7. Tooth enamel (Cas(PO4)3OH) is a slightly soluble compound that exists as the equilibrium shown below. If the Ksp of tooth enamel in water is 6.8 x 10-37 calculate the molar solubility of tooth enamel. Cas(PO4)3OH (s) → 5Ca²+ (aq) + 3PO4³ (aq) + OH- (aq) a. 2.7 x 105 M b. 5.84 x 108 M C. 8.2 x 10-19 M d. 6.4 x 10⁹ M 2.00

7. Tooth enamel (Cas(PO4)3OH) is a slightly soluble compound that exists as the equilibrium shown below. If the Ksp of tooth enamel in water is 6.8 x 10-37 calculate the molar solubility of tooth enamel. Cas(PO4)3OH (s) → 5Ca²+ (aq) + 3PO4³ (aq) + OH- (aq) a. 2.7 x 105 M b. 5.84 x 108 M C. 8.2 x 10-19 M d. 6.4 x 10⁹ M 2.00

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

20.
Good hand written solution
Complete the following solubility constant expression for PbCrO 4. K sp = 0 X Ś
A student combines Fe(NO3)3 solution and KSCN solution to produce a solution in which the initial concentrations of Fe3+(aq) and SCN–(aq) are both 5.58 × 10–2 M. The chemical equilibrium forms FeSCN2+(aq): Fe3+ + SCN- <=> FeSCN2+ The absorbance of this solution (from FeSCN2+) is measured as 0.161, and Beer's law equation (the trend line from best fitting) as Absorbance = 189 x Concentration of FeSCN2+ + 0.02 Determine the equilibrium concentration for SCN- in mol/L.
What is the equilibrium concentration of OH‒ ions when 25 grams of Al(OH)3 is added to 2.50 L of water? Molar Mass of Al(OH)3 = 78.00 g/mol and Ksp(Al(OH)3) = 1.3 × 10‒33
Nitesh
Barium hydroxide, Ba(OH)2, dissolves in water to the extent of 18.5 g per liter. What is the value of Ksp for Ba(OH)2 ? Ba(OH)2(s) ⇒ Ba²+ (aq) + 2 OH¯(aq) K sp =
A student prepares a solution for titration by adding a 10.00 mL aliquot of a solution saturated with Ca(OH)2 at 82.9°C to 25.0 mL of deionized water. This solution is titrated with a standardized 0.01252 M HCl solution. The equivalence point is observed after 17.94 mL of the HCl solution has been added. Calculate the moles and molarity of OH- and Ca2+ in the 10.00ml sample.
A student titrates 10.0 mL of 2.0 M formic acid, HCO,H (K.= 1.8 x 10-4), using 1.0 M sodium hydroxide, NaOH. 1. What volume of NaOH solution would be needed to reach the equivalence point? a. 10.0 mL b. 20.0 mL c. 30.0 mL d. 40.0 mL
HA, a weak acid, also forms the ion HA, in solution. The reaction is HA(aq) + A (aq) = HA, (aq) The weak acid has K, = 8.64 × 10-7 and the reaction has K = 3.80. Calculate the concentrations of A, H*, and HA, in a 1.00 M solution of HA. [A¯] = M [H*] = M [HA,] = M
A student carries out the following titration by adding H2SO4.
At 25 °C, only 0.0500 mol of the generic salt AB3 is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C? AB₂ (s) ⇒ A³+ (aq) + 3 B¯(aq) Ksp =