Hydroxyapatite, Ca₁0 (PO4) 6 (OH)2, has a solubility constant of Ksp = 2.34 x 10-59, and dissociates according to Ca10 (PO4)(OH)2(s) = 10 Ca²+(aq) + 6 PO¾-¯(aq) + 2 OH(aq) Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca²+ in this solution if [OH] is fixed at 3.60 × 10-4 M? [Ca2+] = M

The solubility of Pbl2 (Ksp = 9.8 x 109) varies with the composition of the solvent in which it was dissolved. In which solvent mixture would Pbl2 have the lowest solubility at identical temperatures? 0.8 M Mgl2(aq) 1.0 M Pb(NO3)2(aq) 1.5 M Kl(aq) 1.0 M HCl(aq) pure water D

Consider an amphoteric hydroxide, M(OH)₂ (s), where M is a generic metal. M(OH)₂ (s) = M²+ (aq) + 2OH(aq) Ksp = 4 X 10-16 M(OH)₂ (s) + 2OH(aq) [M(OH)₂1²2-(aq) K₁ = 0.03 Estimate the solubility of M(OH)₂ in a solution buffered at pH = 7.0, 10.0, and 14.0. solubility at pH = 7.0 solubility at pH = 10.0 solubility at pH = 14.0 M M M

To determine the solubility product constant of Al(OH)3 at a specific temperature, a saturated solution of Al(OH)3 at the required temperature was titrated with 0.2M HCl via the reaction: 3HCl + Al(OH)3  → AlCl3 + 3H2O.  Based on the following data, determine the Ksp of Al(OH)3 at the specified temperature:                Volume of Al(OH)3 titrated: Volume of 0.2M HCl required: 9.5 mL 3.44 mL Your answer should follow the format: a) mols of HCl added b) mols of Al(OH)3 c) Molarity of Al(OH)3 d) Ksp of Al(OH)3

Will the solubility of CaCO3 in water increase or decrease if the pressure of CO2 gas above the saturated solution is increased? Note that CO2 gas reacts with water to produce a weak diprotic acid H2CO3. This acid can undergo the loss of one or two protons to form HCO3- and CO32- ions (these are bicarbonate and carbonate).

Of the substances (as pure substances, in aqueous solutions, or of mixtures) tested on video, categorize them into either molecular or ionic substances. molecular ionic No Answers Chosen No Answers Chosen Possible answers | HCI (in toluene) : 0.1 M C12H22O11 (aq) - this is sucrose | CH3COOH (glacial acetic acid) | saturated Ca(OH)2 (aq) | 0.1 M NH4CI (aq) | KCIO3 (s) | C7H8 (toluene) 0.1 МСНЗСН2ОН (аq) | CH3CH2OH (pure) | KCIO3 (1) | 0.1 M NaCI (aq) 0.1 M KCIO3 (aq) | saturated Ca3(PO4)2 (aq) | 0.1 M NH3 (aq) | 0.1 M HCI (aq) H2O (distilled) : 0.1 МСНЗСООН (аq) : 0.1 MNaOН (аq)

Consider the table of equilibrium constant values given below for a given set of conditions. What will be the concentration of [HCO3-] in water that is in equilibrium with both CaCO3 (s) and 225 ppm CO2 (g) under these conditions? Equation Type Value CO2 (g) H2CO3 (aq) KH 1.7 x 102 H2CO3 (aq)=HCO3(aq) + H (aq) Kat 6.44 x 107 HCO3 (aq) CO32 (aq) + H* (aq) Ka2 8.43 x 10-11 CaCO3 (s) Ca2+ (aq) + CO2 (aq) Ksp 8.4 x 10-9 H₂O (1) H(aq) + OH (aq) Kw 7.6 x 10-14 O 1.6 x 103 M O 8.1 x 10-3 M O 5.6 x 104 M O 3.9 x 104 M O 7.9 x 104 M

o A chemist wants to extract a solute from 100 mL of water using only 300 mL of ether. The distribution constant, Kp, between ether and water is 1.99. Calculate q, the fraction of solute that would remain in the water under each of the extraction conditions. The chemist performs a single extraction with 300 mL of ether. 9 = The chemist performs three extractions with 100 mL of ether. 9= The chemist performs six extractions with 50 mL of ether. 9 =

Ksp(CaF2) = 3.9 x 10-11. Assume that we add enough amount of CaF2 into the following 3 solutions so that CaF2 will become saturated in each solution. Solution A. 0.30 M Ca(NO3)2 (aq). Ca(NO3)2 is highly soluble in water. Solution B. 0.30 M NaF (aq). NaF is highly soluble in water. Solution C. 0.30 M NaNO3 (aq). NaNO3 is highly soluble in water. Which of the following statements is true about the solubility of CaF2 in the above 3 solutions? Choose one option only. Options: a. CaF2 (s) has the lowest solubility in Solution B. b. CaF2 (s) has the highest solubility in Solution B. c. CaF2 (s) has the highest solubility in Solution A. d. CaF2 (s) has the lowest solubility in Solution C. e. CaF2 (s) has the lowest solubility in Solution A.

The Ksp for LaF3 is 2 x 10-⁹. What is the solubility of LaF3 in water in moles per liter?