8-21. (a) Write the charge balance and mass balance for the solution in which MgBr2 is dissolved to form Mg2+, Br, MgBrt, and MgOH+. (b) Correct the mass balance above for a solution in 0.2 mol S/ETH = 2TH MgB2 I L.

8-21. (a) Write the charge balance and mass balance for the solution in which MgBr2 is dissolved to form Mg2+, Br, MgBrt, and MgOH+. (b) Correct the mass balance above for a solution in 0.2 mol S/ETH = 2TH MgB2 I L.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter10: Effect Of Electrolytes On Chemical Equilibria

Section: Chapter Questions

Problem 10.11QAP

See similar textbooks

Related questions

Q: 2-28. Describe the preparation of (a) 500 mL of 0.0650 M AgNO3 from the solid (b) 400 mL of a…

A: The steps that are involved in the preparation of a solution of a specific molar concentration from…

Q: A sample of 5.034 g containing ammonium sulphate was warmed with 50 cm³ of 0.400 M NaOH (excess).…

A: a.) To calculate the mass of ammonium sulfate , we first Calculate total moles of NaOH that are used…

Q: During the course of the titration of a 20.0 ml of solution containing 0.1 M of NaOH and 0.08 M of…

A: Initial moles of strong base, NaOH in the solution = C*V = 0.1 molL*20.0 mL = 2.0 mmol Initial moles…

Q: A solution is made by mixing 500.0 ml. of 0.04794 M Na, HASO, with 500.0 mL of 0.02554 M NaOH.…

A: The given data contains, Volume of Na2HAsO4 =500 mlmolarity of Na2HAsO4=0.04794 MVolume of NaOH…

Q: 6. Calculate volume in mL of 0.200 M NaOH solution required to neutralize 1.858 g of primary…

A: Given -> Molarity of NaOH = 0.200 M Weight of potassium hydrogen phthalate = 1.858 gm Molar mass…

Q: (iii) 5.0, 25.0, 50.0 and 100.0 g aliquots of MgCl2 were dissolved in 4 separate 250 ml samples of…

A: Reaction of MgCl2 with water: MgCl2 + H2O → MgO + 2 HCl

Q: 8-19. Write the charge balance for a solution of H2SO, in water if the H2SO, ionizes to HSO, and SO…

Q: An aqueous solution is prepared in which 0.00113 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a…

Q: 4. The molar absorptivities of the indicator weak acid HIn (K₁ = 1.42 x 105) and its conjugate base…

Q: 8-19. Write the charge balance for a solution of H2SO4 in water if the H2SO4 ionizes to HSO, and So?…

A: Sulphuric acid is diprotic in nature. So it can loose it's one or both protons.

Q: 9-20. (a) Calculate how many milliliters of 0.100 M HCI should be added to how many grams of sodium…

A: As the volume of the buffer solution is 250 mL, the volume of HCl solution to be added will be 250…

Q: Calculate the % KHP

Q: A standard solution contains 100 ppm of Fe, which was found to have an absorbance of 0.151 au at 508…

Q: Calculate the solubility of BaSO4 solid in 0.0167 M Ba(NO3)2 solution, taking into activity (…

A: Activity coefficient is the ratio of activity to its molar concentration of any substance. In…

Q: (4) The amount of oxalic acid in a sample of 3+ rhubarb was determined by reacting with Fe as…

A: We should equal equivalent of both acid and Fe+3 ion to get mass of oxyliac acid Equivalent =…

Q: a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm…

Q: 6-39. An acidic solution containing 0.010 M La 3+ is treated with NaOH until La(OH), precipitates.…

A: Given information, Concentration of La3+ = 0.010 M Reaction : La3+ (aq) + NaOH (aq) --> La(OH)3…

Q: An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled at 15 deg C,…

A: Alkaline compounds of sodium may involve sodium hydroxide (NaOH), sodium bicarbonate (NaHCO3) and…

Q: 8-21. a. Write the charge and mass balances for a solution made by dissolving MgBr, to give Mg?+, Br…

A: The chemical formula of a substance provides information about the atoms involved and their…

Q: 10.) Calculate the activity coefficient of K* in 0.050 M KNO3.

Q: Sample containing arsenic weighing 0.800 are titrated with a standard iodine soluton. what should be…

A: To solve this problem, you need to first determine the molar mass of arsenic trioxide (As2O3). The…

Q: 6-21. If a solution containing 0.10 M Cl¯, Br ,I¯, and CrO? is treated with Ag*, in what order will…

A: Precipitation is depend upon the value of Ksp , if the ksp value is high the silver salt will be…

Q: A series of solutions containing NAOH, Na,CO, and NaHCO, alone or in compatible combination, was…

A: Answer: The table showing the volume of 0.1202 M HCl used to titrate 25.00 m of a series of…

Q: A dried sample of commercial salt was prepared by a coning and quartering. A 0.911-g sample of the…

A: NaCl (aq) + AgNO3(aq) -----> AgCl(s) + NaNO3(aq) 1 mole AgNO3(silver nitrate) neutralizes 1 mole…

Q: 8-H. Write charge and mass balances for aqueous Ca3(PO4)2 if the species are Ca2+, CaOH+, CaPO, PO,…

A: The charge balancing equation is an algebraic expression of electroneutral balancing of the…

Q: ionic strength of (a) 0.008 7 M KOH and (b) 0.000 2 M La(IO,)3

Q: (a) For the precipitation reaction: A+ + B–  AB(s)Calculate the value of the equilibrium constant…

A: The answer for part (a) is given below. Kindly repost the other questions as separate question. a)…

Q: Write the balance equation of aqueous Pb(ClO3)2 with NaI. Include phases.

