A solution is 0.0111 M in both Br– and SO42–. A 0.283 M solution of lead(II) nitrate is slowly added to it with a buret. The (Br- or  SO4^2-)  anion will precipitate from solution first. (Ksp for PbBr2 = 6.60 ×× 10–6; Ksp for PbSO4 = 2.53 ×× 10–8)   What is the concentration in the solution of the first anion when the second one starts to precipitate at 25°C?

Q: Part 1 hd See Periodic Tab A solution is 0.018 Min both Br and SO, A0.230 Msolution of lead(II)…

A: Solubility product: It is defined as the product of its dissolved ion concentrations raised to the…

Q: What mass of AgBr will dissolve in 500.0 mL of 5.10 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the…

A: The given formation reaction is, AgBr ionizes to give Ag+ and Br- Overall reaction is,

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Q: A solution is 0.011 Min both Br¯ and SO42.A 0.191 Msolution of lead(II) nitrate is slowly added to…

A: Answer :- Below I have explained step by step solution Hope this will really gonna help you !!!!!…

Q: Will a precipitate form when 20.0 mL of 1.8 × 10–3 M Pb(NO3)2 is added to 30.0 mL of 5.0 × 10–4 M…

A: Given data is as follows:

Q: Will a precipitate form when 3.0 mL of 0.000150 M FeBr₃ is mixed with 1.0 mL of .00030 M AgNO₃ in…

A: We will first find Qsp , then compare it with Ksp to check whether precipitate will form or not.

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A:

Q: A solution is 1×10-4 M in NaF, Na,S, and Na3PO4 What would be the order of precipitation as a source…

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Q: What is the molar solubility of Ag2SO4 in a solution that is 0.0522 M H2SO4? Ksp= 1.40x10^-5

A:

Q: Solid Na2 SO4 is added slowly to a solution that is 0.40M in Pb(NO3), and 0.75M in Ba (NO3)2. In…

A: Given:  Concentration of Pb(NO3)2 = 0.40 M  Concentration of Ba(NO3)2 = 0.75 M  Ksp(PbSO4) = 1.8 x…

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A:

Q: 9. A flask containing 0.10 M NaCl (aq) and 0.010 M K₂CrO4 (aq) has some solid AgNO, added to it. Ksp…

A: #9: 1 mol NaCl is completely dissociated to give 1 mol Cl-(aq). Hence [Cl-(aq)] = [NaCl] = 0.10 M  1…

Q: What is the minimum concentration of KOH required for precipitation to begin in a solution of 0.0150…

A: Since the CaCl2 is completely soluble in water  Hence CaCl2 ------> Ca2+ + 2 Cl-  Since 1 mole or…

Q: What is the molar solubility of Ag2SO4 in a solution that is 0.0522 M AgNO3? Ksp= 1.40x10^-5

A:

Q: A roll of 35-mm black and white photographic film contains about 0.27 g of unexposed AgBr before…

A:

Q: The molar solubility of AgCl is 1.33 x 10-5 M. Ksp=? ANS: [Ag+ ] = [Cl- ] = 3.65 x 10-3 M   -…

A:

Q: What you expect to observe on mixing 0.1M Zn(CO3)2 with 3M H2SO4. Will there be a color? Will…

A: The question is based on qualitative analysis. we have to describe the observations taking place.

Q: The solubility product constant of barium fluoride in water at 25o C is Ksp = 1.3 x 10-6. Calculate…

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Q: What is the molar solubility of AgCl (Ksp = 1.80 × 10-10) in 0.770 M NH3? (Kf of Ag(NH3)2* is 1.7 x…

A:

Q: When solid BaF, is added to pure water at 25 ° C, the salt dissolves until the concentration of Ba2+…

A: The dissociation of BaF2 is ,                        BaF2s↔Ba2+aq + 2F-aq The solubility of Ba2+ is…

Q: Explain what happen to undissolved solid PBI: in a beaker containing saturated solution of PbI: in…

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Q: Sufficient sodium cyanide, NaCN, was added to 2.5x10^-2 M silver nitrate, AgNO3, to give a solution…

A: Given: Molarity of AgNO3 = 2.5×10-2 MMolarity of CN- ion = 0.193 MKf for Ag(CN)2- = 5.6×1018

Q: A solution contains 0.030 M Zn2 and 0.044 M Fe2 A solution containing sulfide lons is added to…

A: The solubility product of salt is a constant at a given temperature irrespective of the source from…

Q: Copper(I) ions in aqueous solution react with NH3(aq) according to Cu+ (aq) + 2NH3(aq) -…

