30 Ib. sucrose in 2.5-gallon solution You need to solve for grams of sucrose from the...
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30 Ib. sucrose in 2.5-gallon solution
You need to solve for grams of sucrose from the...
A) Calculate the molality of a sucrose solution made by dissolving 73.1 grams sucrose into 55.3...
A) Calculate the molality of a sucrose solution made by dissolving 73.1 grams sucrose into 55.3 grams water. The molar mass of sucrose is 342.2 g/mol. Record your answer in scientific notation using 3 significant figures. Use * for the multiplication symbol. B) A sodium hydroxide solution that contains 55.5 grams of NaOH per L of solution has a density of 1.14 g/mL. Calculate the molality of the NaOH in this solution. Record your answer to 2 decimal spaces. C)...
Experimental sucrose solution (final concentration) 30% 15% Amount of 30% stock sucrose solution needed 5 mL...
Experimental sucrose solution (final concentration) 30% 15% Amount of 30% stock sucrose solution needed 5 mL 2.5 mL 0.5 mL Amount of water needed O mL 2.5 mL 4.5 mL 3% 12. Make an additional 200 mL of 15% sucrose solution in Beaker 1 by mixing the 30% stock solution with water. Use the following dilution equation to solve for the necessary amount of stock solution MV, = M2V2 Where: • V1 = Needed volume of stock solution M =...
I need help converting some things from moles to grams, and grams to mL. However, some...
I need help converting some things from moles to grams, and grams to mL. However, some of these calculations need to be done using mass ratio... Convert 0.0537 mole of 30% hydrogen peroxide. **mass ration** - 30% by mass means that you have 30g of H2O2 per 100g of solution. Calculate the mass (g) and then convert to mL. A solution of Cyclohexene (88.8% by mass) and the phase transfer catalyst Aliquat 336 (11.2% by mass). 0.0122 mole of cyclohexene...
In Part A, you explored the relationship between molarity, the number of moles, and solution volume....
In Part A, you explored the relationship between molarity, the number of moles, and solution volume. However, when you prepare a solution, you are unable to directly measure the number of moles of solute. Instead, you can mass the solute and convert between the number of moles and mass using the molar mass of a substance as a conversion factor. The molar mass of a substance can be calculated based on its molecular formula; otherwise, it can be calculated from...
In Part A, you explored the relationship between molarity, the number of moles, and solution volume....
In Part A, you explored the relationship between molarity, the number of moles, and solution volume. However, when you prepare a solution, you are unable to directly measure the number of moles of solute. Instead, you can mass the solute and convert between the number of moles and mass using the molar mass of a substance as a conversion factor. The molar mass of a substance can be calculated based on its molecular formula; otherwise, it can be calculated from...
Need help with freezing point depression expeiment volume of acetic acid 30 volume of unknown solute...
Need help with freezing point depression expeiment volume of acetic acid 30 volume of unknown solute in solution1 1.5 volume of unknown solute in solution 2 1.5 freezing point of pure acetic acid 16.3 freezing point of solution 1 14.5 freezing point of solution 2 11.3 average molar mass of unknown solute Calculations for Part 1 The density of acetic acid is 1.049 g/mL and Kf(acetic acid) =3.90 °C·kg/mol The density of the unknown is 0.791 g/mL. 1.Calculate the masses...
8) What is the molarity (M) concentration of a solution when 18.37 grams of potasslum nitrite...
8) What is the molarity (M) concentration of a solution when 18.37 grams of potasslum nitrite (KNO,) is dissolved in water to make 120 mL of solution ? GENERAL CHEMISTRY LABORATORY II 9) What will the final molarity concentration of the solution in question 8 if the volume is doubled? 10) How many milliliters of 0.153 M KMnO, solution are needed to react with 6.44 grams of iron(II) sulfate in aqueous solution? The balanced reaction is: 10 Feso, + 2...
Learning Goal: A solution is prepared by dissolving 50.4 g sucrose (C H2011) in 0.384 kg...
Learning Goal: A solution is prepared by dissolving 50.4 g sucrose (C H2011) in 0.384 kg of water. The final volume of the solution is 355 ml HU solvent follows: 1 Review Constants Periodic Table MITAR MI HUBUNGI , the total number of moles in solution. The calculation of the mole fraction (x)is summarized as X- You may want to reference (Pages 586-592) Section 13.5 while completing this problem where the number of moles is calculated for both sucrose and...
1. The solubility of a gaseous solute in water is by an increase in pressure. Increased...
1. The solubility of a gaseous solute in water is by an increase in pressure. Increased decreased not affected 2. A supersaturated solution may be prepared by slowly cooling down a solution saturated at an elevated temperature. TRUE FALSE 3. A dilution is a solution made by adding a solvent to a supersaturated solution. TRUE FALSE 4. When sugar & water are mixed, a clear liquid results. In this scenario, the sugar is considered a Solute Solution Solvent All of...
In this problem, I am giving you grams of carbon dioxide gas. You need to convert...
In this problem, I am giving you grams of carbon dioxide gas. You need to convert this to moles in order to do the rest of the work. Please use the periodic table to convert the carbon dioxide mass into moles first. Every gallon of gasoline that you burn in your car puts about 8 884 grams of carbon dioxide into the air. At 22.0 degrees C, and at an outside pressure of 92.3 kPa, what volume of space would...
Experimental sucrose solution (final concentration) 30% 15% Amount of 30% stock sucrose solution needed 5 mL 2.5 mL 0.5 mL Amount of water needed O mL 2.5 mL 4.5 mL 3% 12. Make an additional 200 mL of 15% sucrose solution in Beaker 1 by mixing the 30% stock solution with water. Use the following dilution equation to solve for the necessary amount of stock solution MV, = M2V2 Where: • V1 = Needed volume of stock solution M =...
In Part A, you explored the relationship between molarity, the number of moles, and solution volume. However, when you prepare a solution, you are unable to directly measure the number of moles of solute. Instead, you can mass the solute and convert between the number of moles and mass using the molar mass of a substance as a conversion factor. The molar mass of a substance can be calculated based on its molecular formula; otherwise, it can be calculated from...
8) What is the molarity (M) concentration of a solution when 18.37 grams of potasslum nitrite (KNO,) is dissolved in water to make 120 mL of solution ? GENERAL CHEMISTRY LABORATORY II 9) What will the final molarity concentration of the solution in question 8 if the volume is doubled? 10) How many milliliters of 0.153 M KMnO, solution are needed to react with 6.44 grams of iron(II) sulfate in aqueous solution? The balanced reaction is: 10 Feso, + 2...
Learning Goal: A solution is prepared by dissolving 50.4 g sucrose (C H2011) in 0.384 kg of water. The final volume of the solution is 355 ml HU solvent follows: 1 Review Constants Periodic Table MITAR MI HUBUNGI , the total number of moles in solution. The calculation of the mole fraction (x)is summarized as X- You may want to reference (Pages 586-592) Section 13.5 while completing this problem where the number of moles is calculated for both sucrose and...
1. The solubility of a gaseous solute in water is by an increase in pressure. Increased decreased not affected 2. A supersaturated solution may be prepared by slowly cooling down a solution saturated at an elevated temperature. TRUE FALSE 3. A dilution is a solution made by adding a solvent to a supersaturated solution. TRUE FALSE 4. When sugar & water are mixed, a clear liquid results. In this scenario, the sugar is considered a Solute Solution Solvent All of...
In this problem, I am giving you grams of carbon dioxide gas. You need to convert this to moles in order to do the rest of the work. Please use the periodic table to convert the carbon dioxide mass into moles first. Every gallon of gasoline that you burn in your car puts about 8 884 grams of carbon dioxide into the air. At 22.0 degrees C, and at an outside pressure of 92.3 kPa, what volume of space would...
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