The mole fraction of Mgl2 of the solution in Part A is 1.59x10-2. Calculate the expected vapour pressure of the solution in Part A if the vapour pressure of pure water at 9.7 °C is 9.020 mmHg? 8.59 mmHg 9.16 mmHg O 8.88 mmHg O 7.73 mmHg O 0.431 mmHg

Q: A solution with a dnsity of 0.876 g/mL contains 5.0 grams of toluene and 225 grams of benzene.…

A: Applying formula of molarity M= n/Vl

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A: Since you have posted multiple questions, we will provide the solution only for the first question…

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A:

Q: (a) A solution is made by dissolving 13.5 g of glucose (C6H12O6) in 0.100 kg of water. What is the…

A: a) Since mass percentage is defined as the percentage of solute in the solution  i.e % m/m = mass of…

Q: ny grams of chlorine gas

A:

Q: Calculate

A: moles of Ba(OH)2 = mass / molar mass of Ba(OH)2  Moles of Ba(OH)2 = 9.50g / 171.34 gmol-1  moles of…

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A: we need to calculate the concentration of pesticide

Q: Calculate the mole fraction of the solute in a 0.112M aqueous solution of C6H12O6. The density of…

A:

Q: Calculate the molarity of 10.0g of NaC2H3O2 dissolved in 500 mL of aqueous solution.

A: Compound: NaC2H3O2  Molar mass = 82.03 g/mol given weight = 10g

Q: What is the boiling point of a 1.2 m Ca(NO3)2 solution?

A: Given,molality of Ca(NO3)2 = 1.2 m

Q: Given a 3.59 M solution of magnesium nitrate, Mg(NO3)2, whose density is 1.2 g/ml, determine its…

A: Molarity = moles/ volume in L Molality = moles / mass of solvent on kg

Q: Calculate the molarity of a solution that contains 2.25 molof NaNO3 dissolved in 2.50 L.

A: Given data contains, Moles of NaNO3 is 2.25 mol. Volume of solution is 2.50L.

Q: What is the percent by mass of a sodium sulfate solution in water with a mole fraction of sodium…

A: Mole Fraction of A =[Moles of A/(Moles of A + Moles of B)]Percent by mass of A =[Mass of A/(Mass of…

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A:

Q: Calculate the molarity of a 40.0% acetic acid (C₂H₄O₂) solution. The density of the solution is…

A:

Q: What is the concentration of an aqueous caffeine solution that is prepared by dissolving 36.8 g of…

A: In order to find the concentration of caffeine in the solution we first write down the given data:…

Q: Calculate the concentration of F−F− in solution and its absolute uncertainty.

A: Answer is 0.01185 ± 0.000059 mol/L  Absolute uncertainty  = 0.000059

Q: Calculate the freezing point of a 9.00 m aqueous solution of CaCl2

A: To solve this problem we will use the formula  ∆Tf = i Kf m  Where ,  ∆Tf = depression in freezing…

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Q: Convert 0.601 mol of ammonium (NH+4) ions to equivalents.

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A: Following are the appropriate answers of the given question .

Q: n = M x V For all parts of this problem, consider 7.50 L of an 8.91 x 10 mol/L Ca(OH), solution. -…

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Q: 500 g of anitifreeze, C2H6O2, is mixed with 750 g of water, H2O.  What is the freezing point of the…

A: Mass of antifreeze, C2H6O2 = 500 g Mass of water = 750 g Molecular weight of C2H6O2 = 62.07 g/mol…

Q: Calculate the molarity of 69.0 gg of HClHCl in 1.50 LL of an HClHCl solution.

A:

Q: If 2.5 mL of a 2.8% h2o2 solution from question 1 fully decomposes according to 2H2O2→2H2O+O2 how…

A: 2.8% means 2.8 g of H2O2 is present in 100 g of solution. Calculation of mol of H2O2 in 2.8%:…

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Q: Calculate the molarity of each aqueous solution:(a) 32.3 g of table sugar (C₁₂H₂₂O₁₁) in 100. mL of…

A: (a)

Q: What is the normality of 0.0566 M H3PO4?

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Q: Calculate the molarity of 153 grams of sucrose, C12H22O11, in 2.60 liters of solution

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Q: Calculate the grams of CuSO4.5H2O required to prepare 100.0ml of 0.0500 M CuSO4.5H2O.

A:

Q: Determine the molality of LiBr if 9.6141 g of LiBr was dissolved in 284.65 g of H2O. MW(LiBr) =…

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Q: This question has multiple parts: A solution is prepared by dissolving 155 g of glycine C 2 H 5 NO 2…

A:

Q: Calculate the molarity (MM) of 152.7 gg of H2SO4H2SO4 in 1.140 LL of solution.

A:

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A: Use the formula :

Q: How many grams of chlorine gas are needed to make 4.80× 10^6 of a solution that is 1.60 ppm chlorine…

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Q: I dissolve 100 grams of CaSO4 in 100mL of water. What is the molar concentration of the resulting…

A: Given, mass of CaSO4=100 g volume of water =100 mL= 100×10-3L=0.1 L

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.