Describe the preparation of a) 500 ml of 0.0550 M silver nitrate solution from solid silver nitrate b) 5.00 L of a solution that is 0.0800M in K* starting with solid K3FE(CN), c) 2.00 L of 0.135 M perchloric acid from the commercial reagent [60% perchloric acid (w/w), specific gravity 1.60] d) 9.50 L of a solution that is 60.0 ppm in Na*starting with solid Na2sO4.

Describe the preparation of a) 500 ml of 0.0550 M silver nitrate solution from solid silver nitrate b) 5.00 L of a solution that is 0.0800M in K* starting with solid K3FE(CN), c) 2.00 L of 0.135 M perchloric acid from the commercial reagent [60% perchloric acid (w/w), specific gravity 1.60] d) 9.50 L of a solution that is 60.0 ppm in Na*starting with solid Na2sO4.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 29QRT

See similar textbooks

Similar questions

A solution is made by dissolving 0.455 g of PbBr2 in 100 g of H2O at 50C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
The freezing point of 0.10 M KHSO3 is -0.38C. Which of the following equations best represents what happens when KHSO3 dissolves in water? (a) KHSO3(s)KHSO3(aq) (b) KHSO3(s) K+(aq)+HSO3(aq) (c) KHSO3(s) K+(aq)+SO32(aq)+ H+(aq)
Dimethylglyoxime [DMG, (CH3CNOH)2] is used as a reagent to precipitate nickel ion. Assume that 53.0 g of DMC has been dissolved in 525 g of ethanol (C2H5OH). s The red, insoluble compound formed between nickel(II)ion and dimethylglyoxime (DMG) is precipitated when DMG is added to a bask solution of Ni2+ (aq). (a) What is the mole fraction of DMG? (b) What is the molality of the solution? (c) What is the vapor pressure of the ethanol over the solution at ethanols normal boiling point of 78.4 C? (d) What is the boiling point of the solution? (DMG does not produce ions in solution.) (Kbp for ethanol = +1.22 C/m)
10. A solution was prepared by dissolving 5.76 g of KCI MgCl2.6H20 (277.85 g/mol) in sufficient water to give 2.000 L. Calculate (d) the weight/volume percentage of KCI. MgCl2. 6H2O. (e) the number of millimoles of Cl2 in 25.0 ml of this solution. (f) ppm K+.
O 1.40 L of a solution that is 10.0 ppm in K*, starting with solid K4 Fe (CN) . Dissolve mg K4 Fe (CN)6 in enough water to give a final volume of L.
A natural product, P, has a Kp between water (aq) and ethyl acetate (ea) of 13.4. A 50.00-mL sample of a 0.022 M aqueous solution of the solute is extracted with 10.00 mL of ethyl acetate. What is fraction of P extracted to ethyl acetate after two extractions? O A. 98.5 O B. 92.6% O C. 99.8% O D. 1.5% O E. 7.4%
Describe the preparation of a) 500 ml of 0.0550 M silver nitrate solution from solid silver nitrate b) 5.00 L of a solution that is 0.0800M in K* starting with solid K3FE(CN), c) 2.00 L of 0.135 M perchloric acid from the commercial reagent [60% perchloric acid (w/w), specific gravity 1.60] d) 9.50 L of a solution that is 60.0 ppm in Na*starting with solid Na,SO4.
A solution is prepared by dissolving 11.60 g of a mixture of sodium carbonate and sodium bicarbonate in 1.00 L of water. A 300.0 cm3 sample of the solution is treated with excess HNO3 and boiled to remove all the dissolved gas. A total of 0.940 L of dry CO2 is collected at 298 K and 0.972 atm. Find the molarity of the carbonate and bicarbonate in the solution.
ered nswers A chemist has a 50.0 mL sample of 0.010 M Na₂C₂O4 at 25 °C (solution A, oxalate ion = C₂04² ). An aqueous solution of Ca(NO3)2 with a volume of 50.0 mL (solution B) is added to solution A, at the same temperature. Above what minimum concentration must Ca(NO3)2 in solution B be, prior to mixing, to cause CaC₂O4 to precipitate given that for CaC₂O4, Ksp = 2.7 x 10-⁹ at 25 °C? Enter your answer with two significant figures, without units, and in millimolarity (mM) where: millimolarity = (molarity)(1000) 0.001 (with margin: 0) 0.0011 (with margin: 0)
Five drops of dichlorofluorescein have been added to a solution containing 0.800 g sample which required 25.30 mL of 0.100 M AgNO3. (c) Calculate the weight percent NaCl in the original sample.
What is the solubility of TIBr(s) ? Ksp = 3.4 x 106 %3D
148. Addition of 50.00 mL of 2.238 m H2SO4 (solution density = 1.1243 g/mL) to 50.00 mL of 2.238 M BaCl2 gives a white precipitate. (a) What is the mass of the precipitate in grams? (b) If you filter the mixture and add more H2SO4 solution to the filtrate, would you obtain more precipitate? Explain.