A solution contains 2.0 x 10-4 M Ag+ and 1.5x10-3 M Pb2+ . If KI is added, will AgI (Ksp = 8.3 x 10-17) or PbI2 (Ksp = 7.9 x 10-9 ) precipitate? What are the specific concentrations of I - needed? ANS: AgI will precipitate out first.           [I- ] for AgI = 4.2 x 10-13 M           [I- ] for PbI2= 2.3 x 10-3 M

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Q: 44. In which solution will 0.0010 M AgNO3 form a precipitate? a. 2.0x10-7M NaCl (Ksp of…

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Q: Asolution contains 0.45 M HA ( K. - 1.0x10 and 0.45 M NaA. What is OplI after 0.25 mole of HCI is…

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Q: Lead (II) Bromide is a slightly soluble solute in water. The following equation represents the…

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Q: Consider these slightly soluble salts: 1. PbS Ksp = 8.4 x 10-28 2. PbSO4 Ksp = 1.8 x 10-8 3.…

A: Given data, Ksp of PbS = 8.4 x 10-28 Ksp of PbSO4 = 1.8 x 10-8 Ksp of Pb(IO3)2 = 2.6 x 10-13

Q: 96 mL of 0.080 M NaF is mixed with 32 mL of 0.20 M Sr(NO3)2. Calculate the concentration of Sr2+ in…

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

A: Given that

Q: (a) I f t he molar solubilit y o f CaF2 at 35 °C i s1.24 x 10-3 mol/L, what is Ksp at this…

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Q: Calculate the solubility of HgI2 in 0.25 M KI. K sp (HgI2) = 4.0 × 10-29 at 25 °C.

A:

Q: The Ksp of AgI is 8.5 ´ 10–17 at 25 °C. Calculate the molar solubility of AgI in 0.0045 M KI(aq) at…

A: answer : KI is a strong electrolyte, so it will be present in a completely dissociated form in…

Q: If 5.00 mLof 0.200 M Na2SO4 are added to 1.00 L of 0.100 M BaCl2, will a precipitate form? Ksp of…

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Q: The Ksp of PbBr, is 6.60 × 10-6. What is the molar solubility of PbBr, in pure water? molar…

A:

Q: A solution of Na3PO4 is added dropwise to a solution that is 0.0194 M in Ca2+ and 5.86e-05 M in…

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Q: If 10.0mL of 2.0x10^-3 M Cr(NO3)3 is added to 10.0mL of a pH = 10.0 NaOH solution, will a…

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Q: MISSED THIS? Read Section 18.6 (Pages 823 - 826) ; Watch IWE 18.12. Part B Consider a solution that…

A:

Q: When  600 mL of 8.2 × 10− 6 M Ba(NO3)2 is added to 600 mL of 6.2 × 10− 7 M Na2CrO4, no precipitate…

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

Q: The solubility-product constant for PbI2 is 7.1x10-9 . Calculate the weight (in gram) of PbI2 that…

A:

Q: Solid NaI is slowly added to a solution that is 0.011 M in Cu* and 0.011 M in Ag* (a) Which compound…

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Q: Determine is a precipitate  of Ca3(PO4)2 will form when 100.0 mL of a 2.0x10-6M solution of CaCl2 is…

A: Ionic product  = [Ca2+]3[PO43-]2 Precipitation will form when     KSP < ionic product

Q: 50mL of 0.025 M HF is titrated with 0.045 M NaOH. a) What amount of NaOH is required for…

A: amount of NaOH is required for equivalency point = 27.77 mL

Q: The Ksp of PbBr2 is 2.1 × 10-6 at 25 °C.  Calculate the solubility of PbBr2 in mg/mL of solution.

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Q: A solution of Na;CO, is added dropwise to a solution that is 0.0177 M in Nd and 2.38e-08 M in Hgz.…

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Q: Exactly 1 litre of solution contains 0.016 mole of Co²+ ions and 0.0016 mole of Fe2+ ions. You wish…

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Q: SHOW COMPLETE SOLUTION* Suppose that we have a solution that is 0.0010 M Cland 0.100 M CrO4 2- . If…

A:

Q: Calculate the molar solubility of AuBr3 (Ksp = 4.0 × 10-36 at 25 ºC). A. 2.0×10-18 M B. 6.2×10-10 M…

A:

Q: A solution is prepared by mixing 150.0 mL of 1.0 * 10-2 M Pb(NO3)2 and 75.0 mL of 1.5 * 10-3 M NaF.…

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Q: Ben conduct two titration experiments regarding solubility equilibria. In the first titration, he…

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Q: Will a precipitate of AgBr form, when 300 mL of 5.0 × 10−5 M AgNO3 is added to 200 mL of 2.5 × 10−7…

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Q: Calculate the molar solubility of MX (Ksp = 1.27 * 10 - 36) in each liquid or solution.a. pure…

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Q: KI(aq) is slowly added to a solution with [Pb2+] = [Ag-] = 0.10 M Ksp values: AgI = 8.5 x 10⁻17…

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Q: What is the molar solubility (in mol/L) of 3.41.10-103.41.10-10) in a 0.49 PbCl2 (Ksp = M NaCl…

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Q: TRUE or FALSE 8. Blood uses a buffer bicarbonate ions and carbonic acid. 9. PbSO4 will precipitate…

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A: When Cu3(AsO4)2 gets ionized, three moles of Cu2+ and 2 moles of AsO43- is generated. Rearrange for…

Q: What is the solubility (in mol/L) of silver chromate in 1.10 M potassium chromate aqueous solution?…

A: Reaction involved:- Ag2CrO4 = 2Ag+ + CrO42-

Q: combine 500 ml of 0.01 M lead nitrate with 500 ml of 0.01M hydrochloric acid. Ksp of PbCl2 = 1.17 ×…

A: When the product of [Pb2+][Cl-] exceeds the Ksp  values then precipitation takes place .

Q: A solution contains 0.018 mole each of I-, Br-, and Cl-. When the solution is mixed with 200. mL of…

A:

Q: A sample solution contains two unknown ions. A student did a series of tests on the solution, in the…

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Q: A solution containing 0.21 M each of F , CI", CrO}-, and SO? is titrated by a solution containing…

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Q: Silver nitrate is added to a solution of 1 x 10-2 M sodium acetate (Ksp AgC2H3O2 = 1.9 x 10-3): a)…

A: Concentration of acetate ion = 1 x 10-2 M sodium acetate Ksp AgC2H3O2 = 1.9 x 10-3

Q: AlpQLSfDoHSTx3St-UM4bnqMxleBdEx_zV4qcU5T5gr2maeyKTyW5g/formResponse A solution of 0.25 mol HF…

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Q: assume that 200 ml of 0.8 M KCl solution is mixed with 300 ml of 0.01 M AgNO3 solution. Knowing that…

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Q: A 0.20 M sodium chloride solution is slowly added to a solution containing 0.40M Pb2* and 0.40 M Ag*…

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Q: Solid NaI is slowly added to a solution that is 0.010 M in CuI (Ksp = 5.1 x 10-12 ) and 0.010 M in…

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Q: When  600 mL of 8.2 × 10− 6 M Ba(NO3)2 is added to 600 mL of 6.2 × 10− 7 M Na2CrO4, no precipitate…

A: Answer:- This question is answered by using the simple concept of calculation of reaction quotient…

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