An acidic solution is 9 mM in each of the following metal ions: Sn²+, Co²+, Mn²+, Pb²+. See the Solubility Product Constant Table.(c) At what pH do the metal hydroxides begin to precipitate?Sn(OH)₂ 40 89xCo(OH)2 49 7.9Mn(OH)₂ 49 8.4Pb(OH)2 4.0 5.1Substance Ksp at 25 °CAluminumAl(OH)3BariumBa(OH)25.0 x 10-³BaCO38.1 x 10-⁹BaSO41.1 x 10-10Ba3(PO4)2 3.4 x 10-23CadmiumCd(OH)2CdCO3CdSCalcium1.9 x 10-332.5 x 10-145.2 x 10-128.0 x 10-27Ca(OH)25.5 x 10-6CaCO3 4.8 x 10-⁹Ca3(PO4)2 1.0 × 10-26CaF23.9 x 10-11ChromiumCo(OH)₂Cr(OH)3 6.3 x 10-31Cobalt16 x 10-15✓✓xCopperCu(OH)2Cu₂SCUCO3CuSIronFe(OH)2FeSFe(OH)3FePO4LeadPb(OH)2PbF2PbCl₂PbBr₂Pbl2PbCrO4PbSO4PbS2.2 x 10-201.6 x 10-481.4 x 10-106.3 x 10-368.0 x 10-166.3 x 10-182.5 x 10-399.9 x 10-292.8 x 10-163.7 x 10-81.7 x 10-56.3 x 10-66.5 x 10-91.8 x 10-141.7 x 10-88.4 x 10-28MagnesiumManganeseMn(OH)2MnCO3MnSNickelNi(OH)2SilverAgClAgBrAglAgCNAg₂SAg₂ CrO4Ag3PO4TinSn(OH)2SnSZincZnCO3Zn(OH)21.9 × 10-138.8 x 10-115.6 x 10-161.6 x 10-141.8 x 10-105.0 x 10-138.3 x 10-171.2 x 10-166.3 x 10-501.1 x 10-122.6 x 10-181.4 x 10-281.3 x 10-231.0 × 10-104.5 x 10-17

The concentration of each of the metal ions, [Sn2+], [Co2+], [Mn2+], [Pb2+] is given 0.9 mM. The Ksp…

An acidic solution is 9 mM in each of the following metal ions: Sn²+, Co²+, Mn²+, Pb²+. See the Solubility Product Constant Table. (c) At what pH do the metal hydroxides begin to precipitate? Sn(OH)₂ 40 1.89 X Co(OH)₂ 49 7.9 Mn(OH)₂ 49 8.4 Pb(OH)2 495 5.1 X

An acidic solution is 9 mM in each of the following metal ions: Sn²+, Co²+, Mn²+, Pb²+. See the Solubility Product Constant Table. (c) At what pH do the metal hydroxides begin to precipitate? Sn(OH)₂ 40 1.89 X Co(OH)₂ 49 7.9 Mn(OH)₂ 49 8.4 Pb(OH)2 495 5.1 X

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: 6. 74 mg of Ca(OH)2 is all that can be dissolved in 100 mL solution at a certain temperature. Which…

Q: To determine the amount of Cl in an unknown sample, a NaCl sample was titrated with the titling…

A: Number of moles=massmolar mass From the given information, AgNO3 + NaCl → NaNO3 + AgCl Mass of…

Q: A solution contains 5.21x10-3 M cobalt(II) acetate and 1.22x10-2 M zinc nitrate. Solid sodium…

A: Answer:For a sparingly soluble salt, precipitation only begins when its solubility product becomes…

Q: The solubility of an ionic compound in water can be expressed in terms of the mass that will…

A: Given: The dissociation of Ca(OH)2 in water is as follows: Ca(OH)2 ⇋…

Q: A solution contains 6.69x10-³ M ammonium carbonate and 1.08x10-2 M sodium hydroxide. Solid…

A: When for a particular substance, Ksp > its ionic product, then precipitation starts .

Q: ) A 20.2 mL sample of a 0.422 M aqueous hydrofluoric acid solution is titrated with a 0.426 M…

Q: ake was given an unknown solution thought to contain Pb²⁺ and/or Ba²⁺ and asked to perform chemical…

A: Jake concluded that the white precipitate formed in the solution after the addition of sulphate ions…

Q: soluble in water?

Q: A solution contains 1.16×102 M sodium sulfide and 1.20x10² M potassium hydroxide. Solid…

Q: A solution contains 1.32x102 M sodium carbonate and 8.59x10 M potassium hydroxide. Solid copper(II)…

A: Copper(II) nitrate reacts with sodium carbonate to form copper(II) carbonate and with potassium…

Q: The solubility of Ag2CrO4 (Ksp = 1.2 x 10^-12) is several times greater than that of AgCl (Ksp =…

Q: Which ionic compound below would NOT precipitate from the solution during a chemical reaction? Hint:…

A: This question is related to solubility of salts. Solubility of the salt is the mass of salt which…

Q: A solution contains 5.59×10-3 M iron(II) nitrate and 6.82×10-3 M copper(II) acetate. Solid sodium…

