Answer the following questions concerning a 5.72 wt% acetic acid (CH3COOH) solution.4.If the solution has a density of 1.06 g/m L, then what is its concentration in molarity (mol/L)?a.b. The dissociation of acetic acid in water (below) has an equilibrium constant of 1.8 x 105.Use an "ICE" table to calculate [CH3COO] at equilibrium in molarity (mol/L). Hint: start withyour answer from part (a).CH3C00 (aq) + H30+ (aq)CH3COOH (aq) + H20 (I)

Solution stoichiometry involves the calculation of concentration of solutions in the given…

Answered: Answer the following questions…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter13: Solutions And Their Behavior

Section13.5: Colloids

Problem 2.4ACP

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Ben prepared a salicylic acid in pentanol solution by adding 4.77 g of salicylic acid to 91.88 mL of pentanol. Calculate the mole fraction of salicylic acid in this solution. MW of salicylic acid= 138.12 g/mol MW of pentanol= 88.15 g/mol Density of pentanol= 0.8144 g/mL
Gypsum (CaSO4) is a common percipitant in water desalination. CaSO4 <=> Ca2+ + SO42- where Ksp=10-4.6. Assuming that: [Ca2+]=2x10-2 M; [SO42-]=2x10-3M: a) Find Qsp or IAP for the given water b) Find the solubility index (SI) and determine whether CaSO4 is under, super, or at saturation in water. Feel free to make any assumptions you wish, as long as they're stated.
Barium chloride is reacted with sodium sulfate to produce barium sulfate and sodiumchloride. How many moles of the precipitate is produced from 0.8 moles of BaC12?A. 0.4 moleB. 0.8 moleC. 1.6 molesD. None of the above A 315mL of water was added to 2100 mL of 19M NaCI solution. What is the newconcentration of the solution?(Use the given information: MW: Na = 23 g/mol, C1 = 35g/mol)A. 2.85 MB. 2.48 MC. 18.60 MD 19.0 M 500g of Al2S3 is dissolved in H20 to make 15.0 L of solution. What is its normality? (MW:Al=27g/mol, S=32g/mol, H=1g/mol, 0=16g/molA. 0.11 NB. 0.07 NC. 0.22 ND. 0.04 N
How many grams of CaCl2are needed to make 314.0 g of a solution that is 30.0% w/w calcium chloride in water? How many grams of water are needed? 2. Isopropyl alcohol is mixed with water to produce a 36.0% v/v alcohol solution. How many mL of each liquid are present in 865 mL of this solution? (Assume the volumes are additive.) 3. Calculate the molarity of 27.7 g of MgS in 760.0 mL of solution. 4. If 6.35 g of Cu(NO3)2 is dissolved in water to make a 0.750 M solution, what is the volume of the solution (in mL)?
Calculate the solubility of BaSO4 in water at 25°C. You'll find Ksp data in the ALEKS Data tab. Round your answer to 2 significant digits.
You are to prepare each of the following 100-mL Test Reagents in the Laboratory with concentrations in: 5% (w/v) Sodium hydroxide Given atomic weight: Na- 22.99 O- 15.99 C- 12.01 H- 1.01 Use this formula in solving: mol (for moles) mol/L (for Molarity)mol/kg (for Molality) eg/L (for Normality) FIND: Number of moles of Sodium hydroxide: Number of moles of Solvent: Mole fraction of Solvent: Weight of solute needed to prepare the test reagent: Factor: Molarity: Molality: Normality: Please include complete solution
7.0 mL of 3.0 M NaOH are diluted with water to a volume of 400 mL. (a) Determine the molarity of the resulting solution. How many moles of NaOH there are in 7.0 mL of 3.0 M NaOH? Hint: Use Eq. 1 and make sure the volume is in liters: MA = mol A / soln (L) OR mol A = MA x V ___________ moles (b) The total number of moles of NaOH is not changed on dilution. The molarity after dilution can therefore be found by MA = mol A / soln (L) OR mol A = MA x V using the final volume of the solution. Calculate that molarity.
8. Find the final concentration of ethanol as a percent (v/v) when 30 mL of ethanol 50 % (v/v), 60 mL of ethanol 70 % (v/v), and 40 mL of ethanol 95 % (v/v) are mixed together.
A 10 ml of concentrated acetic acid was added in a sufficient quantity of water to make 350 ml of the acid solution. SG acetic acid= 1.05 kb acetate = 5.556x10^-10 What is the weight of acetic acid in grams? What is the molarity (mole/Liter) of acetic acid solution? What is the ka of acetic acid? What is the Hydronium ion concentration? What is the pH of the solution?
Calculate how many grams of phthalic acid remained in the chilled water (the “mother liquor”) based on the solubility data given (show your work). You will recrystallize phthalic acid, a compound that is used to manufacture synthetic polymers and perfumes. Phthalic acid is very soluble in boiling water, 18 g/100 mL, and is much less soluble in chilled (14°C) water, 0.54 g/100 mL. Thus, water is a very good recrystallization solvent for phthalic acid. 54.8% percent recovery was calculated
Saturated aqueous sodium chloride (d = 1.2 g/mL) is added to the followingmixtures in order to dry the organic layer. Which layer is likely to be on thebottom in each case?a. Sodium chloride layer or a layer containing a high-density organic compound dissolved in methylene chloride (d = 1.4 g/mL)b. Sodium chloride layer or a layer containing a low-density organic compound dissolved in methylene chloride (d = 1.1 g/mL)
1. Calculate the mass required to prepare a 250 mL 3 M NaCl in water.Mass = M x MM x V 10002. Calculate how to prepare the following dilutions, ½, ¼, 1/8 and 1/16 of the initial concentration.There is a helpful equation that is used to determine how much stock solution and how much diluent to combine to get the final solution of a desired concentration

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