Cations of barium, calcium, magnesium, and strontium are each reacted with anions of sulfate, carbonate, oxalate, and iodate. It is observed that some of these cations form insoluble precipitates when reacted with the anions. Rank the cations in order from most soluble (1) to least soluble (4) Ca2+, Sr2+, Ba2+, Mg2+

Q: Calcium oxalate, CaCO4, is very insoluble in water. What mass of sodium oxalate,Na2C2O4, is required…

A: Given: Volume of CaCl2 = 37.5 ml Molarity of CaCl2 = 0.104M

Q: A solution contains 9.92x10-3 M ammonium carbonate and 9.27x103 M sodium hydroxide. Solid iron(II)…

A:

Q: A student weighs out 1.215 g of an impure KHP, dissolves the sample in 100. mL DI water and titrates…

A: kindly find the answer attached

Q: A student adds KF to 867 mL of a 0.0020 M Mg(NO3)2 solution. What is the minimum quantity of moles…

A: the solubility product at standard condition is the product of ions formed when a sparingly soluble…

Q: Some soluble compounds are listed in the table below. Complete the table by filling in the name or…

A: Ionic bonds occur between two species which are electrostatically attracted towards each other.…

Q: Suppose that 0.323 g of an unknown sulfate salt is dissolved in 50 mL of water. The solution is…

A: 1 mole Ba2+ ion react with 1 mole SO42- ion to form 1 mole BaSO4.Precipitation reaction is

Q: Predict the precipitate formed (if any) when aqueous solutions of the following substances are…

A: First we need to write the reaction between given reactants as per solubility rules. A precipitate…

Q: A solution of HCl is prepared by an unknown dilution of concentrated HCl. It is standardized by…

A: #1: Three different samples of the unknown HCl solution are prepared and titrated using Na2CO3(s) as…

Q: 200. mL of 0.50 M NaCl and 800. mL of 0.100 M AgNO3 are mixed together. Calculate the mass of the…

A: Double displacement reactions are basically the reactions in which exchange of various ions takes…

Q: Consider the reaction of a 20.0 mL of 0.220 M CSH»NHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.241 M…

A: A net ionic equation is written excluding the spectator ions from the corresponding total ionic…

Q: Which of the following are soluble in water?  NaCl, BaCl2, Ca(NO3)2, ammonium carbonate, sodium…

A: The solubility of a compound in water follows the rule of like dissolves like. Water is a polar…

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: A solution contains 0.0430 M Ca2+ and 0.0970 M Ag+. If solid Na3PO4 is added to this mixture, which…

A: The objective of this question is to determine which of the phosphate species would precipitate…

Q: A solution is 0.010 M in both Br- and SO42-. A 0.250 M solution of lead (II) nitrate is slowly added…

A: we need to find the solubility product constant (Ksp) for the precipitation reaction and calculate…

Q: scientist is investigating the solubility of two polyatomic ions, oxalate (C2O2−4C2⁢O42−) and…

A:

Q: 6. A buffer is prepared by adding 20.0 g of sodium acetate (CH3COONa) to 500 mL of a 0.150 M acetic…

A:

Q: Calculate the maximum solubility of calcium fluoride, CaF2 in g/L when in the presence of 0.077 M…

A:

Q: Calculate the maximum solubility of silver carbonate, Ag2CO3 in g/L when in the presence of 0.055 M…

A:

Q: A solution contains 7.27x103 M lead nitrate and 1.16×10²M calcium acetate. Solid ammonium sulfate is…

A:

Q: A 160.0 mL solution of 3.041 M strontium nitrate is mixed with 205.0 mL of a 3.340 M sodium fluoride…

A: Given reaction is                                    Sr(NO3)2                 +                2…

Q: A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass…

A: Given, Mass of KHP =0.7840 g Initial reading of burette=0.8400 mL Final reading of burette = 39.20…

Q: A solution contains 1.39x102 M sodium phosphate and 1.11×10-2 M sodium fluoride. Solid calcium…

A: Given: Concentration of sodium phosphate i.e. Na3PO4 = 1.39 × 10-2 M. And the concentration of…

Q: Will the following reaction yields a precipitate? yes or no   Pb(NO3)2(aq)  +  NaC2H3O2(aq) ->

A: The precipitation reactions are the reactions involving the formation of insoluble solid product,…

Q: A solution contains 1.19x102 M ammonium carbonate and 1.39×102M sodium sulfide. Solid nickel(II)…

A: Precipitation occurs when ionic product is greater than solubility product  Thus among two…

Q: You mix 275.0 mL of 1.20 M Pb(NO3)2 with 300.0 mL of 1.85 M KI. Calculate the mass of precipitate.

A: Given data : Concentration of Pb(NO3)2 = 1.20 M Volume of Pb(NO3)2 = 275 mL Concentration of KI =…

Q: A student is preparing 250 mL of a solution of 155.0 mM NaCl in 50.0 mM phosphate pH 6.4.  The…

A: First, we have to find the moles (or millimoles, mmol) of phosphate present in the 250 mL of 50.0 mM…

Q: A solution contains 1.44×102 M sodium carbonate and 1.08×102 M ammonium sulfide. Solid manganese(II)…

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

Q: With the given plot, if a 0.1000 M NaOH solution was used to fully precipitate all the Zn2+ in the…

A: Answer: In this question we have to convert moles of NaOH into moles of Zn2+ ion to find out the…

Q: What is the chemical equation representing the titration reaction?

A: A) As here , acid is HCl and base is NaOH , and both are strong in nature , so the reaction they…

Q: 2. * A sodium hydroxide solution is standardized by titrating 0.8592 g of ordinary standard…

A: Given that:                              Weight of Potassium Hydrogen pthalate (KHP) = 0.8592gMolar…

Q: A 10.00 mL portion of an HCl solution required 11.01 mL of 0.09883 M NaOH to reach an end point with…

A:

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