: For PBC12 (Ksp = 2.4 x 10-4), will a precipitate of PbCl2 form when 0.10 L of 3.0 x 10M Pb(NO3)2 is added to 400 mL of 9.0 x 10-2M NaC1?O Yes, because Q> KspNo, because Q

Answered: Image /qna-images/answer/5de5f187-8ba1-4f82-8f9d-07331375058e.jpg

Answered: : For PBC12 (Ksp = 2.4 x 10-4), will a…

: For PBC12 (Ksp = 2.4 x 10-4), will a precipitate of PbCl2 form when 0.10 L of 3.0 x 10 2M Pb(NO3)2 is added to 400 mL of 9.0 x 10-2M NaC1? Yes, because Q > Ksp No, because Q

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

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 94AE: Will a precipitate of Cd(OH)2 form if 1.0 mL of 1.0 M Cd(NO3)2 is added to 1.0 L of 5.0 M NH3?...

See similar textbooks

Related questions

Q: Consider a scenario wherein a solution containing 6.25×10^-3 M of S(2-) and 5.63×10^-3 M of Cd(2+)…

Q: A solution prepared in the lab contains 3.5 x 10* M Sr2* and 0.0010 M F. Will a precipitate form?…

A: A precipitation occurs when Q > Ksp Q = [Sr2+] [F-]2

Q: A solution contains 3.25x10-5 M Ca2+ and 7.25 x10-5 M CO3²-. Will a precipitate form in the…

A: If KSP < ionic product (Q) Then precipitation occurs. Ionic product ,Q = [Ca2+] […

Q: A solution initially contained 39 g/L of CO3²- and 15 g/L of Mg2+. When equilibrium is finally…

Q: Will a precipitate of magnesium fluoride form when 300.0 mL of 1.1 x 10-3 M MgCl2 are added to 500.0…

Q: f 27.5 mL of 1.63x10-9M of FeCl3 is added to 98.6mL of 2.58x10-9 M NaOH, will a precipitate of…

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

Q: (Q54) Nickel iodate, Ni(IO3)2 is being precipitated out of a 1.00 L solution. If the concentration…

A: Given that, Nickel iodate, Ni(IO3)2 is precipitated Concentration of disdolved Ni2+ ion , [Ni2+] =…

Q: Consider the following equilibrium: Mg(OH)₂(s) Mg²+ (aq) + 2OH(aq) Given that Ksp = 1.8 x 10-11,…

A: Answer: Given data: Concentration of Mg(OH)2 C=1.3×10-7M Solubility product of Mg(OH)2…

Q: Exactly 500 mL of 0.058 M MgCl2 are mixed with exactly 300 ml of 0.0019 M K2CO3. Will a precipitate…

Q: Will Ag2Cr207 precipitate when 150.0 mL of 1.2 × 103 M AGNO3 are added to 50.0 mL of 1.9 x 10-2 M…

A: Solubility product It is the product of concentration term raised to the power of their…

Q: The Ksp for BaF2 is 2.4 × 10–5. When 10 mL of 0.01 M NaF is mixed with 10 mL of 0.01 M BaNO3, will a…

A: The solubility product constant (Ksp) represents the solubility of products at equilibrium for…

Q: Barium Carbonate (BaCO,) has a solubility product of Ksp = 8.1 x 10° at 25°C for the equilibrium…

A: Given that: Solubility product constant of BaCO3 = 8.1×10-9 BaCO3 dissociates into water as :…

Q: Mg3(PO4)2 has Ksp = 1 * 10^-25. Write the balanced equation to which this equilibrium constant…

Q: Solid Naz SO4 is added slowly to a solution that is 0.50M in Pb(NO3), and 0.59M in Ba (NO3),. In…

Q: Will a precipitate form when 100.0 mL of 3.8x10-4 M Mg(NO3)2 is added to 100.0 mL of 2.6x10-4 M…

A: The solubility product constant (Ksp) represents the solubility of products at equilibrium for…

Q: Will a precipitate form when 25 mL of 0.0005 M K2CO3 is mixed with 25 mL of 0.0005 M Ni(NO3)2? The…

A: We need to determine the ionic product of NiCO3 and to predict whether the precipitate will form or…

Q: For nos. 36 - 37, consider a scenario wherein a solution containing 6.25×10-3 M of S2- and 5.63×10-3…

A: Given that, Concentration of S2- , [S2-] = 6.25×10-3 M Concentration of Cd2+ , [Cd2+] = 5.63×10-3 M…

Q: For BaF2 (Ksp = 1.7 × 10–6), will a precipitate of BaF2 form when 0.10 L of 6.0 × 10–2 M Ba(NO3)2 is…

Q: For PBCI 2 (K sp = 2.4 x 10-4), will a precipitate of PbCl , form when 0.10 L of 3.0 x 10 -2 M Pb(NO…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: At what pH will Fe(OH),(s) begin to precipitate from 1.35 x 10-3 M FeCl,? Ksp for Fe(OH), is 2.79 x…

Q: Ksp for Ca(OH)2 is 1.3 x 10-6. A solution has a concentration of 0.0020 M Ca2+ and 0.0040 M OH-.…

A: The solubility product constant for Ca(OH)2 is = 1.3 x 10-6 The concentration of calcium ion is =…

Q: The Ksp for CoCO3 = 1.0 × 10–10 and the Ksp for PbCO3 = 7.4 × 10–14 . When Na2CO3 is added dropwise…

A: Given : Ksp of CoCO3 = 1.0 X 10-10 Ksp of PbCO3 = 7.4 X 10-14 Concentration of Co2+, [Co2+ ] =…

Q: Solid Cag(PO4)2 is added to a solution of 0.080 M Na3PO4 and the system is allowed to come to…

A: Na3PO4 is a strong electrolyte and hence will dissociate completely into Na+ and PO43–. The…

Q: Will a precipitate form when 125.0 mL of 0.10 M AI(NO3)3 is combined with 25.0 mL of 0.01 M NaOH?…

A: Given that: volume of Al(NO3)3 = 125.0 mL molarity of Al(NO3)3 = 0.10 M volume of NaOH = 25.0 mL…

Q: The ksp of NiCO3 is 6.6x10-9 @ a certain temperature. If 5.0 mL of 1.7x10-5M Ni2+ ions were added to…

A: Given, The ksp of NiCO3 is 6.6x10-9 . If 5.0 mL of1.7x10-5M Ni2+ ions were added to 5.0 mL of…

Q: solid sodium sulfate, Na2SO4, is added slowly to a solution that is 1.0x10^-4 in both Ba2+ and Pb2+…

Q: At 25 °C, for Lead (II) sulphate (PbSO4), Ksp = 2.53×10-8 and for Barium sulphate (BaSO4) Ksp =…

A: Solution:

Q: The ksp of CaF2 is 3.9 x 10 -11 at 25o C. Assuming that CaF2 dissociate completely upon dissolving…

A: In a balanced chemical reaction, the product of the equilibrium concentration of the ions of the…

Q: A solution prepared in the lab contains 3.5 x 10-4 M Sr2 and 0.0010 M F-. Will a precipitate form?…

A: Given:[Sr2+] = 3.5 x 10-4 M [F-] = 0.0010 M Dissociation reaction of SrF2: SrF2(s) ⇔ Sr2+(aq) +…

Q: For nos. 36 37, consider a scenario wherein a solution containing 6.25x10-3 M of S2- and 5.63x10-3 M…

Q: 75.0-mL sample of 0.003 M AgNO3 is added to 50 mL of 0.0700 M NaIO3. Determine the ff: a. Initial…

A: Given 75.0-mL sample of 0.003 M AgNO3 is added to 50 mL of 0.0700 M NaIO3 We have to find Initial…

Q: The Ksp for CaF2 is 3.9 x 10-11 at 25 °C. Assuming equilibrium is established between solid and…

A: The solubility reaction is CaF2 (s) -------> Ca2+ (aq) + 2 F- (aq) Hence the equilibrium…

Q: A solution containing lead (II) nitrate is mixed with one containing sodium bromide to form a…

Q: 27. For PbCl2 (Ksp = 2.4 x 10-), will a precipitate of PbCl, form when 0.10 L of 3.0 x 10 M Pb(NOa)a…

A: Given that, 0.10 L of 3.0×10-2 M Pb(NO3)2 is added to 400 ml of 9.0×10-2 M NaCl. Ksp of PbCl2 =…

Q: Solid potassium chromate (K2CrO4) is slowly added to a solution containing 0.50 mol L-1 AgNO3 and…

Q: 3. A solution has [Pb2+] = 0.0012 M and [CI] = 0.010 M. Will PbCl2 precipitate form? Ksp for PbCl₂ =…

Q: For each of the following compounds, decide whether the compound's solubility in aqueous solution…

A: The compounds given are BaCO3, CaI2 and CuBr.

Q: 0.500 M Ca(NO3)2 is added to 25.0mL of 0.250 M NaF at 25°C? (Ksp of CaF2 = 5.3 X 10^-9 at 25

A: Solubility equilibrium of CaF2 CaF2(s) <----> Ca2+(aq.) + 2F-(aq.) Condition for…

Q: What is the solubility product expression for Co(OH)3? Ksp= [Co3+][30H] Ksp= 3[Co3+I[OH73 Ksp=…

Q: After mixing an execess PbCl2 with a fixed amount of water, it is found that the equilibrium…

A: First, the Ksp expression for given compound is determined.

Q: Will a precipitate form if a mixture contains (Ag+) = 1.2 x 10-4 M and (C2O4-2) = 4.7 x 10-3 M?…

A: Here, Concentration of [Ag+] = 1.2 x 10-4 M. Concentration of [C2O4-2] = 4.7 x 10-3 M. Ksp = 3.5 x…

Q: If 250.0 mL of 0.0010 M Sr(NO3)2 were added to 50.0 mL of 0.0000010 M Na2CO3 would a precipitate of…

Q: Will a precipitate form when 400.0 mL of 1.2 x 10-3 M MgCl2 are added to 300.0 mL of 1.2 x 103 M…

A: After mixing, total volume of Solution is 400+300 = 700 mL MgCl2 and NaF are strong electrolytes,…

Q: 3. Ca(OH)2(s)⇄Ca2+(aq)+2OH−(aq) Ksp=5.5×10−6 at 298K The equilibrium in a saturated solution of…

A: The equilibrium expression is, Ca(OH)2 (s) ⇄ Ca2+ (aq) + 2OH− (aq) To find the chance when the…

Q: A 75.0-mL sample of 0.00300 M AGNO3 is added to 50.0 mL of 0.0700 M NalO3. Determine the: a.Initial…

Q: Given the solubility product constants (Ksp): BaSO4 1.5 x 10-9 CoS 5.0 x 10-22 PbSO4 1.3 x 10-8 AgBr…

A: The solubility product is a kind of equilibrium constant and its value depends on temperature. Ksp…

Q: At 15 °C, the solubility product of PbCrO4 is 1.69 × 10-14 mol2dm-6. (a) Write an expression for…

A: Given, Solubility product of PbCrO4 = 1.69×10-14mol2dm6

Q: C2042-) with a ksp of 2.3 x 109 has a concentration of 1.0 x 105 M. What is the reaction quotient…

Q: For PbCl2, Ksp 1.7 x 105. What will occur if 250 mL of 0.10 M %3D Pb(NO3)2 is mixed with 250 mL of…

Q: . 200.0 mL of 0.005 M Na2CO3 are added to 200.0 mL of 0.002 M MgCl2. Does a precipitate form?…

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

: For PBC12 (Ksp = 2.4 x 10-4), will a precipitate of PbCl2 form when 0.10 L of 3.0 x 10
M Pb(NO3)2 is added to 400 mL of 9.0 x 10-2M NaC1?
O Yes, because Q> Ksp
No, because Q<Ksp
No, because Q=Ksp
Yes, because Q< Ksp

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

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 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

A 3.20-L solution of 1.25 103 M Pb(NO3)2 is mixed with a 0.80-L solution of 5.0 101 M NaCl. Calculate Q for the dissolution of PbCl2. No precipitate has formed. Is the solution supersaturated, saturated, or unsaturated?
Will a precipitate of Mg(OH)2 form when 25.0 mL of 0.010 M NaOH is combined with 75.0 mL of a 0.10 M solution of magnesium chloride?
A 45.0-mL sample of 0.0015 M BaCl2 was added to a beaker containing 75.0 mL of 0.0025 M KF. Will a precipitate form?
Silver(I) sulfate (Ksp=1.2105) is used in the electroplating of silver. A 1.0-L solution is prepared by mixing 15 g of silver nitrate with 20 g (2 significant figures) of potassium sulfate. Will a precipitate form? At what [Ag+] concentration will precipitation (if any) start?
The following solutions are mixed: 1.0 L of 0.00010 M NaOH and 1.0 L of 0.0014 M MgSO4. Is a precipitate expected? Explain.
Will a precipitate of Mg(OH)2 form when 25.0 mL of 0.010 M NaOH is combined with 75.0 mL of a 0.10 M solution of magnesium chloride?
Will a precipitate of Cd(OH)2 form if 1.0 mL of 1.0 M Cd(NO3)2 is added to 1.0 L of 5.0 M NH3? Cd2+(aq)+4NH3(aq)Cd(NH3)42+(aq)K=1.0107Cd(OH)2(s)Cd2+(aq)+2OH(aq)Ksp=5.91015
A town adds 2.0 ppm of F- ion to fluoridate its water supply. (Fluoridation of water reduces the incidence of dental caries). If the concentration of Ca2+ in the water is 3.5104 M, will a precipitate of CaF2 form when the water is fluoridated?
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) TlCl(s) in 1.250 M HCl. (b) PbI2(s) in 0.0355 M Cal2. (c) Ag2CrO4(s) in 0.225 L of a solution containing 0.856 g of K2CrO4. (d) Cd(OH)2(s) in a solution buffered at a pH of 10.995
To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
Consider a 2.0-L aqueous solution of 4.17 M NH3, where 21.0 g of NH4Cl are dissolved. To this solution, 4.8 g of CaCl2 are added. (a) What is [OH-] before CaCl2 is added? (b) Will a precipitate form? (c) What is [Ca2+] after equilibrium is established?