A. The typical concentration for the hydrochloric acid is 18.0% by mass of the solution in water....
Question:
A. The typical concentration for the hydrochloric acid is 18.0% by mass of the solution in water. The density of this solution is 1.154 grams per millilitre (at 20 degree Celsius) and {eq}6.0 \times 10^5 {/eq} liters of the solution is used per year. How many kilograms of pure hydrochloric acid (not the solution) is used per year? Show your work.
B. The hydrochloric acid density drops 0.010 grams per millilitre for every 1 degree Celsius of temperature drop. If the acid is cooled by 28 degree Fahrenheit, what will be the new density if it started at the same temperature as the problem above? Show your work.
Density, Volume, and Temperature:
Density is a physical property that describes the distribution of mass in volume. Given that volume changes with temperature, density also changes with temperature. Considering that temperature and volume are directly proportional, the relationship between temperature and density is inversely proportional. When the temperature increases, the density decreases.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerA. We use the density ({eq}\rho {/eq}) and volume ({eq}V {/eq}) of the solution to calculate the mass ({eq}m {/eq}) of the solution.
Mass of...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Density: Definition, Formula & Practice Problems
from
Chapter 1 / Lesson 10
81K
Define key words such as matter, mass, volume, density, and buoyancy. Use the density formula to solve density example problems for density, volume, and mass.
Related to this Question
- The density of a solution of hydrochloric acid is 1.1492 g/cc, and it is 30.00 percent by mass. What volume of the solution (in milliliters) do you need to supply 37.0 g of hydrochloric acid?
- The density of a solution of hydrochloric acid is 1.0929 g / cc, and it is 19.00 percent by mass. What volume of the solution (in millilitres) do you need to supply 30.0 g of hydrochloric acid?
- Concentrated hydrochloric acid is an aqueous solution that is 37.2 % HCl. The density of the solution is 1.19 g/mL. What mass of HCl is contained in 0.683 L of solution? Give your answer as a whole number.
- A solution of hydrochloric acid in water is 38.0% by mass. Its density is 1.1886 g/mL. For this solution, calculate each of the following with respect to hydrochloric acid. a. molarity b. molality c. mole fraction d. mass/volume percent
- Concentrated hydrochloric acid is a 38% w/w solution of HCl in water and has a density of 1.18 g/ml. How many millilitres of concentrated hydrochloric acid are needed to prepare 500 ml of a 1:200 w/v
- What is the molarity of a 40.0% by mass hydrochloric acid solution? The density of the solution is 1.1980 g/mL. a) 18.3 M b) 13.1 M c) 0.0479 M d) 0.400 M e) 13.9 M
- What is the % mass of 12 M hydrochloric acid? The density of 12 M hydrochloric acid solution is 1.18 g/mL and the density of water is 1.00 g/mL.
- A solution of 45% hydrochloric acid has a density of 1.21 g/mL at 20 degrees Celsius. A 25 mL sample of this solution is mixed with enough water to increase the volume of the final solution to 150 mL. Find the molarity of the final solution.
- An aqueous solution of 0.975 M hydrochloric acid has a density of 1.02 g/mL. What is the percent by mass of HCl in the solution?
- The density of a solution of hydrochloric acid is 1.1492 g/cc, and it is 30.00 percent by mass. What volume of the solution (in mL) do you need to supply 37.0 g of hydrochloric acid?
- A certain supply of concentrated hydrochloric acid has a concentration of 36.0% HCl in water solution. The density of the solution is 1.19 g/mL. Calculate the molarity of HCl in the solution.
- Concentrated hydrochloric acid is usually available at a concentration of 37.7% by mass. What is its molar concentration? (The density of the solution is 1.19 g/mL.)
- Concentrated hydrochloric acid is 36.5 % (w/w) and has a density of 1.20 g/mL. What is the molar concentration of this solution?
- The mass percentage of hydrochloric acid within a solution is 10.00%. Given that the density of this solution is 1.049 g/mL, find the molarity of the solution.
- The mass percentage of hydrochloric acid within a solution is 40.00%. Given that the density of this solution is 1.200 g/mL, find the molarity of the solution.
- The mass percentage of hydrochloric acid within a solution is 15.00%. Given that the density of this solution is 1.075 g/mL, find the molarity of the solution.
- 0.2 grams of HCl is dissolved in 0.8 g of water. The density of the solution formed is 1.10 g/mL. What is the molarity of the solution?
- The concentration of a solution of HCl is 33.1% by mass, and its density was measured to be 1.147 g/mL. How many milliliters of the HCl solution is required to obtain 10.0 g of HCl?
- An aqueous 1.50 M hydrochloric acid solution is prepared with a total volume of 0.200 L What mass of hydrochloric acid (in grams) is needed for the solution?
- Concentrated hydrochloric acid is a 38% solution of HCl in water and has a density of 1.18g/ml. How many milliliters of concentrated hydrochloric acid is needed to prepare 500ml of 1:200 HCl solution?
- An aqueous solution is 10.0% by mass hydrochloric acid, HCl, and has a density of 1.05 g/mL. The molarity of hydrochloric acid in the solution is M.
