Concept explainers
On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are not likely to be soluble in water. Indicate which specific rule(s) led to your conclusion.
:math>
:math>
:math>
:math>
Trending nowThis is a popular solution!
Chapter 7 Solutions
Introductory Chemistry: A Foundation
- One way to reduce the presence of lead in water is to add a phosphate corrosion inhibitor, which forms an insoluble saltwith lead, coating the pipes with a protective mineral later: Pb3(PO4)2(s) ⇌ 3Pb2+(aq) + 2PO43-(aq) Kc=9.9 x 10-55 a.) Calculate the solubility of lead (Pb2+) in g/L when Pb3(PO4)2 is dissolved in water. b.) The acceptable level of lead in water is less than 1x10-6g/L. If phosphate is added to drinking water, does it keep the lead levels below the allowed limit? c.) In 2014, the city of Flint, MI, changed water sources to a system that didn’t include phosphate. Instead, it used chlorine to treat water. The Ksp of lead chloride is 1.5x10-5. The switch increased the levels of lead in the drinking water and significantly affected the community. Explain why switching water sources increased the lead levels in Flint’s drinking water.arrow_forwardA 50.00 mL solution containing NaBr was treated with excessive AgNO3 to precipitate 0.214 6g of AgBr (FM 187.772). What was the Molarity of NaBr in the solution?arrow_forwardWhen lead(II) fluoride (PbF2) is shaken with pure water at 25°C, the solubility is found to be 0.64g/L. Calculate the Ksp of PbF2.arrow_forward
- Suppose 234.3 mg of PbCl2 was added to 16.0 mL of water in a flask, and the solution was allowed to reach equilibrium at 21.0 oC. Some solute remained at the bottom of the flask after equilibrium, and the solution was filtered to collect the remaining PbCl2, which had a mass of 91.6 mg . What is the solubility of PbCl2 (in g/L)? -Express the concentration in grams per liter to three significant figures.arrow_forwardGiven the solubility, calculate the solubility product constant (Ksp) of each salt at 25°C: (a) Ag2SO3, s = 4.6 ×10−3 g/L (b) Hg2I2, s = 1.5 ×10−7 g/L (c) Zn3(PO4)2, s = 5.9 × 10−5 g/Larrow_forwardA solution of I3- was standardized by titrating freshly dissolved arsenious oxide (As4O6, FM 395.683). The titration of 25.00 mL of a solution prepared by dissolving 0.3663 g of As4O6 in a volume of 100.0 mL required 31.77 mL of I3-. Calculate the molarity of the I3- solution. As4O6(s) + 6H2O ⇌ 4H3AsO3 H3AsO3 + I3- + H2O ⇌ H3AsO4 + 3I- + 2H+ a. 0.01657 M b. 0.02914 M c. 0.1166 M d. 0.0957 Marrow_forward
- Consider the Solubility Curve for this Problem: Analysis for KClO3 & NH4Cl MW (KClO3) = 122.55 g/mol , MW (NH4Cl) = 53.49 g/mol i) What is the temperature at which KClO3 & NH4Cl both have the same solubility? Round to nearest degree. +/- 1° T = °C ii) What is the solubility (g per 100g H2O) at this temperature. Round to nearest gram. +/- 1 g s (KClO3) = g/100g H2O s (NH4Cl) = g/100g H2O iii) What is the molar solubility for KClO3 at this temperature? Assume the density of the solution is 1.21 g/cc. Round off to 2 sig. figs. |s| KClO3 = M iv) Calculate the Ksp for each of these chemicals at this temperature. Ksp = v) What is the unit of Ksp for KClO3? Unit for Ksp =arrow_forward4. Ascorbic acid (Vitamin C, MW = 176.126g/mol) is a reducing agent, reacting as follows: C6H8O6 C6H6O6 + 2H+ + 2e- It can be determined by oxidation with a standard solution of I2. A 200.0-mL sample of a citrus fruit drink is acidified, and 10.00mL of 0.0500 M I2 is added. After the reaction is complete the excess I2 is titrated with 38.62 mL of 0.0120 M Na2S2O3 . Calculate the number of milligrams of ascorbic acid per milliliter of fruit drink. I2 +2e 2I- I2 + 2Na2S2O3 2NaI + Na2S4O6arrow_forward(a) If the molar solubility of Cd3(AsO4)2 at 25 oC is 1.15e-07 mol/L, what is the Ksp at this temperature?Ksp = __________(b) It is found that 8.90e-06 g of Y2(CO3)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Y2(CO3)3.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3? solubility = ________mol/Larrow_forward
- A sample of freshly precipitated and filtered silver chloride weighs 459.0 mg. If 1.00 % of the silver chloride becomes photo decomposed, what is the precipitate’s weigh?arrow_forwardI need help calculating the solubility. thank you C. Calcium Fluoride, CaF2 (aka, Fluorite), in a solution containing 19 mg/L of LiF (aka, Griceite),with all of the LiF being dissolved into solution. Please assume that LiF dissolves such that [Li] =[F] = 7.33 x 10-4 m. After adding CaF2 to the solution and allowing it to dissolve, what are finalvalues of [Ca], [Li] and [F]?Note: you are given the concentrations of [Li] and [F] that result from dissolving LiF. Nosolubility calculation is required for dissolving LiF; just use the concentration given above.Steps:- First, write the stoichiometric equation for dissolution of CaF2 , with the solidon the left and the two ions in solution on the right, separated by a "two-way" arrow. Hint: whenCaF2 dissolves, you get 2 moles of F for every 1 mole of Ca.- Second, set up a law of mass action equation for dissolution of CaF2. There is a common ioneffect for F, so if [Ca] = x, then [F]= 2x + [FLiF], where [FLiF] is from dissolution of the…arrow_forwardA K2SO4•Al2(SO4)3•24H2O preparation is tested for its purity by converting first to Al(OH)3 then finally to Al2O3. If you start with a 1.2391 g K2SO4•Al2(SO4)3•24H2O and obtained 0.1357 g Al2O3(A). What can you say about the obtained purity value? Is it acceptable?(B). Which is a better choice of precipitate for the quantitative analysis of K2SO4•Al2(SO4)3•24H2O, Al(OH)3 or Al2O3? Explainarrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning