19. 50.0 g of a 6.00% m/m KNO3 in water solution are mixed with 100. g...

Question

Question

Answer 1

Answer #1

Mass of KNO3 in 1st solution = 6.00 % of 50.0 g

= 6.00*50.0/100

= 3.00 g

Mass of KNO3 in 2nd solution = 10.00 % of 100.0 g

= 10.0*100/100

= 10.0 g

Total mass of KNO3 in mixture = 3.00 g + 10.00 g

= 13.00 g

Total mass of solution = 50.0 g + 100 g

= 150 g

Use:

Mass % of KNO3 = mass of KNO3 * 100 / mass of solution

= 13.00 * 100 / 150

= 8.67 %

Answer: a

Answer 2

Similar Homework Help Questions

Cumulative/Challenge Probtems 18. If a 50.0 mL sample of 6.00 M KNO, solution is diluted to...

Cumulative/Challenge Probtems 18. If a 50.0 mL sample of 6.00 M KNO, solution is diluted to 2.00 L, what volume of this new solution would contain 25.0 g KNO,?
A 48.8-mL sample of a 7.8 M KNO3 solution is diluted to 1.20 L . 1.What...

A 48.8-mL sample of a 7.8 M KNO3 solution is diluted to 1.20 L . 1.What volume of the diluted solution contains 10.0 g of KNO3? (Hint: Figure out the concentration of the diluted solution first.)Express your answer using two significant figures. 2. To what volume should you dilute 130 mL of an 8.00 M CuCl2 solution so that 50.0 mL of the diluted solution contains 5.7 g CuCl2? Express your answer using two significant figures.
In a coffee-cup calorimeter, 50.0 ml of .100 M AgNO3 and 50.0 ml of .100 M...

In a coffee-cup calorimeter, 50.0 ml of .100 M AgNO3 and 50.0 ml of .100 M HCl are mixed to yield the following reaction: Ag+(aq) + Cl-(aq) --> AgCl(s) The two solutions were initially at 22.6°C and the final temp is 23.4°C. Assume that the final solution has a mass of 10.0 g and has a specific heat capacity of 4.184 J/g°C. Calculate delta for the reaction in kJ/mole of AgCl formed.

When 4.102 g of KNO3 is dissolved in 39.825 g of water in a "coffee-cup calorimeter"...

When 4.102 g of KNO3 is dissolved in 39.825 g of water in a "coffee-cup calorimeter" at 24 degrees Celsius, the temperature of the solution went down to 19 degrees Celsius. a.) Is this solution reaction exothermic or endothermic? Why? b.) Calcualate qH2O using Eq. 1. c.) Find as it occured in the calorimeter (Eq. 4). d.) Find for the solution of one mole KNO3 in water. e.) Find for the solution of 1.00 g KNO3 in water.
A solution contains 110 g of KNO3 per 100 g of water at 50 degrees Celsius....

A solution contains 110 g of KNO3 per 100 g of water at 50 degrees Celsius. Is the solution saturated, unsaturated, or supersaturated? The graph in the previous problem may be helpful.
5. The solubility of KCl (in grams KCl/100 g of water) is 31.0 g at 10.0...

5. The solubility of KCl (in grams KCl/100 g of water) is 31.0 g at 10.0 °C, 34.0 g at 20.0 °C, 42.6 g at 50.0 °C, and 56.7 at 100 °C. a) You want to make a saturated solution of KCl at 50.0 °C using 2.00 L of water. How many grams of KCl are necessary to make this solution? You may assume that the density of water is 1.00 g/mL. b) You then take your saturated solution of...

A KNO3 solution containing 32 g of KNO3 per 100.0 g of water is cooled from...

A KNO3 solution containing 32 g of KNO3 per 100.0 g of water is cooled from 37 ∘C to 0 ∘C . What mass of KNO3 will precipitate? PLEASE SHOW WORK!
A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL...

A 50.0 mL sample of a 1.00 M solution of CuSO4 is mixed with 50.0 mL of 2.00 M KOH in a calorimeter. The temperature of both solutions was 20.3°C before mixing and 31.7 °C after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate AH for the process: CuSO4(1M) + 2KOH(2M) +Cu(OH)2 (s) + K2SO4(0.5M) Assume that the specific heat and density of the solution after mixing are the same as those of pure...
the date you need is: 2.0 grams of KNO3, the temp was 22.1. extra information that might help if you need it: I added 5 mL of water to the 2.0 g of KNO3. please answer the 3 parts of the question. T...

the date you need is: 2.0 grams of KNO3, the temp was 22.1. extra information that might help if you need it: I added 5 mL of water to the 2.0 g of KNO3. please answer the 3 parts of the question. Thanks. Grams KNO,Cryst. Temp, °c 22.1 2.0 g Type your calculation for solubility (in grams KNO,/100 grams water) using the data for the 2.0 gram sample. Type your calculation for molality of KNO, (in mol KNO3/kg water) using...

50.0 g of water at 22 °C is mixed with 125 g of water initially at...

50.0 g of water at 22 °C is mixed with 125 g of water initially at 36 °C. What is the final temperature of the water after mixing, assuming no heat is lost to the surroundings?