- A solution of hydrochloric acid is 37.2% HCl. Express this concentration in molarity and mole fraction, and molarity (density of the solution is 1.034 g/mL).
- Concentrated hydrochloric acid has a concentration of 12.1 moles per liter. How many milliliters of the concentrated acid should be used to create 3.25 L of a 0.100 M solution?
- An aqueous solution is 3.50% by mass hydrochloric acid and has a density of 1.02 g/mL. What is the mole fraction of hydrochloric acid in this solution?
- An aqueous solution is 10.0 % by mass hydrochloric acid, HCl, and has a density of 1.05 g/mL. What is the mole fraction of hydrochloric acid in the solution ?
- An acid solution is 5.00% HCl by mass. Assuming that the density of the solution is 1.0 g/mL, find the molarity of the hydrogen ion in the solution. The molar mass of HCl is 36.5 g/mol.
- Given 100 mL of pure water at 40 degree C, what volume of a solution of hydrochloric acid, with a density of 1.175 g / mL and containing 34.4 % HCI by weight, could be prepared?
- How much 37% concentrated hydrochloric acid (with a density of 1.20 g/mL) is needed to make 2.5 liters of a 0.50 M hydrochloric acid solution.
- Calculate the molarity of a 10.0% (by mass) aqueous solution of hydrochloric acid. (a) 0.274 M (b) 2.74 M (c) 3.04 M (d) 4.33 M (e) The density of the solution is needed to solve the problem.
- Concentrated hydrochloric acid is a 38% solution of HCl in water and has a density of 1.18g/ml. How many milliliters of concentrated hydrochloric acid is needed to prepare 500ml of a 1:200 HCl solutio
- A certain HCl solution is 30 percent HCl and has a density of 1.2 g/mL. What mass of HCl is present in 167 mL of this solution? (a) 2.2 times 10^2 g (b) 60 g (c) 39 g (d) 6.9 times 10^2 g (e) 85 g
- A solution of HCl has a specific gravity of 1.120 and contains 23.81% HCl by wt. How many grams and how many milliequivalents of HCl are present in each milliliter of the solution?
- Hydrochloric acid is usually obtained as a 36% hydrochloric acid solution. If it is 13.42 M, what is the density of this solution? What is its molality? Density = g/mL Molality = m No need to show work.
- You have a 12 M solution of hydrochloric acid. How many milliliters of this solution will give 25.0 mL of 2.0 M hydrochloric acid when diluted?
- What is the molarity of a solution that contains 0.0372 moles hydrochloric acid in 1.2 liters of solution?
- An aqueous stock solution is 36.0% HCl by mass and its density is 1.18 g/mL. What volume of this solution is required to make 1.25 L of 1.65 mol/L HCl(aq)? Give your answer in millilitres, accurate to three significant figures.
- How many grams of a 0.30 M solution of hydrochloric acid would contain 5.2 g of pure hydrochloric acid? The density of 0.30 M hydrochloric acid is 1.2 g/mL.
- What is the molarity of hydrochloric acid in a solution containing 88.5 g of HCl in 215 mL of solution.
- Hydrochloric acid is usually purchased in concentrated form with a 37.0% HCl concentration by mass and a density of 1.20 g/mL. How much of the concentrated stock solution in milliliters should you use
- A solution of HCl is prepared by dissolving 5.00 mL of HCl in 55.0 g of water. What is the mass percent of HCl? (Density of HCl is 1.23 g/mL)
- According to the label on a bottle of concentrated hydrochloric acid, the contents are 36.0% HCl by mass and have a density of 1.18 g/mL. What volume of it would you need to prepare 789 mL of 2.20 M HCl solution?
- Concentrated hydrochloric acid is 12 M. What is the molarity of an HCl solution prepared by diluting 10.0 mL of concentrated acid to a total volume of 250.0 mL?Concentrated hydrochloric acid is 12 M.
- Calculate the molarity of a hydrochloric acid solution that is 26.4% HCl by mass and has a density of 1.19 g/mL.
- You are using a concentrated hydrochloric acid solution (12.0 M) to make 445.0 ml of a 5.85 M solution. Calculate the number of milliliters of concentrated HCl required to make the solution.
- How much quantity is needed to prepare 250 mL of 0.1 M hydrochloric acid solution from commercially available 35% hydrochloric acid (density = 1.16)?
- 1. Common commercial hydrochloric acid is an aqueous solution that is 38% HCl by mass, with a density of 1.19 g/cm^3. a. Calculate the molarity of this reagent. b. Calculate the molality of this reage
- Conversions: 4.00 wt% HCl(aq) solution has a density of 1.0181 g/ml at 20 degrees C. Convert the weight percent to these concentration units: a. the molality of HCl solution b. the molarity of HCl solution ...
- The commercial concentrated hydrochloric acid is rated at 38 w/w%. The density of the solution is 1.18 g/mL. Calculate the molarity of HCl, the molality of HCl, and the mole fraction of HCl.
- An aqueous solution of 11.6 M HCl has a density of 1.18 g/mL. What is the percent by mass of HCl in the solution?
