2.65 g of Ba(OH)2 is dissolved in 70.0 mL of water to produce a saturated solution...

2.65 g of Ba(OH)₂ is dissolved in 70.0 mL of water to produce a saturated solution at 20⁰C. Calculate the solubility in units of g/100 mL; g/L ; and M.

Solutions

Expert Solution

Molar mass of Ba(OH)₂ = [1*137.327 + 2*(15.9994 + 1.008)] g/mol = 171.3418 g/mol.

Moles of Ba(OH)₂ = (2.65 g)/(171.3418 g/mol) = 0.01547 mole.

Volume of water taken = 70.0 mL = (70.0 mL)*(1 L/1000 mL) = 0.07 L.

70.0 mL water contains 2.65 g Ba(OH)₂.

Therefore, 100.0 mL water contains (2.65 g)*(100 mL/70 mL) = 3.7857 g ≈ 3.786 g.

Solubility of Ba(OH)₂ = 3.786 g/100 mL (ans).

Again 100 mL water = (100 mL)*(1 L/1000 mL) = 0.100 L.

Solubility of Ba(OH)₂ in a liter of water = (3.786 g/100 mL) = (3.786 g/0.100 L) = 37.86 g/L (ans).

Solubility of Ba(OH)₂ in M = (0.01547 mole)/[(70.0 mL)*(1 L/1000 mL)] = (0.01547 mole)/(0.07 L) = 0.221 mol/L = 0.221 M (ans).

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

In a constant-pressure calorimeter, 70.0 mL of 0.300 M Ba(OH)2 was added to 70.0 mL of...

In a constant-pressure calorimeter, 70.0 mL of 0.300 M Ba(OH)2 was added to 70.0 mL of 0.600 M HCl. The reaction caused the temperature of the solution to rise from 21.98 °C to 26.07 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g·°C, respectively), what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.

You dissolve 10.0 g of mixture of NaOH and Ba(OH)2 in 240.0 ml water and titrate...

You dissolve 10.0 g of mixture of NaOH and Ba(OH)2 in 240.0 ml water and titrate with 1.55 M hydrochloric acid. The titration is complete after 108.5 ml of the acid has been acid. What is mass in grams of NaOH and Ba(OH)2

You dissolve 10.0 g of mixture of NaOH and Ba(OH)2 in 240.0 ml water and titrate...

A 0.4400-g sample of impure Ca(OH)2 is dissolved in enough water to make 60.30 mL of...

A 0.4400-g sample of impure Ca(OH)2 is dissolved in enough water to make 60.30 mL of solution. 20.00 mL of the resulting solution is then titrated with 0.1461-M HCl. What is the percent purity of the calcium hydroxide if the titration requires 18.33 mL of the acid to reach the endpoint?

You added 20 mL of 0.20M solution of Ba(OH)2(aq) to 50 mL of 0.10M solution of...

You added 20 mL of 0.20M solution of Ba(OH)2(aq) to 50 mL of 0.10M solution of HCl(aq). The pH of the resulting solution is ________.

Solution of Ba(OH)2 has pH=12.10. How many grams of Ba(OH)2 contain 250.0mL of solution?

If 4.90 g of Na2CO3 is dissolved in enough water to make 250. mL of solution,...

If 4.90 g of Na2CO3 is dissolved in enough water to make 250. mL of solution, what is the molar concentration of the sodium carbonate? Molar concentration of Na2CO3 = ______M What are the molar concentrations of the Na+ and CO32- ions? Molar concentration of Na+ = ______M Molar concentration of CO32- = _______M

A 1.00-g sample of piperazine hexahydrate is dissolved in enough water to produce 100.0 mL of...

A 1.00-g sample of piperazine hexahydrate is dissolved in enough water to produce 100.0 mL of solution and is titrated with 0.500 M HCl. A.) What is the initial pH of the solution, before any titrant is added? B.) The percent neutralization points for a titration indicate the percent of the reagent that has reacted. For example, at the 25% neutralization point for piperazine, 75% (0.75×[Pip]) of the base remains, and 25% is neutralized to form PipH+. Calculate the pH...

If I collect 14 grams of Ba(OH)2 and add it to water, what kind of solution...

If I collect 14 grams of Ba(OH)2 and add it to water, what kind of solution do you expect to be formed (acidic or basic)? Suppose that I make up a solution that is 750 ml using this barium salt and add it to my buret. I collect 6 grams of a solid material and titrate it against the barium, and I do this a total of 3 times. The volumes of barium containing solution used were: 22.9 ml, 24...

The B4O5(OH)4^2- ion, present in 5.0-Ml of a saturated Na2B4O5(OH)4 solution at a measured temperature, is...

The B4O5(OH)4^2- ion, present in 5.0-Ml of a saturated Na2B4O5(OH)4 solution at a measured temperature, is titrated to the bromocresol endpoint with 3.25 mL of 0.291 M HCl. a) How many moles of B4O5(OH)4^2- are present in the sample? b) What is the molar concentration of B4O5(OH)4^2- in the sample? c) Calculate the Ksp for Na2B4O5(OH)4 from this data. d) What is the free energy change for the dissolution of Na2B4O5(OH)4 at this temperature?

Subjects