A: The solubility products are required to solve this question. Using reference chart below I mentioned…

Q: A

Q: A solution contains 1.08×10-2 M lead nitrate and 1.24x10-2 M silver acetate. Solid ammonium bromide…

A: Given: Concentration of silver acetate i.e. AgCH3COO = 1.24 × 10-2 M Concentration of lead nitrate…

Q: A solution contains 1.16x102 M sodium sulfide and 1.20×10-2 M potassium hydroxide. Solid…

A: Given: Concentration of sodium sulfide i.e. Na2S = 1.16 × 10-2 M Concentration of potassium…

Q: When the aqueous solutions of ZnSO4, K2S, and Ba(ClO3)2 are mixed together, which of the following…

A: In the given reaction we have to predict all the possible precipitates formed when ZnSO4, K2S, and…

Q: A solution contains 1.22×10-2 M chromium(III) nitrate and 6.44×10-3 M manganese(II) acetate. Solid…

A: We need to find the hydroxide ion at which the Manganese(II) ion precipitates. Then, at this…

Q: You have a solution of 1M BaCl2 and another of 1M Hg2(NO3)2. If you poured them together, what…

A: 1. In double displacement reaction, cation of one species easily replaces cation of another species…

Q: 25 mL 0.125 M aluminum acetate is combined with 35 mL 0.300 M rubidium hydroxide, and the reaction…

A: •Here we have to calculate yield. •So firstly we find limiting reagent. •Than on the basis of…

Q: A solution contains 1.16×102 M sodium sulfide and 1.20x10-2 M potassium hydroxide. Solid…

A: Given: Concentration of sodium sulfide i.e. Na2S = 1.16 × 10-2 M Concentration of potassium…

Q: A solution contains 7.81x10-3 M sodium hydroxide and 7.99x10-3 M ammonium sulfide. Solid iron (III)…

A: Sodium hydroxide, NaOH is completely dissociated to form Na+(aq) and OH-(aq). Ammonium sulfide,…

Q: solution contains 1.05×102M zinc acetate and 1.04×10 M nickel(II) nitrate. olid sodium cyanide is…

A: The question is based on the concept of solubility product Principle. it states that a weak…

Q: A student makes a solution using the following volumes of stock solutions. mL 0.019 M Fe(NO3)3 3.37…

A: Fe(NO3)3 is a strong electrolyte. It dissociates 100% to the ions Fe3+ and NO3-.

Q: A solution contains 0.0450 M Ca2+ and 0.0940 M Ag+. If solid Na3PO4 is added to this mixture, which…

A: 1. Which is the more stable?Ca3(PO4)2 Ag3PO41. 2. Ksp value of both substanceCa3(PO4)2 - 2.07 x…

Q: Determine the mass, in grams, of precipitate that forms when 608, ml. of 0.499 M Na₂CO, reacts with…

A: The question is based on the concept of reaction stoichiometry. we need to calculate mass of calcium…

Q: A solution contains 6.69x10-3 M sodium hydroxide and 1.48x10-2 Mammonium phosphate. Solid…

A: The question is based on the concept of solubility product principle. It states that when a weak…

Q: Part 1 Solution A is a 5.0 L aqueous sodium iodide (Nal) solution, and I want to determine the…

A: Using law of chemical equivalance we can determine the concentration of iodide in the given…

Q: A solution contains 1.17x102 M iron(III) nitrate and 1.22x10² M silver acetate. Solid sodium…

Q: If we mix 45 mL of 1.5 M sodium iodide with excess lead nitrate, how many grams of precipitate will…

Q: The solubility-product constant for Ce(IO3)3 is 3.2 x 107 -10 40.00 mL of a. water? b. 0.0440 M…

Q: Chemistry I have 250 mL of 0.250M Cd(NO3)2 that I mix with 500 mL of 0.100 M Cu(NO3)2 and 250 mL of…

A: First, we have to find the respective ion concentrations before just after mixing. Each of…

Q: Analysis shows the 15.0 L of seawater simulant contains a mercury (II) ion concentration of 3 X 10-4…

A: The number of moles of potassium iodide (KI), nKI, in the 15.0 L of seawater is;…

Q: A solution contains 0.0120 M Pb² + (aq) and 0.0120 M Sr2 + (aq). If you add SO-(aq), what will be…

Q: Did the student conduct the experiment correctly? (may need to consult solubility rules and your…

A: A student obtained results in the lab:Mg(NO3)2 was reacted with NaCl, Na2S , NaOH and Na2CO3But in…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

