When sodium sulfide reacts with cobalt (II) acetate in water, cobalt (II) sulfide and sodium acetate are produced. (a) Write the balanced (i) molecular; (ii) total ionic; and (iii) net ionic equations. Include phases. (b) If 4.00 mL of 0.250 mol/L sodium sulfide solution are reacted with 6.80 mL of 0.350 mol/L cobalt (II) acetate solution, what mass of precipitate is formed? Show all your work, including a complete dimensional analysis. (c) Assume the reaction proceeds to completion with 100% yield and that the excess reactant could not be recycled. What is the mass of wasted starting material?

When sodium sulfide reacts with cobalt (II) acetate in water, cobalt (II) sulfide and sodium acetate are produced. (a) Write the balanced (i) molecular; (ii) total ionic; and (iii) net ionic equations. Include phases. (b) If 4.00 mL of 0.250 mol/L sodium sulfide solution are reacted with 6.80 mL of 0.350 mol/L cobalt (II) acetate solution, what mass of precipitate is formed? Show all your work, including a complete dimensional analysis. (c) Assume the reaction proceeds to completion with 100% yield and that the excess reactant could not be recycled. What is the mass of wasted starting material?

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

A supplement was tested for iron content in a laboratory. First, a random sample of 10 tabletsweighing a total of 13.7421 g was turned into fine powder. A scoop of this powder weighing2.7544 g was then dissolved and precipitated as Fe(OH)3 which was then rinsed and ignited to aconstant weight as Fe2O3 (159.69 g/mol). The recorded constant weight of Fe2O3 is 0.2629 g.a. What is the %Fe (55.85 g/mol) content of the supplement?b. What is the iron content of the supplement reported as g FeSO4∙7H2O (277.908 g/mol)per tablet?
If 25.0 mL of 0.120 M Na3PO4 and 30.0 mL of 0.110 M CaCl2 are mixed, what precipitate forms? Write out the net ionic equation. How many grams of the precipitate forms?
A sample of solid Ca(OH), was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH), as it could hold. A 75.5-mL sample of this solution was withdrawn and titrated with 0.0683 M HBr. It required 53.6 mL of the acid solution for neutralization. (a) What was the molarity of the Ca(OH), solution? (b) What is the solubility of Ca(OH), in water, at the experimental temperature, in grams of Ca(OH), per 100 mL of solution? 9/100mL MY NOTES ASK YOUR TEACHER
A metal, Manganese (Mn) was discovered from a mining site. Mn presentin the ore sample was analysed by forming a precipitate of MnSO4. If4.21 g of ore sample gives 0.22 g of MnSO4. Calculate the percentageof Mn present in the sample.
A sample of solid Eu(OH)3 was stirred in water at a certain temperature until the solution contained as much dissolved Eu(OH)3 as it could hold. A 650-mL sample of this solution was withdrawn and titrated with 1.33e-05 M HBr. It required 21 mL of the acid solution for neutralization.What is the solubility of Eu(OH)3 in water, at the experimental temperature, in grams of Eu(OH)3 per liter of solution? a) The solubility is 7.06e-10 g/L. b) The solubility is 8.72e-05 g/L. c) The solubility is 0.000262 g/L. d) The solubility is 2.91e-05 g/L. e) The solubility is 6.08e-06 g/L.
Complete the followin reaction by providing the products formed. Then balance the reaction and write the molecular reaction and the total and net ionic reactions. The reaction is: Zn(NO3)2 (aq) + Ba(OH)2 (aq) ---> Products.
(b) (i) How many grams of NaOH are present in 53.0 mL of a 5.50 M solution?(ii) Calculate the volume in mL of a 1.420 M NaOH solution required to titrate 50.00 mL of a4.50 M H 2 SO 4 solution
(a) Write the balance equation for the reaction of sulfuric acid and barium hydroxide. (b).What is the concentration of the sulfuric acid solution, if 100 ml of the solution is neutralized by 50 ml of 0.5 M Ba(OH)2 solution?
X bMy Questions | bartleby 101 Chem 101 X X app.101edu.co Submit Question 38 of 43 Write the balanced COMPLETE ionic equation for the reaction when Na2CO3 and AgNOs are mixed in aqueous solution. If no reaction occurs, write only NR. 4- |2- |2+ 3+ 4+ + 83 1 2 3 4 5 6 7 0 4 3 17 1 5 (g) (aq) (s) (1) NR Ag С N Na Reset Delete x H20 8:47 AM е OTYPE here to search 11/8/2019 S LO
Aluminum sulfate, known as cake alum, has a wide range ofuses, from dyeing leather and cloth to purifying sewage. Inaqueous solution, it reacts with base to form a white precipitate.(a) Write balanced total and net ionic equations for its reactionwith aqueous NaOH. (b) What mass of precipitate forms when185.5 mL of 0.533 M NaOH is added to 627 mL of a solutionthat contains 15.8 g of aluminum sulfate per liter?
A sample of solid Mg(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Mg(OH)2 as it could hold. A 450-mL sample of this solution was withdrawn and titrated with 0.00357 M HClO4. It required 58.3 mL of the acid solution for neutralization.What is the solubility of Mg(OH)2 in water, at the experimental temperature, in grams of Mg(OH)2 per liter of solution?
a) 400.0 mL of 0.20 M mercury (II) nitrate solution and 400.0 mL of 0.35 M potassium iodide solution react in a double displacement reaction, how many grams of precipitate are expected? b) Calculate the volume of 0.855 M sulphuric acid, H₂SO4, required to completely neutralize a sample of 48.5 mL of 0.600 M sodium hydroxide, NaOH.