A: Given: The solubility constant of CuBr is 6.3×10-9. The concentration of NH3 is 0.87 M. The…

Q: A solution has a Fe2+ concentration of 5.0 x 10-3M.   What is the minimum concentration of CO32- ion…

A: In a saturated solution, the molar solubility of salt is used to determine the solubility product.…

Q: The molar solubility of Cu(OH)2 in H2O is 1.8 x 10-7 while that of Pb(OH)2 is 6.7 x 10-6. If sodium…

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Q: At what pH wil a 0.00201 M FeCl2 solution begin precipitating Fe(OH)2? (Ksp = 1.6 x 10-14)

A:

Q: A solution is 0.10 M in Pb(NO3)2 and 0.10 M in AgNO3.  Solid NaI is added until the second solid…

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A:

Q: Although AgCN(s) is very insoluble (Ksp = 2.20 × 10⁻¹⁶), it will dissolve in higher concentrations…

A: Solubility equilibrium for AgCN is given as: AgCN(s)⇔Ag+(aq)+CN-(aq)   -----(1)

Q: What is the molar solubilty of AgBr in 0.010M NaBr solution. Ksp = 5.0x10^-13 Agbr ⇌ Ag+ + Br-

A: Given data :- Concentration of NaBr solution = 0.010M Ksp = 5.0 x 10-13

Q: What is the molar solubility of nickel(II) sulfide in: a) Pure water b) 1.79x10-3 M nickel(II)…

A: a) Pure water: Ksp = [Ni2+] [S2-]         =[ X × X] 3×10-19 = X2 X =( 3×10-19)1/2 X = 5.477×10-10 M…

Q: The solubility of Ag2CrO4 (Ksp = 1.2 x 10-12) is several times greater than that of AgCl (Ksp = 1.82…

A: Given: Mass of K2CrO4 = 1 mg Ksp  Ag2CrO4 = 1.2 x 10-12 Ksp  AgCl  = 1.82 x 10-10 To determine: The…

Q: A student mixes 33.0 mL of 2.94 M Pb(NO,),(aq) with 20.0 mL of 0.00217 M Na, SO,(aq). How many moles…

A:

Q: At what pH will Fe(OH)₃(s) begin to precipitate from 3.25 × 10⁻³ M FeCl₃? Ksp for Fe(OH)₃ is 2.79 ×…

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Q: Given that the average concentration of calcium ion in natural waters is 3.8x10⁻⁴ M, and that the…

A:

Q: Calculate the solubility of lead(II) iodide, PbI2, in 0.025 M KI. For PbI2, Ksp= 7.9x10^-9

A: Given :  Concentration of KI = 0.025 M  Ksp of PbI2 = 7.9 x 10-9

Q: At what pH will Fe(OH),(s) begin to precipitate from 5.15 x 10³ M FeCl,? Ksp for Fe(OH), is 2.79 x…

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

Q: silver sulfate

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Q: ?What is the molar solubility, s, of Ba3(PO4)2 in terms of Ksp s = [Kgp/108]/5 a O S = Kg/2 b O S =…

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Q: What mass of AgBr will dissolve in 500.0 mL of 1.35 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the…

A: The two equations as per the question along with their rate constants are given below:- Ag+(aq)    +…

Q: What is the molar solubility of silver iodide, Agl, in 0.0325 M -17. CH;NH;? For AgI Ksp = 8.52 x 10…

A:

Q: Q1) In titration of the solution containing 0.1 Molar of l'and 0.1 Molar of Cro, , with the solution…

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Q: 16. Equal volumes of 0.020 M Ag+ solution and 2.0 M NH3 solution are mixed. Kf for [Ag(NH3)2]+ is…

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Q: A solution contains 5.61×10 M silver acetate and 5.52x10 M calcium nitrate. Solid sodium sulfite is…

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Q: 8. Calculate the ion product constant for mixing 100.0 mL of 0.003 M CaCI, with 100.0 mL of .0020 M…

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Q: What mass of AgBr will dissolve in 500.0 mL of 5.90 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the…

A: The overall reaction for the solubility of AgBr in ammonia can be written as follows:

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Q: What is the concentration of iodate in a 0.025 M Ba3(PO4)2 1eu uonnı barium iodate, Ba(1O3)2 ? (Ksp…

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Q: What is the molar solubility of Ca(OH)2 in the presense of dissolved Cacl2 if the volume of the…

A: Ca(OH)2 dissolves as: Ca(OH)2 (s) = Ca2+ (aq) + 20H- (aq) So, Ksp = [Ca2+ ][01-112 , where [..]…

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