1) Hydroxylapatite, Ca10(PO4)6(OH)2, has a solubility constant of Ksp = 2.34 × 10-59, and dissociates according...

1) Hydroxylapatite, Ca10(PO4)6(OH)2, has a solubility constant of Ksp = 2.34 × 10-59, and dissociates according to Ca10(PO4)6OH2 <======> 10Ca(2+) + 6PO4(3-) + 2OH-

Solid hydroxylapatite is dissolved in water to form a saturated solution. What is the concentration of Ca2 in this solution if [OH–] is somehow fixed at 1.20 × 10-6 M?

2) Determine the concentration of an HBr solution if a 40.00 mL aliquot of the solution yields 0.6828 g AgBr when added to a solution with an excess of Ag ions. The Ksp of AgBr is 5.0 × 10–13.

Expert Solution

queen_honey_blossom answered 2 years ago

Hydroxylapatite, Ca10(PO4)6(OH)2, has a solubility constant of Ksp 2.34 x106, and dissociates acc...

Hydroxylapatite, $\mathrm{Ca}_{10}\left(\mathrm{PO}_{4}\right)_{6}(\mathrm{OH})_{2}$, has a solubility constant of $K_{\mathrm{sp}}=2.34 \times 10^{\mathrm{F}}$, and dissociates according to$$ \mathrm{Ca}_{10}\left(\mathrm{PO}_{4}\right)_{6}(\mathrm{OH})_{2}(s) \rightleftharpoons 10 \mathrm{Ca}^{2+}(a q)+6 \mathrm{PO}_{4}^{3-}(a q)+20 \mathrm{H}^{-}(a q) $$Solid hydroxylapatite is dissolved in water to form a saturated solution. What is the concentration of $\mathrm{Ca}^{2+}$ in this solution if $\left[\mathrm{OH}^{-}\right]$ is somehow fixed at $6.50 \times 10^{-6} \mathrm{M}$ ?Let $\left[\mathrm{Ca}^{2+}\right]=x .$ For every $10 \mathrm{~mol}$ of $\mathrm{Ca}^{2+}$ produced there are $6 \mathrm{~mol}$ of $\mathrm{PO}_{4}{ }^{3-}$, so $\left[\mathrm{PO}_{4}{ }^{3-}\right]=(6 / 10) x=(3 / 5) x$. The...

Hydroxylapatite, Ca10(PO4)6(OH)2, found in teeth and bones within the human body, has a solubility constant of...

Hydroxylapatite, Ca10(PO4)6(OH)2, found in teeth and bones within the human body, has a solubility constant of Ksp = 2.34 × 10–59, and dissociates according to Ca10(PO4)6(OH)2 (s) ⇄10Ca2+ (aq) + 6 PO4 3– (aq) + 2 OH– (aq) Solid hydroxylapatite is dissolved in water to form a saturated solution. (a) What is the pH of this saturated solution? (b) What is the solubility of Hydroxylapatitein this solutionif [OH– ] is fixed at 5.0 × 10–8 M (optimal pH of saliva)?...

Mg(OH)2 is a sparingly soluble salt with a solubility product constant, Ksp, of 5.61×10−11. It is...

Mg(OH)2 is a sparingly soluble salt with a solubility product constant, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. Calculate the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.150 mol L−1 NaOH solution.

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Use the solubility-product constant for Cr (OH) 3 ( Ksp = 6.7×10?31) and the formation constant for Cr (OH) ?4 from the following table to determine the concentration of Cr (OH) ?4 in a solution that is buffered at pH= 11 and is in equilibrium with solid Cr (OH) 3. Table Formation Constants for Some Metal Complex Ions in Water at 25 ?C Complex Ion Kf Equilibrium Equation Ag(NH3)+2 1.7×107 Ag+(aq)+2NH3(aq)?Ag(NH3)+2(aq) Ag(CN)?2 1×1021 Ag+(aq)+2CN?(aq)?Ag(CN)?2(aq) Ag(S2O3)3?2 2.9×1013 Ag+(aq)+2S2O2?3(aq)?Ag(S2O3)3?2(aq) CdBr2?4 5×103 Cd2+(aq)+4Br?(aq)?CdBr2?4(aq)...

The molar solubility of Mg3(PO4)2 is 6.26×10-6 mol/L at 25°C. 1. Calculate the solubility of Mg3(PO4)2...

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1)The Ksp of nickel(II) hydroxide, Ni(OH)2, is 5.84 × 10-16. Calculate the solubility of this compound...

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Mg(OH)2 is a sparingly soluble salt with a solubility product, Ksp, of 5.61×10−11. It is used...

Mg(OH)2 is a sparingly soluble salt with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. What is the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2dissolved in a 0.160 M NaOH solution? Express your answer numerically as the ratio of molar solubility in H2O to the molar solubility in NaOH.

1 - For the insoluble salt lead (ii) phosphate Pb3(PO4)2, the solubility product, Ksp is 3.10x10-44...

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