08:17Introduction to solubility equilibria | Equilibrium | AP Chemistry | Khan AcademyKhan Academy418views
Multiple ChoiceDetermine the molar solubility of CaCO3 in a solution of 0.500 M Na2CO3. Ksp for CaCO3 is 4.96 × 10−9.518views
Multiple ChoiceWhat is the molar solubility of PbBr2 in pure water? Ksp for PbBr2 is 4.67 × 10−6.738views
Multiple ChoiceSolubility of Sn(OH)2 was found to be 1.11 x 10-9 M; calculate Ksp of this compound.348views2rank
Multiple ChoiceIf a saturated solution of Ag2CO3 contains 2.56 × 10−4 M of Ag+ ions, determine its solubility product constant.255views1rank1comments
Multiple ChoiceWhat is the solubility of CN− ions in a solution of 5.5 M Hg2(CN)2, with a Ksp of 5.0 × 10−40?195views1rank
Textbook QuestionWhat is the solubility-constant expression for Ca3(PO4)2 (s)? (a) [Ca2+]3 [PO43-]2 (b) [Ca2+]3 [PO43-]2 / [Ca3(PO4)2] (c) [Ca(PO4)2] / [Ca2+]3 [PO43-]2 (d) [Ca2+]2 [PO43-]3972views
Textbook Question(b) Write the expression for the solubility-product constant for each of the following ionic compounds: Cu31PO422.702views
Textbook Question(a) True or false: 'solubility' and 'solubility-product constant' are the same number for a given compound.922views
Textbook Question(a) I f t he molar solubility of CaF2 at 35 C i s 1.24 * 10-3 mol>L, what is Ksp at this temperature?1069views1rank
Textbook Question(b) If 0.0490 g of AgIO3 dissolves per liter of solution, calculate the solubility-product constant.950views
Textbook QuestionA 1.00-L solution saturated at 25 C with calcium oxalate 1CaC2O42 contains 0.0061 g of CaC2O4. Calculate the solubility-product constant for this salt at 25 C.1143views
Textbook QuestionA 1.00-L solution saturated at 25 C with lead(II) iodide contains 0.54 g of PbI2. Calculate the solubility-product constant for this salt at 25 C.635views
Textbook QuestionCalculate the minimum pH needed to precipitate Mn1OH22 so completely that the concentration of Mn2 +1aq2 is less than 1 mg per liter [1 part per billion (ppb)].1104views
Textbook QuestionWrite balanced equations and expressions for Ksp for the dissolution of each ionic compound. c. Ag2CrO4709views1rank
Textbook QuestionWrite balanced equations and expressions for Ksp for the dissolution of each ionic compound. b. PbBr2335views
Textbook QuestionWrite balanced equations and expressions for Ksp for the dissolution of each ionic compound. a. BaSO4921views
Textbook QuestionRefer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. a. AgBr1282views
Textbook QuestionUse the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27 * 10 - 11 M476views
Textbook QuestionUse the given molar solubilities in pure water to calculate Ksp for each compound. b. PbF2; molar solubility = 5.63 * 10- 3 M2184views1rank
Textbook QuestionUse the given molar solubilities in pure water to calculate Ksp for each compound. b. Ag2SO3; molar solubility = 1.55 * 10- 5 M855views
Textbook QuestionUse the given molar solubilities in pure water to calculate Ksp for each compound. a. BaCrO4; molar solubility = 1.08 * 10- 5 M1042views
Textbook QuestionThe precipitation of Al(OH)3 (Ksp) = 1.3x10-33) is sometimes used ot purify water. (a) Estimate the pH at which precipitation of Al(OH)3 will begin if 5.0 lb of Al2(SO4)3 is added to 2000 gal of water1640views
Textbook QuestionTwo compounds with general formulas AX and AX2 have Ksp = 1.5 * 10 - 5. Which of the two compounds has the higher molar solubility?1040views
Textbook QuestionConsider the compounds with the generic formulas listed and their corresponding molar solubilities in pure water. Which compound has the smallest value of Ksp? a. AX; molar solubility = 1.35 * 10 - 4 M b. AX2; molar solubility = 2.25 * 10- 4 M c. A2X; molar solubility = 1.75 * 10 - 4 M921views
Textbook QuestionThe solubility of copper(I) chloride is 3.91 mg per 100.0 mL of solution. Calculate Ksp for CuCl.1338views
Textbook QuestionCalculate the molar solubility of barium fluoride in each liquid or solution. a. pure water788views
Textbook QuestionLead(II) carbonate, PbCO3, is one of the components of the passivating layer that forms inside lead pipes. (d) The EPA threshold for acceptable levels of lead ions in water is 15 ppb. Does a saturated solution of lead(II) carbonate produce a solution that exceeds the EPA limit?1148views
Textbook QuestionFor each pair of compounds, use Ksp values to determine which has the greater molar solubility: (b) PbCO3 or BaCrO4.770views
Textbook QuestionFor each of the following compounds, write a balanced net ionic equation for the dissolution of the compound in water, and write the equilibrium-constant expression for Ksp. (d) Hg2Cl2444views
