Answered: Inorganic Chemistry: Qualitative…

Inorganic Chemistry: Qualitative Analysis of Anions What is the importance or purpose of adding H2O2 to the centrifugate to confirm the presence of SO3-2 ? How does it confirm the presence of SO3-2 ?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.12QAP

See similar textbooks

Related questions

Q: Calculate the pH of a buffer solution containing 10.0 cm3 of 0.100 mol dm–3 NaOH and 20.0 cm3 of…

Q: Why do you add NaHCO3 to the sample solutions in the determination of chloride by the Mohr Method…

A: Mohr method is a process in which we determine chloride by reacting it with silver nitrate solution…

Q: Look at Figure 2.17. If you did this titration using TRIS instead of phosphate, how would the…

Q: Calculate the molar concentration of Agtao) kons in a 2.12 M solution of AgCl 2 with no excess…

Q: Why does the solubility of a salt of a basic anion increase with decreasing pH? Write chemical…

A: On decreasing the pH of the solution, the concentration of H+ in the solution increases. The…

Q: In solution, fentanyl is most stable in the pH range 3.5-7.5. What mass of acetic acid and sodium…

A: Solution- Data given- volume is 1 L, concentration is 30 mM, molecular mass (RMM) of acetic acid…

Q: what volume of 2.00 M NaOH should be added to 250.0 ml of 1.00 M glycolic acid(Ka = 1.48 x 104) to…

A: Given data: Molarity of NaOH = 2 M Molarity of glycolic acid = 1 M Volume of glycolic acid = 250 mL…

Q: A solution of acetic acid (Ka = 1.8 x 10-5) is found to be 0.15% dissociated. What was the initial…

Q: Chikana experimentally determined the ionization constant of a weak monoprotic acid Chumami (Λ0 =…

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

Q: Determine the pH of (a) a 0.40 M CH3COOH solution and (b) a solution that is 0.40 M CH3COOH and 0.20…

A: a) CH3COOH dissociates in the solution as: CH3COOH⇌CH3COO-+H+Initial…

Q: Zinc uranyl acetate, Magnesium uranyl acetate and Cobalt uranyl acetate, forms insoluble salts with…

A: zinc uranyl acetate, magnesium uranyl acetate, and cobalt uranyl acetate, forms insoluble salt with…

Q: 1. The formation constant for the lead(II)-EDTA chelate, PbY2, is 1.10 x 1018. Calculate the…

A: The expression for calculating the conditional formation constant is as follows,…

Q: 5. Why should the titration solution be buffered at pH 10.0?

A: In complexometric titration the titrant used is EDTA. EDTA forms a complex with the metal ions which…

Q: The dissociation constant, ka, of a weak acid is 5.9 x 10-6. What is the pKa of the acid?

Q: What is the pH and fraction of dissociation of a 0.100 M solution of the weak acid HA with Ka =1.00…

A: pH and fraction of dissociation of a 0.100 M solution of the weak acid HA with Ka =1.00 X10(-5) are…

Q: Why is Iodide(I-) the most interesting qualitative test for the identification of an anion?

A: Iodide anion exhibits some of the most interesting qualitative analysis tests in chemistry. Like,…

Q: when 15.00 mL of 2.00 x 10^-6 M lithium sulfate is mixed with 17.00 mL of 1.00 x 10^-6M sodium…

A: Given: Concentration of lithium sulfate i.e. Li2SO4 = 2.00 × 10-6 M Volume of Li2SO4 solution =…

Q: Calculate the pH during the titration of 43.0 mL 0.108 M nitrous acid (pK, = 3.15) with 0.104 M NAOH…

A: EXPLANATION: pH is the measurement of acidity and alkality of a solution.It is defined as a negative…

Q: What would the pH be after addition of 10.09 mL of 0.1000 M HCl to 25.00 mL of 0.1000 B (a weak…

A: First we will calculate number of moles of both and then using ICE table, calculate pH of the final…

Q: The molar solubility of sulfathiazole (weak acid) in water is about 0.001 M. a. What is the lowest…

A: Given: pKa of sulfathiazole = 7.2 Molar solubility of sulfathiazole = 0.001 M

Q: Find the pH and fraction of dissociation of a 0.010 0 M solution of the weak acid HA with Ka = 1.00…

A: Dissociation reaction of a weak acid is as following :- HA ↔ H+ +…

Q: A newly discovered extremely basic polar amino acid has pka values of 2.37, 13.01, and 11.89 for…

A: Here we are required to find the overall charge over amino acid at the given pH=13.01

Q: Calculate pBr for a solution that is 4.62 x 10-3 M in KBr and 1.78 x 10-3 M in BaBr, 1. O2.09 2.…

A: From given datas Initially reaction is given and from that we found how many Br- produced for each…

Q: Explain briefly in 2 sentences andin your OWN words. 1. NH4CNS used in the test for cobalt must be…

A: Gravimetric analysis is one of the most accurate analytical methods available. It is concerned with…

Q: What is the pKa value of Tris-HCl?

A: The molecular formula of Tris-HCl is: NH2C(CH2OH)3 ·HCl

Q: Solid sodium sulfate, Na2SO24, is added slowly to a solution that is 1.0*10^-4 M in both Ba^2+ and…

A: Given,[Ba2+] = 1.0*10-4 M[Pb2+] = 1.0*10-4 MBaSO4 (Ksp=1.1*10-10)PbSO4 (Ksp=1.7*10-8)

Q: What is selective precipitation? What is confirmatory test and its significance? What are the…

A: In selective precipitation only specifically the one which is desired is precipitated in presence of…

Q: Zinc uranyl acetate, Magnesium uranyl acetate and Cobalt uranyl acetate, forms insoluble salts with…

Q: Propanoic acid, C₂H5COOH, is a weak acid, with Ka = 1.35 x 10-5 mol dm-³. i) Write an expression for…

Q: Determining the Ksp of Calcium Hydroxide: Ca(OH)2 (s) ↔ Ca2+ (aq) + 2OH– (aq) Ksp = [Ca2+][OH–]2…

A: Acid-base titrations involve neutralization of an acid by a base. This is called neutralization. If…

Q: To 10,00 ml of 0,0500 mol/l solution of potassium bromide – 9,00 ml of solution of 0,05500 mol/l…

Q: Calculate the pH of a buffer solution containing 10.0 cm³ of 0.100 mol dm-³ NaOH and 20.0 cm³ of…

A: 1 dm^3 = litre 1 cm^3 = milli litre Millimoles = molarity (mol/L)* volume (in ml)

Q: *D. Ksp = [Ag*]² · [SO4 1 %3D Ksp- pwidut/deacte.cauh una bulilor liguel. 2. If the gram solubility…

Q: Calculate pBr for a solution that is 4.62 x 10 M in KBr and 1.78 x 10- M in BaBr2 1. O2.09 2. O1.96…

A: We have KBr as 4.62*10-3 M, BaBr2 as 1.78*10-3 M .we have to calculate the pBr.

Q: The equilibrium constant for the dissolution of Mg (OH) 2: Kps = 5.6 x 10-12 What is the molar…

A: Given data,Ksp of Mg(OH)2=5.6×10-12

Q: Would the indicator bromocresol green, with a transition range of pH 3.8–5.4, ever be useful in the…

A: weak acid react with strong base, it give basic solution. So, the pH of the solution after…

Q: Calculate the pH at intervals of 20mL (from 0 to 100 mL) by titrating 40 mL of hydrogencyanate (pKa1…

Q: In a different situation, you want to use acid-base extraction to separate compound A (pK, = 5.9)…

A: We will add Na2CO3 solution to separate A from B

Q: Find the pH during the titration of 20.00 mL of 0.1000 Mtri-ethylamine, (CH₃CH₂)₃N…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: 6. C„H¾CI, proton coupled solvent proton decoupled 200 160 120 80 40

A: The molecular formula of the organic compound = C2H4Cl2 The degree of unsaturation = C+1-H/2-X/2…

Q: Find the conditional formation constant, Kr, for FeY² at pH 8.00 given: ay = 4.2 x 10³ and Kp=…

A: Formation constant ( Kf) The equilibrium constant for the reaction with metal with ligand is called…

Q: 2. (a) How would you compare the Lewis acidity of Fe2+ and Cu?+? (b) The measured pka values for…

A: Lewis acids are the species which accepts pair of electron and Lewis bases donate a pair of…

Q: Construct a titration curve (E vs. Vtitrant) for the titration of 25.00 mL of 0.100 M Fe2+ with…

