An unknown solution containing 25.00 mL of Ni2* in dilute HCI is treated with a known excess of 25.00 mL of 0.05382 M EDTA solution. The solution turns yellow when a few drops of indicator are added. The excess unreacted EDTA back titrated with 0.02299 M Zn2*, which requires 17.00 mL to reach the red end point. What is the molarity of Ni2* in the unknown solution? (b)

An unknown solution containing 25.00 mL of Ni2* in dilute HCI is treated with a known excess of 25.00 mL of 0.05382 M EDTA solution. The solution turns yellow when a few drops of indicator are added. The excess unreacted EDTA back titrated with 0.02299 M Zn2, which requires 17.00 mL to reach the red end point. What is the molarity of Ni2 in the unknown solution? (b)

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: Potassium thiocyanate, KSCN, is often used to detect thepresence of Fe³⁺ ions in solution through…

Q: A 0.5745 g sample of an alloy containing principally bismuth and lead is dissolved in nitric acid…

Q: 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…

A: Initial moles of SCN- before dilution of the solution can be calculated using the molarity of NaSCN…

Q: Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution.…

A: Molar concentration is the measure of the concentration of a chemical species, in particular of a…

Q: Find the concentration of 50.0 ml of an acidified Fe2+ solution if 18.72ml of 0.01500M solution of…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: A 350.00 mL solution of 0.00265 M A3B4 is added to a 280.00 mL solution of 0.00205 M C3D2. What is…

A: Calculation of no. of mol of A3B4: No. of mol=Molarity×Volume=0.00265 mol/L×350.00×10-3…

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: titration of 50.00 mL of 0.1100 M Fe3+ with 0.07750 M Sn2+ is carried out. The analytical reaction…

Q: 3. A 100 mL sample of hard water is titrated with 22.4 mL of the EDTA solution from problem 2. The…

A: Volume of hard water sample = 100mL

Q: a. A 0.3108-g sample of primary-standard-grade Na2 C2O4 was dissolved in H2SO4 and titrated with…

Q: System #12: 0.10 Miron (III) chloride (source of Fe(H20),* complex) 3+ [FeCH20)6]* Kb of FelH20)s…

A: Given that : The concentration of [Fe(H2O)6]3+ = 0.10 M The reaction of [Fe(H2O)6]3+ with water is…

Q: (d). If the selling price of the milk powder is $0.67 for a box containing 12.8 ounces, what is the…

A: According to Q&A guidelines of Bartleby, we are supposed to answer only the first question out…

Q: Calculate the concentration of Fe2O3 in a mineral sample after solubilization of 0.4891g and…

A: from the reaction, 6 mole Fe2+ react with 1 mole K2Cr2O7. mole = mass molar mass

Q: 5(a) A sample containing 4.00 x 102 mmol of CuSO4 and 1.00 x 10-2 mmol of KNO3 is passed through a…

A: To solve problem 5(a) regarding the volume of 0.010 M NaOH needed to titrate the eluate from a…

Q: Use the data below to determine the % by mass of Fe to TWO decimal places, if a 0.021 M KMnO…

A: the correct answer is as follows:

Q: Calculate the M of the malonic in the sample.

A: 20 mL aliquot of malonic acid treated with 10 mL of 0.25 M Ce4+ Excess Ce4+ titrated with Fe2+…

Q: In what volume should iron fumarate (M=169.85g/mol) with a mass of 152.1mg be dissolved and what…

A: To determine the volume in which 152.1 mg of iron fumarate (molecular weight 169.85 g/mol) should be…

Q: You want to measure the concentration of carbonate (CO32-) in a mildly basic solution by using an…

A: The concentration and the number of moles of Ca2+ ion in the filtered solution is;…

Q: 0.0322 M EDTA solution is used as the titrant in the titration of a 50.00 mL solution that is 0.0129…

A: EDTA titration is a type of complexometric titration that uses ethylenediaminetetraacetic acid…

Question

(b)
An unknown solution containing 25.00 mL of Ni2+ in dilute HCI is treated with a known
excess of 25.00 mL of 0.05382 M EDTA solution. The solution turns yellow when a
few drops of indicator are added. The excess unreacted EDTA back titrated with
0.02299 M Zn²*, which requires 17.00 mL to reach the red end point. What is the
molarity of Ni2+ in the unknown solution?

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

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 1 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

To find the pH of a buffer composed of H₂PO4 (aq) and HPO2(aq), which pKą value should be used in the Henderson-Hasselbalch equation? PK₁3 = 12.32 PK₁2 = 7.21 OpKal = 2.16 Calculate the pH of a buffer solution obtained by dissolving 26.0 g of KH₂PO4(s) and 43.0 g of Na₂HPO4(s) in water and then diluting to 1.00 L. pH || = Incorrect
Use the data below to determine the % by mass of Fe to TWO decimal places, if a 0.02 M KMnO4 solution was used for the titration. gH * + MnO 4 + 5Fe 2+ -> SFe 3+ + Mn 2+ + 4H 20 (MM Fe = 56 a/moll mass of iron compound (g) 0.604 initial buret reading (mL) 0.94 Tinal buret reading (mL 16.21
Determine the molarity of the 10.00 mL standard EDTA solution titrated using 1.000 g zinc sulfate in 100 mL solution. (ZnSO4 = 161.47 g/mol ) 0.006193 M 0.6193 M 6.193 M 0.06193 M
A solution containing 60 mL of a 0.025 mol / L metal ion (Mn +) buffer buffered to pH 7.0 was titrated with a 0.05 mol / L EDTA solution. Data: Conditional formation constant (Kf)=10^15. Determine: i) The concentration of the free metal when ½ of the equivalence volume is added. ii) the concentration of free metal in the equivalence volume. iii) the concentration of free metal with an excess of 2 mL of EDTA? (Data - EDTA constants: K1=0.01; K2=2.19.10^-3; K3=6.92.10^-7; K4=5.75.10^-11)
A 25.00 mL unknown water sample is titrated with a standardized 0.0140 M EDTA solution. It is determined that 8.54 mL of EDTA is required to reach the end point. The blank titre was determined to be 1.50 mL. Determine the concentration of Calcium in the water sample in ppm. (mwt. of CaCO3 = 100.0892 g/mol).
A titration of 50.00 mL of 0.1100 M Fe3+ with 0.07750 M Sn2+ is carried out. The analytical reaction is 2Fe3+ + Sn2+ ⇋ 2Fe2+ + Sn4+ and Fe3+ + e− ⇋ Fe2+ E° = +0.732 V Sn4+ + 2e− ⇋ Sn2+ E° = +0.139 V What is the volume of Sn2+ is added at the equivalence point?
Titration of 30.00 mL of 0.02502 M Na2C2O4 required 34.75 mL of a potassiumpermanganate solution.2MnO -+ 5H C O + 6H+  2Mn2- + 10CO + 8H O4 2 2 4 2(g) 2Calculate the molar concentration of the KMnO4 solution