Textbook QuestionThe solubility of CaCO3 is pH dependent. (b) Use the Kb expression for the CO32 - ion to determine the equilibrium constant for the reaction CaCO31s2 + H2O1l2 ΔCa2 + 1aq2 + HCO3-1aq2 + OH-1aq21542views
Textbook QuestionTooth enamel is composed of hydroxyapatite, whose simplest formula is Ca51PO423OH, and whose corresponding Ksp = 6.8 * 10-27. As discussed in the Chemistry and Life box on page 746, fluoride in fluorinated water or in toothpaste reacts with hydroxyapatite to form fluoroapatite, Ca51PO423F, whose Ksp = 1.0 * 10-60. (a) Write the expression for the solubility-constant for hydroxyapatite and for fluoroapatite.1658views
Textbook QuestionThe solubility of AgCl(s) in water at 25 °C is 1.33 * 10 - 5 mol>L and its ΔH° of solution is 65.7 kJ>mol. What is its solubility at 50.0 °C?1901views
Textbook QuestionUse the following solubility data to calculate a value of Ksp for each compound. (d) Zn(CN)2; 4.95 x 10^-4 g/L487views1rank
Textbook QuestionUse the following solubility data to calculate a value of Ksp for each compound. (a) SrF2: 1.03 x 10^-3 M598views
Textbook QuestionUse the values of Ksp in Appendix C to calculate the molar solubility of the following compounds: (b) Mg(OH)2611views
Textbook QuestionUse the values of Ksp in Appendix C to calculate the solubility of the following compounds (in g/L): (c) Cu3(PO4)2726views
Textbook QuestionThe osmotic pressure of a saturated solution of strontium sulfate at 25 C is 21 torr. What is the solubility product of this salt at 25 C?805views
Textbook QuestionA concentration of 10–100 parts per billion (by mass) of Ag+ is an effective disinfectant in swimming pools. However, if the concentration exceeds this range, the Ag+ can cause adverse health effects. One way to maintain an appropriate concentration of Ag+ is to add a slightly soluble salt to the pool. Using Ksp values from Appendix D, calculate the equilibrium concentration of Ag+ in parts per billion that would exist in equilibrium with (c) AgI.975views
Textbook QuestionPseudogout, a condition with symptoms similar to those of gout (see Problem 126), is caused by the formation of calcium diphosphate (Ca2P2O7) crystals within tendons, cartilage, and ligaments. Calcium diphosphate will precipitate out of blood plasma when diphosphate levels become abnormally high. If the calcium concentration in blood plasma is 9.2 mg>dL, and Ksp for calcium diphosphate is 8.64 * 10 - 13, what minimum concentration of diphosphate results in precipitation?430views1comments
Textbook Question(b) If Ksp = 1.1 * 10-12 for Ag2CrO4, what are the molar concentrations of Ag+ and CrO4 2-in solution?516views
Textbook QuestionWrite the expression for the solubility product constant of MgF2 (see Problem 4.139). If [Mg2+] = 2.6 * 10-4 mol/L in a solution, what is the value of Ksp?485views
Textbook QuestionA 0.0100 mol sample of solid Cd(OH)2 (Ksp = 5.3 x 10^-15) in 100.0 mL of water is titrated with 0.100 M HNO3. (c) How many milliliters of 0.100 M HNO3 must be added to completely neutralize the Cd(OH)2?360views
Textbook QuestionA saturated solution of an ionic salt MX exhibits an osmotic pressure of 74.4 mm Hg at 25 °C. Assuming that MX is completely dissociated in solution, what is the value of its Ksp?481views
Textbook QuestionSome progressive hair coloring products marketed to men, such as Grecian Formula 16, contain lead acetate Pb(CH3CO2)2. As the coloring solution is rubbed on the hhair, the Pb2+ ions react with the sulfur atoms in hair proteins to give lead(II) sulfide (PbS), which is black. A typical coloring solution contains 0.3 mass% Pb(CH3CO2)2, and about 2 mL of the solution is used per application. (b) Suppose the hair is washed with shampoo and water that has pH = 5.50. How many washings would be required to remove 50% of the black color? Assume that 3 gal of water is used per washing and that the water becomes saturated with PbS. (c) Does the calculated number of washings look reason-able, given that frequent application of the coloring solution is recommended? What process(es) in addition to dissolution might contribute to the loss of color?267views
Open QuestionCalcium oxalate, CaC2O4 (m = 128.1), dissolves to the extent of 0.67 mg L–1 . What is its Ksp?80views
Open QuestionThe solubility of Ag3PO4 in water at 25 °C is 4.3 × 10-5 M. What is Ksp for Ag3PO4?131views
Open QuestionThe Ksp of PbBr2 is 6.60×10−6. What is the molar solubility of PbBr2 in pure water?72views