Calculate the solubility of **silver phosphate**, Ag₃PO₄, in units of grams per liter.\( K_{sp} (\text{Ag}_3\text{PO}_4) = 1.3 \times 10^{-20} \).\[\text{solubility} = \_\_\_\_\_\_\_\_\_\_ \, \text{g/L}\]

Answered: Image /qna-images/answer/b50437e7-729e-4213-a874-4a6b0027dcba.jpg

Answered: Calculate the solubility of silver…

Calculate the solubility of silver phosphate, Ag3PO4 in units of grams per liter. Ksp (Ag3PO4) = 1.3x10-20 solubility = g/L

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

If you wish to precipitate Ag* from a 3.5 x 10-4 M solution, which of the following solutions could you use? Show the calculations that allowed you to determine the answer. There may be more than one correct choice. 5.0 x 10-5 M NaCI (Ksp for AgCl = 1.8 x 10-10) 5.0 x 10-5 M Na3PO4 (Ksp for Ag3PO4 = 8.9 x 1017) 5.0 x 10-5 M NaBr (Ksp for AgBr = 5.0 x 10-13) 5.0 x 10-5 M Na2CO3 (Ksp for Ag2CO3 = 8.1 x 10-12)
if u add 400.0 mL of water to 50.0 mL of 6.0 M HCl what is new concentration ?
A technician would like to standardize an unknown Ca(OH)2 solution. It takes 18.26 mL of a 0.191 M solution of HCl to titrate 25.00 mL the unknown Ca(OH)2 solution. Calculate the molarity of the Ca(OH)2 solution. Tip: Don't forget to consider the mole ratio between HCl and Ca(OH)2. 2HCl(aq)+Ca(OH)2(aq)⟶CaCl2(aq)+2H2O(l)
If 500.0mL of a 0.150mol/L solution of the aluminum nitrate (AI(NO3) (aq)) is mixed with 400.0mL of a 0.200 mol solution of calcium hydroxide (Ca(OH)2 (aq)), precipitate results (Use a solubility table to determine which product of this double displacement is the precipitate) Calculate the percent yield of the experiment if 3.00g of the solid precipitate is filtered out.
Can you help me filling all the table with this data please I really appreciate it! Titration of Acetic Acid and Vinegar - Topic
A technician would like to standardize an unknown Ca(OH)2 solution. It takes 18.53 mL of a 0.174 M solution of HCI to titrate 25.00 mL the unknown Ca(OH)2 solution. Calculate the molarity of the Ca(OH)2 solution. Tip: Don't forget to consider the mole ratio between HCl and Ca(OH)2. 2 HCI (aq) + Ca(OH), (aq) CaCl2 (aq) + 2 H2O (1)
The molar solubility of Mg(OH)2 in water is 8.9×10–12 mol/L. What is thesolubility product (Ksp) of Mg(OH)2?
The solubility product constant for a certain metal fluoride, MF2 is Ksp = 1.2 × 10−6. Its molar mass is ℳ = 175.90 g/mol. What is its solubility in mol/L? Report your answer to TWO significant figures. Enter your answer in scientific notation using the appropriate boxes. Remember, a number like 1.6, in scientific notation is 1.6 × 100. Note: Your answer is assumed to be reduced to the highest power possible.
Sodium-ion (Na+) and Calcium ion (Ca2+) produce nearly the same color in a flame test (yellow and yellow-orange, respectively). Describe a way to differentiate between the two using a solution of Na2CO3 and write the correct balanced equations. (Hint: Recall the solubility rules of Na+ ion.)
A solution containing cobalt (I) ions is added to a solution that is 0.034 M Br– and 0.069 M Cl–. What is the identity of the precipitate that forms, and at what concentration of cobalt (I) ions does this begin to occur? Solubility Product Constants: CoCl = 2.1 × 10–5 CoBr = 6.2 × 10–12 No precipitate will form at any concentration of cobalt (I). CoCl, 9.0 × 10–11 M CoBr, 3.0 × 10–4 M CoCl, 6.2 × 10–4 M CoBr, 1.8 × 10–10 M
The solubility of an ionic compound in water can be expressed in terms of the mass that will dissolve in a given volume of water, or in terms of the solubility product, Ksp. If only 0.251 g of Ca(OH)2 dissolves in enough water to give 0.204 L of aqueous solution at a given temperature, what is the Ksp value for calcium hydroxide at this temperature?
CuO(s) + HCl(aq) → CuCl2 (aq) + H20(1) The mass of CuO was measured to be 2.500 g. The volume of HCl was measured to be 13.3 mL. The concentration of HCl was measured to be 1.50 M. b. Calculate the theoretical number of moles of CuCl2(ag) produced from HCI.