Calcium phosphate crystallises in a number of different modifications of which β-$\ce{Ca3(PO4)2}$ is the stable room temperature and ambient pressure modification. It has a rather complex structure not easily described, consisting of chains and rings with phosphate and calcium ions in specific patterns.

Answer to 5) What is the equilibrium constant expression for. Science; Chemistry; Chemistry questions and answers; 5) What is the equilibrium constant expression for the Ksp of Ca3(PO4)2?

Write charge and mass balance equations for aqueous Ca3(PO4)2 if species are Ca2+, CaOH+, CaPO4-, PO43-, HPO42-, H2PO4- and H3PO4. Your solution’s ready to go! Our expert help has broken down your problem into an easy-to-learn solution you can count on.

Question: Write the Ksp expression for the sparingly soluble compound calcium phosphate, Ca3(PO4)2- Ksp If either the numerator or denominator is 1, please enter 1. Submit Answer Retry Entire Group 1 more group attempt remaining

Question: Part B What is the molar mass of calcium phosphate, Ca3(PO4)2? Express your answer to five significant figures and include the appropriate units. View Available Hint(s) μΑ Value Units Submit

Question: What is the correct heat of formation reaction equation for Ca3(PO4)2 (s)? (Hint: The standard state of phosphorous exists as P4(s).

Determine the molecular formula of a compound that has a molar mass of 183.2 g/mol and an empirical formula of C2H502. A) C2H5O2 B) C6H1506 C) C3H703 D) C4H1004 E) C3H12008 24. Determine the empirical formula for a compound that is 36.86% N and 63.14%O by mass.

Answer to A saturated solution of Ca3(PO4)2 has [Ca2+] = 1.90. Your solution’s ready to go! Our expert help has broken down your problem into an easy-to-learn solution you can count on.

It is found that 1.66e-06 g of Ca3(PO4)2 dissolves per 100 mL of aqueous solution at 25 ^oC. Calculate the solubility-product constant for Ca3(PO4)2. The solubility of magnesium phosphate is 8.64 x 10-6 mol/1.0 L of solution. What is the Ksp for Mg3(PO4)2? Determine the molar solubility of a compound with K_{sp} = 4.32 \times 10^{-6} in pure water.

Given that the solubility reaction for calcium phosphate is Ca3(PO4)2(s) = 3Ca2+ (aq) + 2PO43- (aq) why does the addition of acid increase the solubility of calcium phosphate? View Available Hint(s) O It decreases the phosphate ion concentration, forcing the equilibrium to the right It decreases the phosphate ion concentration, forcing the ...