Question

In: Chemistry

Kemmi pipets 25.00 mL of pure 1-propanol (C3H7OH, a liquid organic alcohol) into a 100.0 mL...

Kemmi pipets 25.00 mL of pure 1-propanol (C3H7OH, a liquid organic alcohol) into a 100.0 mL volumetric flask. She dilutes it with water. Help her calculate the strength of her diluted solution.

Volumes: 25.00 mL volumetric pipet, 100.00 mL volumetric flask.

Molar mass of pure 1-propanol: 60.09 g/mol. Density of pure 1-propanol: 0.803 g/mL

Calculate the number of moles in exactly 25.00 mL of 1-propanol. (3 significant figures; units of mol)  [x]

Calculate the molarity of the diluted solution. (3 significant figures; units of M or mol/L)  [y]

Solutions

Expert Solution

V = 25 mL
density = 0.803 g/mL
mass of propanol= V* density
                                   = 25 mL*0.803 g/mL
                                   = 20.075 g
Molar mass = 60.09 g
number of moles of propanol = mass / molar mass
                                                             = 20.075/60.09
                                                             = 0.334 mol

Final volume = 100 mL = 0.1 l
final concentration = number of moles / volume
                                        = 0.334/0.1
                                        = 3.34 M
Answer: X = 0.334 mol
Y= 3.34 M


Related Solutions

al alcohol solution contains 35.0g of propanol (C3H7OH ) and 150.0g of ethanol . Calculate the...
al alcohol solution contains 35.0g of propanol (C3H7OH ) and 150.0g of ethanol . Calculate the mass percent of propanol : 45.6, 18.9, 25.3. 67.9, 81.1
An organic chemist has discovered a catalyst that reacts 2-propanol (C3H7OH) with water to form ethanol...
An organic chemist has discovered a catalyst that reacts 2-propanol (C3H7OH) with water to form ethanol (C2H5OH). 1.23 L of 90% (by mass) 2-propanol mixed with water (10% by mass) is treated with the catalyst. The reaction goes to completion. The specific gravity of the solution is 0.82. 1. What is the balanced chemical equation for the reaction? 2.How much 2-propanol is in the solution (in gmol)?
 3. What is the limiting reagent?
 4. What percent of the non-limiting reagent...
If you combine 360.0 mL of water at 25.00 °C and 100.0 mL of water at...
If you combine 360.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.
If you combine 330.0 mL of water at 25.00 °C and 100.0 mL of water at...
If you combine 330.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.
f you combine 320.0 mL of water at 25.00 °C and 100.0 mL of water at...
f you combine 320.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.
An organic liquid is a mixture of methyl alcohol (CH3OH) and ethyl alcohol (C2H5OH). A 0.220-g...
An organic liquid is a mixture of methyl alcohol (CH3OH) and ethyl alcohol (C2H5OH). A 0.220-g sample of the liquid is burned in an excess of O2(g) and yields 0.380 g CO2(g) (carbon dioxide). Set up two algebraic equations, one expressing the mass of carbon dioxide produced in terms of each reagent and the other expressing the mass of sample burned in terms of each reagent. What is the mass of methyl alcohol (CH3OH) in the sample?
An organic liquid is a mixture of methyl alcohol (CH3OH) and ethyl alcohol (C2H5OH). A 0.220-gsample...
An organic liquid is a mixture of methyl alcohol (CH3OH) and ethyl alcohol (C2H5OH). A 0.220-gsample of the liquid is burned in an excess of O2(g) and yields 0.348 g CO2(g) (carbon dioxide). Set up two algebraic equations, one expressing the mass of carbon dioxide produced in terms of each reagent and the other expressing the mass of sample burned in terms of each reagent. What is the mass of methyl alcohol (CH3OH) in the sample?
An organic liquid is a mixture of methyl alcohol (CH3OH) and ethyl alcohol (C2H5OH). A 0.220-g...
An organic liquid is a mixture of methyl alcohol (CH3OH) and ethyl alcohol (C2H5OH). A 0.220-g sample of the liquid is burned in an excess of O2(g) and yields 0.376 g CO2(g) (carbon dioxide). Set up two algebraic equations, one expressing the mass of carbon dioxide produced in terms of each reagent and the other expressing the mass of sample burned in terms of each reagent. What is the mass of methyl alcohol (CH3OH) in the sample?
The vapor pressures of ethanol (C2H5OH) and 1−propanol (C3H7OH) at 35°C are 100 mmHg and 37.6...
The vapor pressures of ethanol (C2H5OH) and 1−propanol (C3H7OH) at 35°C are 100 mmHg and 37.6 mmHg, respectively. Assume ideal behavior and calculate the partial pressures of ethanol and 1−propanol at 35°C over a solution of ethanol in 1−propanol, in which the mole fraction of ethanol is 0.277. P1−propanol = mmHg
Calculate the energy change (with the correct sign) when the temperature of 100.0 mL of liquid...
Calculate the energy change (with the correct sign) when the temperature of 100.0 mL of liquid water decreases by 3.40 ∘ C. Calculate the mass of KCl needed to absorb the same amount of energy when dissolved in water. ΔHsolution(KCl)=983.5 J/mol.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT