The density of a 0.438 M solution of potassium chromate (K2CrO4) at 298 K is 1.063...

The density of a 0.438 M solution of potassium chromate (K2CrO4) at 298 K is 1.063 g/mL. a.Calculate the vapor pressure of water above the solution. The vapor pressure of pure water at this temperature is 0.0313 atm. Assume complete dissociation.

Expert Solution

raoults law

P0-P/P0 = i*Xsolute

P = vapor pressure of water above the solution = ?

p0 = vapor pressure of pure water at this temperature = 0.0313 atm

Molarity = w/w%*d*10 / Mwt

Mwt = molarmass of K2CrO4 = 194.2 g/mol

density = 1.063 g/ml

w/w% = 0.438*194.2/(1.063*10) = 8% by mass

means 8 g K2cro4 present in 100 g solution

no of mole of K2cro4 = w/mwt = 8/194.2 = 0.04 mol

no of mole of water in solution = (100-8)/18 = 5.11 mol

, XK2CrO4 = molefraction of K2CrO4 = 0.04/(5.11+0.04) = 0.0077

i = vanthof factor of K2CrO4 = 3

(0.0313-p)/0.0313 = 3*0.0077

p = vapor pressure of water above the solution = 0.0306 atm

queen_honey_blossom answered 2 years ago

What is the solubility ( in g/L) of lead(II) chromate, PbCrO4 in 0.13M potassium chromate, K2CrO4.

if a titration using these solutions started with 25.00 mL of potassium chromate solution (0.5056 M),...

if a titration using these solutions started with 25.00 mL of potassium chromate solution (0.5056 M), what volume of 0.2456 M lead (II) nitrate solution would be required to reach the end point? what MASS of the products would be created in that reaction?

when a solution of lead(ii) nitrate is mixed with a solution of potassium chromate, a yellow...

when a solution of lead(ii) nitrate is mixed with a solution of potassium chromate, a yellow precipitate forms according to the equation: Pb(NO3)2 (aq) + K2CrO4 (aq) -> 2 KNO3 (aq) + PbCrO4. Volume of 0.105 M lead(ii) nitrate react with 100.0 ml of 0.120 M potassium chromate. What mass of PbCrO4 will be formed?

A solution contains 1.43×10-2 M potassium bromide and 1.37×10-2 M ammonium chromate. Solid silver nitrate is...

A solution contains 1.43×10-2 M potassium bromide and 1.37×10-2 M ammonium chromate. Solid silver nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of silver ion when this precipitation first begins? [Ag+] = M

Calculate the pH of the cathode compartment solution if the cell emf at 298 K is...

Calculate the pH of the cathode compartment solution if the cell emf at 298 K is measured to be 0.600 V when [Zn2+]= 0.21 M and PH2= 0.87 atm . Express answer using two decimal places. Thank you!

Given the following solution, 50.00 mL 0.10M Potassium Chlorate, K2CrO4 answer the following. 1) What volume(mL)...

Given the following solution, 50.00 mL 0.10M Potassium Chlorate, K2CrO4 answer the following. 1) What volume(mL) of the solution contains 5.00 x 10^-4 miles of the solute? 2) What volume of the solution contains 1.00 g of the solute? 3) What is the new molarity of a solution made by pipeting 5.00 mL of the solution and diluting with 95.00 mL of deionized water? 4) What volume of the solution is required to react with 10.00 mL of 0.10M Pb(NO3)2?...

Which of the following types of substances are weak electrolytes in aqueous solution at 298 K?...

Which of the following types of substances are weak electrolytes in aqueous solution at 298 K? CHOOSE ALL CORRECT ANSWERS, there may be more than one correct answer. weak acids strong bases aminium salts ionic salts metals strong acids weak bases non-metals metalloids

Silver chromate is more soluble in solutions containing some (less than 1 M) potassium nitrate, even...

Silver chromate is more soluble in solutions containing some (less than 1 M) potassium nitrate, even though neither potassium nor nitrate show up in the BCE for the dissolution reaction Ag2CrO4 (s) ↔ 2 Ag+(aq) + CrO4 2-(aq) The solubility product constant (which is not the same as the solubility!) for silver chromate is Ksp = 1.1 x 10-12 making it a pretty insoluble substance. Your job is to figure out the molar solubility in pure water, then the molar...

If the density of water is 1g/mL and the density of a 0.16 M HCl solution...

If the density of water is 1g/mL and the density of a 0.16 M HCl solution is 1.023 g/mL, how do I use this information to determine the mass of both water and HCl in one liter of the solution? ***Cancel this question! I figured it out!

1. An aqueous solution of potassium hydroxide is standardized by titration with a 0.117 M solution...

1. An aqueous solution of potassium hydroxide is standardized by titration with a 0.117 M solution of hydrobromic acid. If 18.7 mL of base are required to neutralize 15.7 mL of the acid, what is the molarity of the potassium hydroxide solution? 2. .An aqueous solution of nitric acid is standardized by titration with a 0.183 M solution of calcium hydroxide. If 28.5 mL of base are required to neutralize 21.4 mL of the acid, what is the molarity of...

Question