The Ksp of La(OH) 3 is 2.0x10-21 When activities are considered, what is the concentrationof La³+ in a saturated solution with an ionic strength of 0.082 M?La(OH)3 (s) = La² + 3OH+3ОН(aq)(aq)Ksp = 2.0x10--21For La 3+ with a charge of +3 and a hydrated radius of 900 pm, the activity coefficientfrom the extended Debye Hückle equation is 0.194 when the ionic strength is 0.082 M.For OH with a charge of -1 and a hydrated radius of 350 pm, the activity coefficient fromthe extended Debye Hückle equation is 0.776 when the ionic strength is 0.082 M.Answer using scientific notation with 3 significant digits. For example typing "3.14E-6 M"

Step 1: For the concentration of [La3+] in a saturated solution, we will use the equation for Ksp to…

Answered: The Ksp of La(OH) 3 is 2.0x10-21 When…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter10: Effect Of Electrolytes On Chemical Equilibria

Section: Chapter Questions

Problem 10.8QAP

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Consider the solutions presented: (a) Which of the following sketches best represents the ions in a solution of Fe(NO3)3(aq)? (b) Write a balanced chemical equation showing the p10ducts of the dissolution of Fe(NO3)3.
A solution saturated with a salt of the type M3X2 has an osmotic pressure of 2.64 102 atm at 25C. Calculate the Ksp value for the salt, assuming ideal behavior.
Write the expression for the equilibrium constant and calculate the partial pressure of CO2(g), given that Kp is 0.25 (at 427 C) for NaHCO3(s) NaOH(s) + CO2(g)
The thermodynamic solubility product of A9CN is 6.0×10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.75e-9 mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.81e-16 X mol·L-1
Calculate the equilibrium concentration of Ag* (aq) in a solution that is initially 0.170 M AgNO3 and 0.870 MNH3, and in which the following reaction takes place: Agt (aq) + 2NH3(aq) Ag(NH3)2(aq) (Kf = 1.70x107) 3.46 x 10-7 = M Ag
The thermodynamic solubility product of AGCN is 6.0x10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.7e-9 X mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.8e-15 X mol·L-1
Tooth enamel is composed of the mineral hydroxyapatite, Ca5(PO4)3(OH), which ionizes water as follows: Ca5(PO4)3(OH)(s) ⇌ 5Ca2+(aq) + 3PO43–(aq) + OH–(aq) (a) Write the expression for Ksp of this compound. (b) If the solubility of hydroxyapatite in water is S mol/L, what is Ksp in term of S? (c) If Ksp= 6.8 x 10–37, calculate the solubility of Ca5(PO4)3(OH) in water in mol/L. (d) How is the solubility of hydroxyapatite affected by adding acid? Is the solubility in acidic solution higher or lower compared with that in water? (e) When hydroxyapatite is treated with fluoride, the mineral fluoroapatite, Ca5(PO4)3F, is formed. This mineral has Ksp~ 1 x 10–60. Write equation for the ionization of fluoroapatite in water, the expression for Ksp,and calculate its solubility in water. (f) Compare the solubility of fluoroapatite, Ca5(PO4)3F, with that of hydroxyapatite, Ca5(PO4)3(OH), and explain the rationale for the fluoridation of drinking water.
Calculate the solubility in grams per liter of Pb(IO3)2 (s) in 0.10 M KIO3 (aq) at 25 °C. The Ksp for Pb(103)2 (s) is 3.7 × 10-13 at this temperature. Answer:
The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20 so if a chemist added 1.19 x 10-2 M of Pb3(AsO4)2(aq) which is a common ion then what would be the concentration of the Magnesium ion Mg2+(aq) in Molarity at equilibrium? 3.89 x 10-6 4.07 x 10-6 3.47 x 10-6 2.45 x 10-6 2.81 x 10-6 3.28 x 10-6 2.64 x 10-6 3.69 x 10-6 3.01 x 10-6 4.29 x 10-6
(a) If the molar solubility of Nd₂(CO3)3 at 25 °C is 1.00e-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 °C. Calculate the solubility- product constant for Y₂(CO3)3. Ksp = (c) The Ksp of Ag₂C₂04 at 25 °C is 5.40e-12. What is the molar solubility of Ag2C₂04? solubility mol/L
Given the equilibria below, determine the mass of AgBr that will dissolve in 200 mL of 0.100 M NaCN. AgBr(s) Ag*(aq) +Br (aq) Ksp = 5.0 x 10-13 Ag"(aq) + 2 CN (aq) Ag(CN)2 (aq) Kr= 1.3 x 1021

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