Which of the following could be used to separate Pb²+ from Ba²+ by precipitation?CATIONSHighSolubility(aq)LowSolubility(s)Na3PO4Na₂SO4NaOHNa₂CO3Cl, Br, I-HalidesNaNO3MostAg+, Pb²+,Tl+, Hg₂2+,Hg, CuS2-Solubility TableGroup 1,NHÀ,Group 2MostANIONSOHGroup 1,NH4*, Sr²*,Ba²+, TlMostSO4²-MostAg+, Pb²+,Ca²+, Ba²+,Sr²+, Ra²All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility inwater.CO3²-,PO4³¹,SO3².C₂H302 NO3Group 1, Most AllNH4*Most Ag+ None

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High Solubility (aq) Low Solubility (s) Cl-, Br, I- Halides Most Ag+, Pb²+, Tl, Hg²+, Hg", Cu 52- Group 1, NHÀ, Group 2 Most ANIONS OH- Group 1, NH4*, Sr²+, Ba²+, Tl. Most SO4²- Most Ag", Pb²+, Ca²+, Ba²+, Sr²+, Raz CO3²-, PO4³¹, SO3²- C₂H30₂ NO3 Group 1, Most All NH4* Most Ag None roup 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in -

High Solubility (aq) Low Solubility (s) Cl-, Br, I- Halides Most Ag+, Pb²+, Tl, Hg²+, Hg", Cu 52- Group 1, NHÀ, Group 2 Most ANIONS OH- Group 1, NH4, Sr²+, Ba²+, Tl. Most SO4²- Most Ag", Pb²+, Ca²+, Ba²+, Sr²+, Raz CO3²-, PO4³¹, SO3²- C₂H30₂ NO3 Group 1, Most All NH4 Most Ag None roup 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in -

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 57QAP: Calcium ions in blood trigger clotting. To prevent that in donated blood, sodium oxalate, Na2C2O4,...

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A solution is 1.5 104 M Zn2 and 0.20 M HSO4. The solution also contains Na2SO4. What should be the minimum molarity of Na2SO4 to prevent the precipitation of zinc sulfide when the solution is saturated with hydrogen sulfide (0.10 M H2S)?
Calcium ions in blood trigger clotting. To prevent that in donated blood, sodium oxalate, Na2C2O4, is added to remove calcium ions according to the following equation. C2O42(aq)+Ca2+(aq)CaC2O4(s)Blood contains about 0.10 mg Ca2+/mL. If a 250.0-mL sample of donated blood is treated with an equal volume of 0.160 M Na2C2O4, estimate [Ca2+] after precipitation. (KspCaC2O4=4109)
A solution consists of 0.050 M Mg2+(aq) and Cu2+(aq).Which ion precipitates first as OH-(aq) is added? Whatconcentration of OH-(aq) is necessary to begin the precipitationof each cation? [Ksp = 1.8 x 10-11 for Mg(OH)2, andKsp = 4.8 x 10-20 for Cu(OH)2.]
How will the following sitations affect the final calculation of the molarity of HC2H3O2? The end point of the vinegar titration was surpassed. (excess NaOH was added.)
A student was performing this experiment with an antacid tablet which contained C a CO3 but forgot to heat the antacid solution prior to starting the back-titration. As sodium hydroxide was added the student noticed the formation of an insoluble white precipitate. Would the presence of this precipitate cause the students experimentally determined volume of N a O H be incorrectly high or incorrectly low? Briefly explain. Hint: Carbon dioxide reacts with water to form carbonic acid. Question 3 options: Incorrectly high, the solution becomes more acidic if not boiled gently Incorrectly high, the solution becomes less acidic if not boiled gently Incorrectly low, the solution becomes more acidic if not boiled gently Incorrectly low, the solution becomes less acidic if not boiled gently
Benzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. C6H5COOH(s) -> C6H5COO–(aq) + H+(aq) Ka = 6.46 x 10^-5 Calculate the pH of the solution after the following amounts of NaOH have been added… A. 0 mL B. 10 mL C. 85 mL
Le Châtelier’s Principle is described in terms of adding/removing reactants or products. While it is easy to add reactants/products, describe how you were able to remove reactants/products from the equilibria by using the procedures in this experiment. What are the net ionic equations as appropriate for: The following reaction is examined:HSO4¯ (aq) + H2O (l) ⇌ SO42¯ (aq) + H3O+ (aq) Obtain about 5 mL (one small test tube) of “NaHSO4 solution” and “Na2SO4 solution” in two appropriately labeled test tubes. In a well plate, take 10 drops of NaHSO4 into wells A1, A2 and A3, and 20 drops to wells A4 and A5 using a pipet. Add 1 drop of Thymol Blue indicator solution to wells A1 to A5. Thymol Blue is red in very acidic solution, and changes from red to yellow between pH 1.2-2.8. Add one drop of Na2SO4 to well A1. Continue to add drops of Na2SO4 to well A1 until you see a color change, making sure to mix the solution after the addition of each drop (do not use the pipet tip to mix the…
Suppose that 150 mL of 0.200 M K2CO3 and 100 mL of 0.400 M Ca(NO3)2 are mixed together. Assume that the volumes are additive, that CaCO3 is completely insoluble, and that all other substances that might be formed aresoluble. Calculate the mass of CaCO3 precipitated, and calculate the concentrations in the final solution of the four ions that were present initially.
Benzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. C6H5COOH(s) ⇄ C6H5COO–(aq) + H+(aq) Ka = 6.46 x 10–5 a.Calculate the pH of the solution after the following amounts of NaOH have been added… 0 mL 10 mL 85 mL b. State whether the solution at the equivalence point of the titration is acidic, basic, or neutral. Explain your reasoning. c. How many mL of 0.25 M NaOH need to be added in order to make the ideal buffer solution?
In the experiment conducted to determine the amount of acetic acid in vinegar, 8.2 mL of NaOH standard solution adjusted to 0.098 M was spent besides the phenolphthaleley indicator. Accordingly, which of the following is the amount of acetic acid in the vinegar sample in grams? (Ma (CH3COOH): 60.05 g / mol)
Which of the following are not water-soluble: Ba(NO3)2, FeCl3, CuCO3, CuSO4, Zns, and ZnSO4?
PH of diluted calcium hydroxide=7.01 1.) Hydronium ion concentration in dilute solution,M? 2.)Hydroxide ion concentration in diluted solution, M? M1 V1= M2 V2 V1=100mL V2=5mL saturated solution M1=#2 Hydroxide in concentration in saturated solution,M? Calculate solubility product of calcium hydroxide

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