A 45.00 mL mixture containing 0.0746 M TI and 0.0746 M Hg* is titrated with 0.0839 M Nal resulting in the formationof the precipitates TII and Hg, L,. Calculate pl at the given points in the titration. The K values for TII and Hg, I, are5.54 x 10- and 2.9 x 10-29, respectively.62.2 ml. pl96.2 ml. pl=second equivalence point pl =125.0 mL pl =

First calculate the number of moles of Tl+ and Hg22+ present initially in the mixture of molarity…

A 45.00 mL mixture containing 0.0746 M TI and 0.0746 M Hg* is titrated with 0.0839 M Nal resulting in the formation of the precipitates TIl and Hg, L,. Calculate pl at the given points in the titration. The K, values for TIl and Hg,I, are 5.54 x 10* and 2.9 x 10-, respectively. 62.2 ml. pl= 96.2 ml. pl = second equivalence point pl = 125.0 ml pl =

A 45.00 mL mixture containing 0.0746 M TI and 0.0746 M Hg* is titrated with 0.0839 M Nal resulting in the formation of the precipitates TIl and Hg, L,. Calculate pl at the given points in the titration. The K, values for TIl and Hg,I, are 5.54 x 10* and 2.9 x 10-, respectively. 62.2 ml. pl= 96.2 ml. pl = second equivalence point pl = 125.0 ml pl =

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: In the determination of chloride by the Mob method, what will be the equiliblium concentration of…

A: The objective of the question is to determine the equilibrium concentration of silver ions in mg/L…

Q: Calculate the concentration of IO, in a 6.30 mM Pb(NO,), solution saturated with Pb(IO,),. The Ksp…

A: Here we have to determine the concentration of iodate ion if 6.3mM Pb(NO3)2 is saturated with…

Q: If 175ml of a 0.00550 M KCI solution is mixed with 145ml of a 0.00150M AgNO3 solution,will AgCl…

A: Given data,Molarity of KCl=0.00550MVolume of KCl=175mL=0.175LMolarity of AgNO3=0.00150MVolume of…

Q: What is the molar solubility of AgCl (Ksp = 1.80 x 10-10) in 0.890 M NH.? (Kf of Ag(NH.): is 1.7 x…

Q: Calculate the molar solubility of barium fluoride in: (a.) pure water (b.)0.10 M Ba(NO3)2 (c.)0.15…

A: Here We have to calculate the molar Solubility of barium fluoride in different solvents given…

Q: A solution contains 3.00 x 10-3 M of calcium ion. A concentrated sodium fluoride solution is added…

A: Answer: When Ionic product of a substance becomes equal to its solubility product, that's when…

Q: 2. Silver iodide is an insoluble salt with Ksp-8.5x10-17. The solubility can be increased by causing…

A: The objective of the question is to determine whether the addition of NaBr or NaCN would increase…

Q: If 10 mL 0.10 M Ba(NO3)2is mixed with 10 mL 0.10 M K103, a precipitate forms. Which ion will still…

A: Ksp is the solubility product means the minimum ionic product of a salt required for its…

Q: A 23.7 mL sample of 0.216 M triethylamine, (C₂H5)³N, is titrated with 0.309 M nitric acid. At the…

Q: 25) PROVE using calculations and also state whether or not a precipitate will form, (aq., const.…

Q: A 41.00 mL mixture containing 0.0564 M Mn²+ and 0.0564 M Pb2+ is titrated with 0.0813 M K₂S…

A: The initial volume of the mixture = 41.00mLcalculate the number of minimoles of number of millimoles…

Q: A HCN / NaCN buffer system is to be constructed that is also 0.048 M in Mg2+. What is the minimum…

Q: The solubility of Ni(CN), is measured and found to be 2.13x10-6 g/L. Use this information to…

Q: A chemistry graduate student is given 500. mL of a 1.60M propanolc acid (HC,H,CO,) solution.…

Q: Determine the molar solubility (S) of Ag,CO, in a buffered solution with a pH of 4.689 using the…

A: Given: pH = 4.689 pOH can be calculated as: pOH = 14 - pH = 14 - 4.689 = 9.311 pOH = - log [OH-]…

Q: Does a precipitate form for 100.0 mL of 0.002 M Na2CO3 are added to 100.0 mL of 0.002 M MgCl2. The…

A: Introduction: The product of the concentration of ions in a solution, which raised to the same power…

Q: A 35.0-mL solution of 0.075 MCaCl₂ is mixed with 25.0 mL of 0.090 MBaCl₂.(a) If aqueous KF is added,…

A: Volume of CaCl2 = 35 mL Molarity of CaCl2 = 0.075 M Volume of BaCl2 = 25 mL Molarity of BaCl2 =…

Q: A 500 mL sample of a solution saturated at 25°C with calcium oxalate is evaporated to dryness,…

A: Equation involved:- Ca(C2O4)(s) = Ca2+(aq) + C2O42-(aq)

Q: What is the molar solubility of AgCl (Ksp = 1.80 × 101º) in 0.680 M NH,? (Kf of Ag(NH,),* is 1 ×…

A: The explanation is given below-

Q: a. Will silver chloride precipitate from a solution that is 0.010 M AGNO, and 0.010 M NaCl? b. Will…