A: Answer : We have Fe+2 as initial solution and Ce+4 is as titrant As reduction potential of Ce+4 is…

Q: Which of these compounds would be the best buffer at pH 5.0: formic acid (pKa = 3.8), acetic acid…

A: Given: The pH of the buffer solution = 5.0 The pKa of formic acid = 3.8 The pKa of acetic acid =…

Q: The solubility of CaCO3 is pH dependent. (a) Calculate themolar solubility of CaCO3 (Ksp = 4.5 x…

Q: Determining the Ksp of Calcium Hydroxide: Ca(OH)2 (s) ↔ Ca2+ (aq) + 2OH– (aq) Ksp = [Ca2+][OH–]2…

A: For HCl versus Calcium hydroxide titration, Ca(OH)2+2HCl⇔CaCl2+2H2O MHClVHCl=2×MCa(OH)2VCa(OH)2

Q: Dr. Stone and Princess Bubble gum wanted to run an experiment to determine at what volume they will…

A: Given: Titration of CF3COOH with a pKa of 0.52 with 0.1 M NaOH.

Question

Inorganic Chemistry: Qualitative Analysis of Anions

What is the importance or purpose of adding H₂O₂to the centrifugate to confirm the presence of SO₃^-2 ? How does it confirm the presence of SO₃^-2?

Branch of chemistry that involves the study of compounds that are not carbon-based, which are known as inorganic compounds. Such compounds include many of Earth's metals and minerals. Inorganic chemistry's importance spans across many of the same disciplines that organic chemistry is needed in, yet it is of particular interest to materials science and agriculture.

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 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

Would the indicator bromocresol green, with a transition range of pH 3.8–5.4, ever be useful in the titration of a weak acid with a strong base? Why?
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)
b. A student has a sea water sample which contains Ca2+ ions . Describe briefly how he willdetermine the concentration of Ca2+ ion in the sample using a simple titration. Explain the colourchanges at the endpoint. Which medium is suitable for performing the titration, acidic or basic medium and why?
What is selective precipitation? What is confirmatory test and its significance? What are the products formed when Group 1 cations are allowed to react with KOH? Why is it necessary to have an acidic environment when separating Group 1 cations from other metal ions?
Sketch a plot of the fraction of species, f, vs pH for Tyr. Show your calculations for several points on the plot. You want to calculate the fraction of the species for more than 3 of the points. pKa’s for Tyr is 2.24, 9.04, and 10.10.
A student has a sea water sample which contains Ca2+ ions . Describe briefly how he willdetermine the concentration of Ca2+ ion in the sample using a simple titration. Explain the colourchanges at the endpoint. Which medium is suitable for performing the titration, acidic or basic medium and why?
I was just wondering how you got the 4.0 x 10-4 for the acidionzation constant.
A particular solution is 0.05M with respect to ethanoic acid and 0.2M with respect to sodium ethanoate (Ka for ethanoic acid = 2 x 10-5moldm-3). What is this type of solution called? Calculate the pH of the solution
Many chemical reactions are carried out in the presence of buffers. Use the Henderson-Hasselbalch equation to provide a recommendation for a suitable acete/acetic acid buffer under the following reaction conditions. a) If a checial reaction produces hydroxide ion, OH-, what would be the range for the target pH of a buffer soution that would favor pH stabilizatoin under these conditions? Explain.
Suppose your colleague was relying on receiving your purified product in order to prepare a dilute aqueous standard solution of benzoic acid e.g. for a titration. She takes 160 mg of your benzoic acid and dissolves it in just enough water so the solution exactly fills a 250 mL volumetric flask. Given that the acid dissociation constant of benzoic acid Ka = 6.3 x 10-5, calculate the pH of her resulting solution.
Which of these compounds would be the best buffer at pH 5.0: formic acid (pKa = 3.8), acetic acid (pKa = 4.76), or ethylamine (pKa = 9.0)? Briefly justify your answer.
Many chemical reactions are carried out in the presence of buffers. Use the Henderson-Hasselbalch equation to provide a recommendation for a suitable acete/acetic acid buffer under the following reaction conditions. a) If a checial reaction produces hydroxide ion, H3O+, what would be the range for the target pH of a buffer soution that would favor pH stabilizatoin under these conditions? Explain.