An acidic solution is 9 mM in each of the following metal ions: Sn²+, Co²+, Mn²+, Pb²+. See the Solubility Product Constant Table.
(c) At what pH do the metal hydroxides begin to precipitate?
Sn(OH)₂ 40 89
x
Co(OH)2 49 7.9
Mn(OH)₂ 49 8.4
Pb(OH)2 4.0 5.1
Substance Ksp at 25 °C
Aluminum
Al(OH)3
Barium
Ba(OH)2
5.0 x 10-³
BaCO3
8.1 x 10-⁹
BaSO4
1.1 x 10-10
Ba3(PO4)2 3.4 x 10-23
Cadmium
Cd(OH)2
CdCO3
CdS
Calcium
1.9 x 10-33
2.5 x 10-14
5.2 x 10-12
8.0 x 10-27
Ca(OH)2
5.5 x 10-6
CaCO3 4.8 x 10-⁹
Ca3(PO4)2 1.0 × 10-26
CaF2
3.9 x 10-11
Chromium
Co(OH)₂
Cr(OH)3 6.3 x 10-31
Cobalt
16 x 10-15
✓
✓
x
Copper
Cu(OH)2
Cu₂S
CUCO3
CuS
Iron
Fe(OH)2
FeS
Fe(OH)3
FePO4
Lead
Pb(OH)2
PbF2
PbCl₂
PbBr₂
Pbl2
PbCrO4
PbSO4
PbS
2.2 x 10-20
1.6 x 10-48
1.4 x 10-10
6.3 x 10-36
8.0 x 10-16
6.3 x 10-18
2.5 x 10-39
9.9 x 10-29
2.8 x 10-16
3.7 x 10-8
1.7 x 10-5
6.3 x 10-6
6.5 x 10-9
1.8 x 10-14
1.7 x 10-8
8.4 x 10-28
Magnesium
Manganese
Mn(OH)2
MnCO3
MnS
Nickel
Ni(OH)2
Silver
AgCl
AgBr
Agl
AgCN
Ag₂S
Ag₂ CrO4
Ag3PO4
Tin
Sn(OH)2
SnS
Zinc
ZnCO3
Zn(OH)2
1.9 × 10-13
8.8 x 10-11
5.6 x 10-16
1.6 x 10-14
1.8 x 10-10
5.0 x 10-13
8.3 x 10-17
1.2 x 10-16
6.3 x 10-50
1.1 x 10-12
2.6 x 10-18
1.4 x 10-28
1.3 x 10-23
1.0 × 10-10
4.5 x 10-17

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

CaCl2(aq) + 2 AgNO3(aq) ⟶Ca(NO3)2 + 2 AgCl Fill in the blanks with either an (s) or an (aq) to indicate the phase of each product. Use the Solubility Rules.
Please don't provide handwriting solutions..
Silver chromate is sparingly soluble in aqueous solutions. The ?sp of Ag2CrO4 is 1.12×10−12 M^3 What is the solubility (in moles per liter) of silver chromate in a 1.10 M silver nitrate aqueous solution? M=
What is the iron(II) ion concentration in a solution prepared by mixing 329 mL of 0.411M iron(II) nitrate with 421 mL of 0.249 M sodium hydroxide? The K of iron(II) hydroxide is 4.87 x 10 – 17. [Fe**] = M
When a strong base is added to a solution of CuSO4, which is pale blue, a precipitate forms and the solution above the precipitate is colorless Part 1 See Periodic Table Include phases in the balanced chemical equations. What is the net chemical equation that describes this reaction? Cu+2(aq)+2OH−(aq)Cu(OH)2(s) Part 2 When ammonia is then added, the precipitate dissolves and the solution turns a deep navy blue. What is the net chemical equation that describes this event?
Will a precipitate of SrF2 form if you mix 25 mL of 7.1 x 10^-2 M Sr(NO3)2 (aq) with 85 mL of 3.2 x 10^-3 M NaF (aq)?
The iodide ion concentration in a solution may be determined by the precipitation of lead iodide. Pb2+ (aq) + 21 (aq) →→→→PbI₂ (s) A student finds that 22.10 mL of 0.5530 M lead nitrate is needed to precipitate all of the iodide ion in a 25.00-mL sample of an unknown. What is the molarity of the iodide ion in the student's unknown? M
A solution contains 8.55x103 M potassium cyanide and 1.36x10-2 M sodium hydroxide. Solid nickel(II) acetate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of nickel ion when this precipitation first begins? [Ni2*] = M
When taking into consideration the attached problem, How would I calculate the Theoretical yield in grams?
25 mL 0.125 M aluminum acetate is combined with 35 mL 0.300 M rubidium hydroxide, and the reaction below is allowed to proceed to completion. Al(C2H3O2)3 (aq) + 3 RbOH (aq) --> Al(OH)3 (s) + 3 RbC2H3O2 (aq) 186 mg of aluminum hydroxide (78.00 g/mol) is collected. The yield of the reaction is _____ % Round your answer to the nearest whole number.
2Fe(s) + 3Cu2+(aq) 2Fe3+(aq) + 3Cu(s) a)Calculate the minimum volume of 1.16M CuSO4 solution that is required to ensure complete reaction of 1.04g of Fe.Since you do not know which reaction will be the one to occur, you must base the calculation on whichever of the equations requires more CuSO4 solution. b)To ensure that sufficient CuSO4 is used, it is common practice to add an excess.Calculate the volume of 1.16M CuSO4 needed to provide a 20% excess in this case.
Solid nickel(II) fluoride is slowly added to 50.0 mL of a potassium hydroxide solution until the concentration of nickel ion is 0.0266 M. The maximum amount of hydroxide remaining in solution is M.