A: balanced chemical equation of Pb(ClO3)2 with NaI

Q: Complete this reaction Mn, O, Mn; + A providing A, B and C

Q: What mass of ZnS (Ksp = 2.5 x 10-22) will dissolve in 325.0 mL of 0.050 M Zn(NO3)2? Ignore the basic…

A: Since Zn(NO3)2 is completely soluble in water as Zn(NO3)2 -----> Zn2+ + 2 NO3- Hence…

Q: Calculate the mass of silver (in grams) in 772 ml of 2.22 M Na [Ag (NO,) ,] solution. -3 (K, -2 ([Ag…

Q: Use the following atomic masses (in g/mol): Mg = 24.31; O = 16; Ca = 40.08; C = 12.01; Na = 23; H =…

A: HCl + NaOH→ NaCl + H2O at equivalence point Number of equivalents of HCl = Number of equivalents of…

Q: Consider the titration of 100.0 mL of 0.010 0 M Ce4+ in 1 M HClO4 by 0.040 0 M Cu+ to give Ce3+ and…

Question

8-21. (a) Write the charge balance and mass balance for the solution in which
MgBr2 is dissolved to form Mg2+, Br, MgBrt, and
MgOH+. (b) Correct the mass balance above for a solution in 0.2 mol
MgB2 I L.

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 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

cion 12 of 13> OAttempt 4 A solution is made by mixing 500.0 mL of 0.04794 M Na, HASO, with 500.0 mL of 0.02554 M NAOH. Complete the mass balance expressions for the sodium and arsenate species in the final solution. (HASO + (H, AsO 1+ [H, AsO,+ [Aso 1 Incorrect (Na") = 3.67 xid 2 M. Incorrect
4. The molar absorptivities of the indicator weak acid HIn (K₁ = 1.42 x 105) and its conjugate base In at 570 were determined as ε(HIn) = 7120 and ɛ(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 × 10%. (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 x 105 and pH = 6.5.
2-28. Describe the preparation of (a) 500 mL of 0.0650 M AGNO3 from the solid reagent. (b) 400 mL of a solution that is 0.0825 M in Kt. starting with solid K,Fe(CN)6 . (c) 2.00 L of 0.120 M HCIO, from the commercial reagent [60% HCIO4 (w/w), sp gr 1.60].
Consider the titration of 100.0 mL of 0.010 0 M Ce4+ in 1 M HClO4 by 0.040 0 M Cu+ to give Ce3+ and Cu2+, using Pt and saturated Ag | AgCl electrodes to find the end point. (a) Write a balanced titration reaction. (b) Write two different half-reactions for the indicator electrode. (c) Write two different Nernst equations for the cell voltage. (d) Calculate E at the following volumes of Cu+: 1.00, 12.5, 24.5, 25.0, 25.5, 30.0, and 50.0 mL. Sketch the titration curve.
What mass of ZnS (Ksp = 2.5 x 10-22) will dissolve in 325.0 mL of 0.050 M Zn(NO3)2? Ignore the basic properties of S2-.
Complete this reaction Mn, 0, - Mn;" + A providing A, B andC
Sample containing arsenic weighing 0.800 are titrated with a standard iodine soluton. what should be the normality of the iodine in order that each ml of titrant represents 1/2% As2O3 in the sample (Answer: 0.0809 N show full solution please)
a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.
8-21. a. Write the charge and mass balances for a solution made by dissolving MgBr, to give Mg?+, Br , MgBrt, and MGOH+. b. Modify the mass balance if the solution was made by dissolving 0.2 mol MgBr, in 1 L.
4
It is required to know the concentration of an aqueous solution of H2SO4 that appeared in the laboratoryChemistry III and it's unlabeled. To this end, a student of analytical chemistry carried out the followingProcedure: He took 5.00 mL of a fresh and standardized solution of 0.525M NaOH and brought them to a250.0 mL balloon to be completed with distilled water. Subsequently, he poured 15.00 mL of the solutionH2SO4 of unknown concentration in an Erlenmeyer flask and added 2 drops of phenolphthalein.Using a burette filled with the last NaOH solution, he noticed that when adding 39.40 mL of the hydroxidethe Erlenmeyer solution reached a faint but permanent pink. With the above dataDetermine the concentration and pH of the H2SO4 solution.
Calculate the % KHP of the 1.294-g sample which consumed 48.25 mL in 0.09605 N NaOH solution in titration. (MW KHP = 204.22)