 mL of EDTA to reach the Eriochrome Black T endpoint. A blank containing the same amount of Mg2+ requires 2.60 mL of EDTA. What is the molarity of the EDTA solution?A 2.02.0 mL aliquot of 0.001 M NaSCNNaSCN is diluted to 30.030.0 mL with 0.2 M Fe(NO3)3Fe(NO3)3 and 0.1 M HNO3.HNO3. How many moles of SCN−SCN− are present? If all the SCN−SCN− is complexed with Fe3+Fe3+ to form FeSCN2+,FeSCN2+, what is the molar concentration of FeSCN2+?If a water has a carbonate alkalinity of 120.00 mg/L as the ion and a pH of 10.30, what is the bicarbonate alkalinity in mg/L as the ion? The answer is HCO_3=130.686 or 130.7 mg/LPlease do explain the steps