A student makes a solution that is 35.00% (by mass) nitric acid in water. Determine the...
A student makes a solution that is 35.00% (by mass) nitric acid in water. Determine the molality of the nitric acid, if the solution has a density of 1.340 g/mL? (Show work)
a.) 9.568 m
b.) 17.51 m
c.) 12.98 m
d.) 10.73 m
e.) 8.545 m
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A student makes a solution that is 35.00% (by mass) nitric acid
in water. Determine the...
17. The density of nitric acid (which is HNO3 in water) is 1.42 g/mL. The m/m% of HNO, in nitric acid is 69% m/m. H...
17. The density of nitric acid (which is HNO3 in water) is 1.42 g/mL. The m/m% of HNO, in nitric acid is 69% m/m. How many grams of HNO3 are in 1 mL of nitric acid? a) 0.99g b) 99g c) 2.1g d) 0.021 g e) 0.49g
A student makes a solution for analysis by mixing 5.86 grams of Cu2SO4 into 283.2 grams...
A student makes a solution for analysis by mixing 5.86 grams of Cu2SO4 into 283.2 grams of water. The density of water at the temperature of the lab at the time the solution was made is 0.9926 g/mL. Calculate the molarity, molality, mole fraction, and mass percent of the copper I sulfate. • The molarity of the solution is: 0.09 * • The molality of the solution is: 0.09 * • The mole fraction of the solution is: 0.001269* •...
3. Concentrated nitric acid is 70.4% HNO, by mass and has a density of 1.42 g/mL....
3. Concentrated nitric acid is 70.4% HNO, by mass and has a density of 1.42 g/mL. What is the molarity of concentrated nitric acid? a. 11.2 M b. 55.5 M c. 7.87 M d. 14.6 M e. 15.9 M
I Caleulat mdar.concentration of acetic acid (CH3 COOH in 35.00% vinegar 5100% solution of acetic acid...
I Caleulat mdar.concentration of acetic acid (CH3 COOH in 35.00% vinegar 5100% solution of acetic acid inutter Density of the vinegar is 1.080/mL. Isemolar mass of acetic acidas 60.05 g/mol. Show your work to gethulleredit.
Introductory chemistry 20 A nitric acid solution containing 71.0% HNO3 (by mass) has a density of...
Introductory chemistry
20 A nitric acid solution containing 71.0% HNO3 (by mass) has a density of 1.42 g/mL. ow many moles of HNO, are present in 2.36 L of this solution? b) Determine the molarity of the acid.
Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and...
Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and has a density of 1.41 g/mL. How much concentrated solution would you take to prepare 1.30 L of 0.105 M HNO3by mixing with water?
Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and...
Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and has a density of 1.41 g/mL. How much concentrated solution would you take to prepare 1.05 L of 0.120 M HNO3 by mixing with water?
Vitamin C or Ascorbic acid (C6H8O6) is a water soluble vitamin. A solution is prepared by...
Vitamin C or Ascorbic acid (C6H8O6) is a water soluble vitamin. A solution is prepared by dissolving 80.5 g of Ascorbic acid in 210 g of water. The resulting solution has a density of 1.22 g/ml. Calculate the concentration of Ascorbic acid in terms of a) Mass Percent b) Mole fraction c) Molality d) Molarity
40. What is the molality of a 30.0% by mass hydrochloric acid solution? The density of...
40. What is the molality of a 30.0% by mass hydrochloric acid solution? The density of the solution is 1.1493 g/mL. a. 0.300 m b. 9.46 m 11.8 m 0.0345 m e. 9.30 m work?
B. Commercial nitric acid comes in a concentration of 16.0 mol/L. The density of this solution...
B. Commercial nitric acid comes in a concentration of 16.0 mol/L. The density of this solution is 1.42 g/mL Calculate the percent (w/w) of nitric acid, HNO3, in this solution. How many milliliters of the concentrated acid have to be taken to prepared 250 g of a solution that is 10.0%(w/w) HNO3? C. Citric acid, H3C6H5O7, occurs in plants. Lemons contain 5% to 8% citric acid by mass. The acid is added to beverages and candy. An aqueous solution...
17. The density of nitric acid (which is HNO3 in water) is 1.42 g/mL. The m/m% of HNO, in nitric acid is 69% m/m. How many grams of HNO3 are in 1 mL of nitric acid? a) 0.99g b) 99g c) 2.1g d) 0.021 g e) 0.49g
A student makes a solution for analysis by mixing 5.86 grams of Cu2SO4 into 283.2 grams of water. The density of water at the temperature of the lab at the time the solution was made is 0.9926 g/mL. Calculate the molarity, molality, mole fraction, and mass percent of the copper I sulfate. • The molarity of the solution is: 0.09 * • The molality of the solution is: 0.09 * • The mole fraction of the solution is: 0.001269* •...
3. Concentrated nitric acid is 70.4% HNO, by mass and has a density of 1.42 g/mL. What is the molarity of concentrated nitric acid? a. 11.2 M b. 55.5 M c. 7.87 M d. 14.6 M e. 15.9 M
I Caleulat mdar.concentration of acetic acid (CH3 COOH in 35.00% vinegar 5100% solution of acetic acid inutter Density of the vinegar is 1.080/mL. Isemolar mass of acetic acidas 60.05 g/mol. Show your work to gethulleredit.
Introductory chemistry
20 A nitric acid solution containing 71.0% HNO3 (by mass) has a density of 1.42 g/mL. ow many moles of HNO, are present in 2.36 L of this solution? b) Determine the molarity of the acid.
40. What is the molality of a 30.0% by mass hydrochloric acid solution? The density of the solution is 1.1493 g/mL. a. 0.300 m b. 9.46 m 11.8 m 0.0345 m e. 9.30 m work?
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