46. Given this solution at equilibrium: CaF2(s) = Ca2+(aq) + 2F-(aq)What is the solubility products (Ksp) expression? * a. Ksp = [Ca²+][F-] b. Ksp = [Ca2+][2F-] %3D c. Kp = [Ca²+][F-]? [Ca²+][F=]? d. Ksp = [Ca2+]2[F ]? %3D a. b.

What happens when equal volumes of 2x104 M aqueous solutions of calcium nitrate, Ca(NO3)2, and sodium fluoride, NaF, are combined? The K of calcium fluoride, CaF 2, is 4.0x10-11, sp O a. Q K; no precipitate forms c. Q K; a precipitate forms

calculate their solubility product constants.

The expression for the solubility product of Ca3(PO4)2 is: 2+1 3 2 [Ca²+]³ x [PO³ ]² 3- 4 2+ 3- 03 [Ca²+] × 2 [PO³-] 4 2+ 3 3 [Ca ²+1³ + 2[PO³ ]² 2 3- 4 3- 2 [3 × Ca²+]³ × [2 × PO³-]² 4

A solution contains 0.0010 mol of KI and 0.10 mol of KCl per liter. AgNO3 is gradually added to this solution. Which forms first, solid AgI or solid AgCl?

1. How do you prepare a 100mL of 0.1 M phosphate buffer?To make 100 mL of 0.1 M phosphate buffer: Calculate the amount of sodium phosphate needed. moles of sodium phosphate = (0.1 mol/L) x (0.1 L) = 0.01 moles mass of sodium phosphate = moles x molar mass = 0.01 moles x 142 g/mol = 1.42 g Dissolve 1.42 g of sodium phosphate in distilled water in a 100 mL volumetric flask. Adjust the pH of the solution to the desired value (usually around 7.4) using a strong acid or strong base. Bring the solution to the final volume (100 mL) with distilled water.   2. From the anterior buffer, how do you make 100mL of 0.05 M? To make 100 mL of 0.05 M phosphate buffer from the 0.1 M stock solution: Calculate the amount of the 0.1 M phosphate buffer needed. moles of phosphate buffer = (0.05 mol/L) x (0.1 L) = 0.005 moles Calculate the volume of the 0.1 M phosphate buffer needed. moles = concentration x volume (in liters) volume = moles / concentration = 0.005 moles / 0.1 mol/L = 0.05 L or 50 mL Measure…

Write a solubility product constant, Ksp, equilibrium expression for the following ionic solid. Assume A is a metal ion and B is an anion. For example, for CaCO3(s): Ksp = [Ca2+][CO32-] A4B1(s): Ksp = [A+]x[B-]y What is the value of x?

5) Calculate the solubility of each of the following salts in moles per liter given their Ksp values. Ignore any acid-base properties.a. Ag3PO4, Ksp=1.8x10−18b. CaCO3, Ksp=8.7x10−9C) Calculate the solubility of the silver phosphate and the calcium carbonate in question 5 in grams/L.

Suppose 60.0 mL of 0.100 M Pb(NO3)2 is added to 30.0 mL of 0.150 M KI. How many grams of Pbl2 will be formed? Mass Pbl₂ = 1.037 Hint [K+] Your answer is correct. [1] What will be the molar concentrations of all the ions in the mixture after equilibrium has been reached? Record all answers to three (3) significant figures. Your answer is partially correct. [Pb²+] 0.05 i 0.05 g [NO3] 0.13 0.067 M M 3 3 M

22.