CHEMISTRY REPOST

Calculate the concentration, in percent by mass, of a refrigerant brine solution which is 4.03 M in NaCl with a density of 1.116 g mL-1.

detailed answer, please, i don't understand how to do this at all!!!

1. 👍
2. 👎
3. 👁
1. Assume some volume, say 1 liter.

Then the mass is 1116grms, from the density.

4.03=moles/lites >> 4.03moles in solution.

mass solute= 4.03*molmassNaCl= 4.03*53

percentmass= masssolute/massollution * 100

1. 👍
2. 👎
👤
bobpursley
2. Just a quick note to say Bob P obviously hit the wrong key for molar mass NaCl. You should confirm this number yourself. It's closer to 58.5 but that isn't exact.

1. 👍
2. 👎
3. thanks a lot guys, i got it!!! :)

1. 👍
2. 👎

Similar Questions

1. Chemistry

1. What is the percent by mass of a solution that contains 50 grams of solute dissolved in 200 grams of solution? What is the concentration of the same solution in parts per million? 2. What is the percent mass of a solution that

2. chemistry

An aqueous solution of Na2SO4 has a molal concentration of 0.293 mol kg-1. Its density is 1.0350 g mL-1. Calculate the molar concentration of Na2SO4. ----- mol L-1 Calculate the mass percent of Na2SO4 in the solution. ------- %

3. chemistry

What is the percent by mass of 3.55 g NaCl dissolved in 88 g H2O? 2. A solution is made by adding 1.23 moles of KCl to 1000.0 g of water. What is the % by mass of KCl in this solution? 3. If you have 100.0 mL of a 25% aqueous

4. Chemistry

A is a solution of trioxonitrate (v)acid, HNO3 of unknown concentration.B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution. 25 cm3 portion solution B required an average of 24.00cm3 of solution A for

1. chemistry

A 2.500×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was

2. chemistry

A is a solution of trioxonitrate(v) acid, HNO3, of unknown concentration. B is standard solution of sodium hydroxide containing 4.00g per dm3 of solution. 25cm3 portions solution B required an average of 24.00cm3 of solution A for

3. REGENTS(PRACTICE)

A scientist wants to determine the best conditions for hatching brine shrimp eggs. In a laboratory, brine shrimp hatch at room temperature in glass containers of salt water. The concentration of salt in the water is known to

4. Chemistry

A is a solution of trioxonitrate(v)acid (nitric acid) HNO3 of unknown concentration.B is a standard solution of sodium hydroxide containing 4.00g per dm3 of solution a). Suggest with a reason,a suitable indicator for the reaction

1. Chemistry

Calculate the amount of water (in grams) that must be added to (a)5.00 g of urea (NH2)2CO in the preparation of a 16.2 percent by mass solution, and (b)26.2g of MgCl2 in the preparation of a 1.5 percent by mass solution.

2. Chemistryyy

a) A standard solution of 0.243 M NaOH was used to determine the concentration of a hydrochloric acid solution. If 46.33 mL of NaOH is needed to neutralize 10.00 mL of the acid, what is the molar concentration of the acid? b) A

3. Chem

A bottle of win contains 12.5% ethanol by volume. The density of ethanol (C2H5OH) is .79 g/mL. Calculate the concentration of ethanol in wine as mass percent and molality. I calculated molality as 2.4 m/kg, but I'm stumped on the

4. chemistry

A is a solution containing 5.00 g of HNO3 in 500 cm\(^3) of solution. B is a solution of NaOH of unknown concentration. 21.30cm3 of A was titrate it with 25.0 cm3 portions of B using methyl orange as an indicator. calculate the: