How many moles of solute in 2.00 L of a 3.00 M solution ? The solute could be anything, and the solvent is usually water. The concentration will always be the conversion factor. M stands for mol/L. mol L)(- a. 0 b. 1 d. 3 j. 100. k. 1.71 I. 0.856 c. 2 e. 4 m. 10.0 f. 5 -) = L g. 6 h. 234 mol i. 58.44

How many moles of solute in 2.00 L of a 3.00 M solution ? The solute could be anything, and the solvent is usually water. The concentration will always be the conversion factor. M stands for mol/L. mol L)(- a. 0 b. 1 d. 3 j. 100. k. 1.71 I. 0.856 c. 2 e. 4 m. 10.0 f. 5 -) = L g. 6 h. 234 mol i. 58.44

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter7: Solutions And Colloids

Section: Chapter Questions

Problem 7.86E

See similar textbooks

Similar questions

6-21 Are mixtures of gases true solutions or heterogeneous mixtures? Explain.
What mass of a 4.00% NaOH solution by mass contains 15.0 g of NaOH?
The solubility of lead nitrate at 100C is 140.0 g/100 g water. A solution at 100C consists of 57.0 g of lead nitrate in 64.0 g of water. When the solution is cooled 10C to 25.0 g of lead nitrate crystallize out. What is the solubility of lead nitrate in g/100 g water at 10C?
The dispersed phase of a certain colloidal dispersion consists of spheres of diameter 1.0 102 nm. (a) What are the volume (V=43r2) and surface area (A = r2) of each sphere? (b) How many spheres are required to give a total volume of 1.0 cm3? What is the total surface area of these spheres in square meters?
A certain liquid X has a normal freezing point of 7.10°C and a freezing point depression constant =Kf3.27·°C·kgmol−1. A solution is prepared by dissolving some ammonium chloride (NH4Cl) in 700.g of X. This solution freezes at 6.4°C. Calculate the mass of NH4Cl that was dissolved. Round your answer to 1 significant digit. __g
You have a container of 17.42 M conc. acetic acid (CH3COOH(aq)) with density 1.05 g/mL, find the molality of a 150ml sample of the solution. molality = moles solute/Kg solvent moles solute = (0.150 L)(17.42 mol/L) = 2.613 mol CH3COOH molar mass of CH3COOH = 60.06 g/mol grams of solution = (150mL)(1.05 g/mL) = 157.5 g solution grams of solute = (2.613 mol)(60.06 g/mol) = 156.9 g CH3COOH so the total grams of water in this solution would be: g H2O = g solution - g CH3COOH = 157.5g - 156.9 g = 0.6g H2O 0.6g H2O = 0.0006 Kg H2O so molality = (2.613 mol CH3COOH) /(0.0006 kg H2O) = 4355 molal this seems rather high to me but if its 'concentrated' acetic acid, I know that you can get it to about 98% as glacial acetic acid so perhaps there is 4355 moles of acetic acid per kg of water. Did I do this correctly? I know that typically the solvent is the larger component of a solution but the fact that it gives me CH3COOH(aq) would imply that H2O is the solvent still in this situation, I have…
What is the mass of propanol present in a 3.50 molal aqueous solution of propanol, C3H7OH? The molar mass of propanol is 60.094 g/mol. Mass Solute = [?] g C3H₂OH Mass Solute (g) Copyright © 2003-2022 International Academy of Science. All Rights Reserved. DELL Enter Just Short Answer q Jefferson, Thomas
A certain liquid X has a normal freezing point of 0.90°C and a freezing point depression constant Kf=6.96·°C·kgmol−1.A solution is prepared by dissolving some barium hydroxide (Ba(OH)2) in 900.g of X. This solution freezes at−3.7°C. Calculate the mass of Ba(OH)2 that was dissolved. Round your answer to 2 significant digits.
- 1 A certain liquid X has a normal freezing point of –1.00 °C and a freezing point depression constant K,=2.88 °C·kg•mol *. A solution is prepared by dissolving some zinc chloride (ZnCl,) in 350. g of X. This solution freezes at -2.1 °C. Calculate the mass of ZNC1, that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. alo 18.2 g Ar х10
✓- a Gasoline vaporizes in the carburetor of an automobile engine 2Hg (1) + O₂ (g) --> - 2HgO (s) seperating solute particles throughout a solvent SO₂(g) + CaO(s) -----> CaSO3(s) freezing water to form ice BaF2 (s)--> Ba2+ (aq) + 2F (aq) PCL3(g) + Cl₂(g) ----> PCL5 (g) melting ice to form water Raindrops form in a cloud | C₂H4(g) + H₂(g) ---> - C₂H6 (g) Ni(s) + 2 HCl(aq) -----> H₂(g) + NiCl₂(aq) Sugar dissolves in coffee CO₂(g) + H₂O(1) ----> H₂CO3(aq) 2NO₂ (g) - dissolution of solid KCl in water mixing of two gases into one container boiling water to form steam Frost forms on the windshield of your car --> N₂O4 (g) CaO(s) + 2 HCl(g) ---> CaCl₂(s) + H₂O(l) Moisture condenses on the outside of a cold glass ir is pumped into a tire Sub question a. As0
1. ASSERTION: The solubility of gases in water follows the order O2 < N2 < SO2 < CO2 < NH3. REASON: For appreciable solubility, the solute-solvent interactions should outweigh the solute-solute and solvent-solvent interactions. a. Assertion and reason both are correct statements and reason is the correct explanation for assertion. b. Assertion and reason both are correct statements but reason is not the correct explanation for assertion. c. Assertion is a correct statement but reason is a wrong statement. d. Assertion is a wrong statement but reason is a correct statement. 2. ASSERTION: The solubility of all gases in water decreases with the rise in temperature. REASON: The dissolution of gases in water is an endothermic process. a. Assertion and reason both are correct statements and reason is the correct explanation for assertion. b. Assertion and reason both are correct statements but reason is not the correct explanation for assertion. c. Assertion is a correct…