A: a. We have to tell whether silver chloride will precipitate from a solution that is 0.010 M of AgNO3…

Q: Please provide detailed solution and give the explanation of the concept.... Please don't provide…

A: In this problem, you are tasked to create a buffer solution using dimethylamine(CH3)2NH), which is a…

Q: The Ksp of AgCl is 1.82 x10-10 and the Ksp of AgSCN is 1.1 x10-12. Calculate the molar solubility of…

A: Given that, Ksp of AgCl = 1.82×10-10 Ksp of AgCl = 1.1×10-12 AgCl ionises in water to give Ag+ and…

Q: -6 A solution contains 2.54×100 M NaCl and 6.85×109 M AgNO3. Will a precipitate form? (K AgCl =…

Q: A mixture contains 1.0 x 10-3M Cu+ and 1.0 X 10-3 M Mn²+ and is saturated with 0.10 M H,S. Determine…

Q: TRUE OR FALSE When a precipitating agent is added to a solution with ions, the salt formed out of it…

A: There are some possible conditions for an aqueous solution to produce precipitate - if Q< Ksp ,…

Q: A 42.00 ml. mixture containing 0.0635 M TI* and 0.0635 M Hg+ is titrated with 0.0868 M Nal resulting…

Q: A 25.00 mL solution of 0.08010 M Nal is titrated with 0.05020 M AgNO,. Calculate pAg* following the…

A: Volume of NaI = 25.00 NaIMolarity of NaI = 0.08010 MMolarity of AgNO3 = 0.05020 MKsp of AgI =…

Concept explainers

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

A 45.00 mL mixture containing 0.0746 M TI and 0.0746 M Hg* is titrated with 0.0839 M Nal resulting in the formation
of the precipitates TII and Hg, L,. Calculate pl at the given points in the titration. The K values for TII and Hg, I, are
5.54 x 10- and 2.9 x 10-29, respectively.
62.2 ml. pl
96.2 ml. pl=
second equivalence point pl =
125.0 mL pl =

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 5

Step by step

Solved in 5 steps

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

When Na3PO4 (aq) is added to a solution containing a metal ion and a precipitate forms, the precipitate generally could be one of two possibilities. What are the two possibilities?
Aluminum trifluoride (AIF3) is sparingly soluble with a Ksp value of 1.1 x 103. Calculate the molar solubility ("s") of this precipitate in pure water. 04.1 x 105 06.4 x 10-3 O0.080 O0.14
Silver iodide is an insoluble salt with Ksp=8.5x10-17, The solubility can be increased by causinga different precipitate to be formed. Would the addition of NaBr or NaCN increase thesolubility of AgI? Write the corresponding net ionic equation and accompanying equilibriumconstant to justify your answer. Ksp(AgBr)=5.4x10-13 and Ksp(AgCN)=6.0x10-17
18. Calculate the ion product constant for mixing 100.0 mL of 0.003 M CaCl, with 100.0 mL of 0.0020 M Na,CO,. Ksp for CaCO, is 1.4 x 10°. Does a precipitate form?
What is the molar solubility of AgCl (Ksp = 1.80 x 10-10) in 0.710 M NH:? (Kf of Ag(NH:)2+ is 1.7 x 10") %3D
What is the concentration of Mg2* required (molarity) in a solution that is 0.0019 M in F in order to cause a precipitate to begin to form? The Ksp for MGF2 is 6.14x10-. Report your answer to the tenths place and enter your answer using scientific notation.
A 0.20 M sodium chloride solution is slowly added to a solution containing 0.40 M Pb2* and 0.40 M Ag* ions. What is the remaining concentration of the first ion at the point where the second ion just begins to precipitate? The Ksp of PbCl2 is 1.2x10-5, and the Ksp of AgCl is 1.8x10-10. 1.6x10-6 M 6.0x10-9 M ) 3.1x10-2 M 1.4x10-2 M 3.4x10-5 M
Two students conducted an experiment, where they mixed 6 ml of 0.002M Fe(NO with 3 ml of 0.050 M HNO, A1 ml of 0.002 M NasCN was then added. Assuming that the equilibrium of FeSCN" concentrate is 7.96x 10 M. Determine Keg for the formation of FeSCN O 741 10-4 O 169 10-3 O 3.32 102 O 5.90 10 2 O 117 105
If 10 mL 0.10 M Ba(NO3)2 is mixed with 10 mL 0.10 M KIO3, a precipitate forms. Which ion will still be present at appreciable concentration in the equilbrium mixture if Ksp for barium iodate is very small?
In the determination of chloride by the Mob method, what will be the equiliblium concentration of silver ions in mgil, on the basis of the solubility product principle, when the chloride concentation has been reduced to 0.2 ma? (b) If the concentration of chromate indicator used is 5X M, how much excess silver ion in mgil must be present before the formation of a red precipitate will begi(a) In the defermination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in meL., an the basis of the solubility. pcoduct principle, when the chloride concencration has beea reduced to 0.2m 1.2m? (b) If -3 the concentration of chromate indicator ased is 5 x 10M, bow much excess silver ion in mel, must be present before the formatice of a red precipitate will begin?
We received 15000 Ci of 28Mg, present as Mg(NO3)2 and want to dissolve is in 10 mL water at pH 8. Will we form a precipitate or will the solid entirely dissolve?