- 1. In the laboratory, a student dilutes 16.3 mL of a 7.87 M hydrochloric acid solution to a total volume of 300.0 mL. What is the concentration of the diluted solution? 2. How many milliliters of 9.94
- What mass of HCl is contained in 30.5 mL of an aqueous HCl solution that has a density of 1.19 g/mL and is 37.21% HCl by mass? mass = ..... g
- The mass percentage of HCl within a solution is 10.00 %. Given the density of this solution is 1.049 g / mL. Find the molarity?
- How many mL of 8.12 M hydrochloric acid solution should be used to prepare 2.50 L of 0.800 M hydrochloric acid solution?
- Concentrated hydrochloric acid is 38% , by mass, HCl in water. How many grams of HCl are there in 25.0 g concentrated hydrochloric acid?
- A 8.00 M solution of hydrochloric acid is provided. You need to make 25.0 mL of a 0.490 M HCl solution. What volume, in mL, of the 8.00 M solution should you use?
- What is the molarity of 25 grams of HCl in 250 mL of solution?
- How many milliliters of 3.0 M hydrochloric acid are required to prepare 500 milliliter of 1.0 M hydrochloric solution?
- Hydrochloric acid is sold as a concentrated aqueous solution. If the molarity of commercial HCl is 12.0 and its density is 1.18 g/cm^3, calculate the mass percentage of HCl in the solution.
- Commercial grade HCl solutions are typically 39% (by mass) HCl in water. Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.
- Calculate the molarity of a solution made by adding 42.8 mL of concentrated hydrochloric acid (37.3 wt%, density 1.19 g/mL) to some water in a volumetric flask, then adding water to the mark to make e
- A 150.0 mL solution has a mass-volume percent of 6.50% calculated in units of grams per milliliter of solution. What is the mass of solute present in the solution?
- A 2.00-L bottle of solution of concentrated HCl was purchased for the general chemistry laboratory. The solution contained 868.8 grams of HCl. What is the molarity of the solution?
- How many cm3 solutions of 36% HCl with density 1.183 g/cm3 should be taken to prepare a 250 cm3 solution with a concentration of 0.215 g/dm3?
- Common commercial hydrochloric acid is an aqueous solution that is 38% HCl by mass, with a density of 1.19 g/cm3. a. Calculate the molarity of this reagent. b. Calculate the molality of this reagent. c. Calculate the mole fraction of this reagent.
- According to a label on a bottle of concentrated hydrochloric acid, the contents are 36.0% HCl by mass and have a density of 1.18 g/mL. What is the molarity of concentrated HCl. What volume of it woul
- An aqueous solution of HCl has a concentration of 0.160m and a density of 1.0691 g/mL. What is the concentration of HCl as molarity?
- An aqueous solution is 20.0 % by mass hydrochloric acid, HCl, and has a density of 1.10 g/mL. The mole fraction of hydrochloric acid in the solution is [{Blank}].
- Concentrated hydrochloric acid contains 1.00 mol HCl dissolved in 3.31 mol H_2O. a. What is the mole fraction of HCl in concentrated hydrochloric acid? b. What is the molal concentration of HCl?
- Commerical grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL. Molecular weight of Hcl is 36.46 g/mol. Molecu
- If 1 mol L of 2.0 mol L hydrochloric acid is diluted to form a solution with concentration 0.2 mol L, A. What is the final volume? B. How much water must be added to the original acid?
- If 1.5 grams of 80.0% by mass sample of potassium hydroxide is titrated with 10.0 mL of hydrochloric acid, determine the molarity of the hydrochloric acid. KOH + HCl to KCl + H_2O
- Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20 g/mL . Part A How much concentrated solution would you take to prepare 2.85 L of 0.4
- How many grams of HCl are contained in 3.00 L of the solution with a concentration of 0.0129 M HCl ?
- Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20 g/mL. How much concentrated solution would you take to prepare 3.05 L of 0.460 M HCl by mixing with water?
- Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20 g/mL. How much concentrated solution would you take to prepare 2.80 L of 0.540 M HCl by mixing with water?
- A solution is made by dissolving 3.5 grams of LiF in 3.75 liters of water at 80 degrees Celsius. Given that the density of water at this temperature is 0.9718 g/mL, find the following: a. molarity b. mass percent c. percent mass over volume (m/v%) d. dilu
- A hydrochloric acid solution, HCl, has a concentration of 12.1 M. A 41.2 mL sample is used to make a more dilute sample. If the new solution has a concentration of 0.5 M, determine the volume of the new solution.
- What is the molarity of 20 grams of HCI mixed with water to make 1 liter of the solution?
- What volume of concentrated hydrochloric acid (12.0 M HCl) is required to make 2.0 liters of a 3.0 M HCl solution?
- . A bottle of concentrated hydrochloric acid contains aqueous HCl, 36.0% by mass with a density of 1.18 g/mL. a. What is the molarity of HCl in the bottle? b. What volume of this concentrated soluti
- Concentrated HCl acid is 38% by weight of HCl and has a density of 1.19 g/mL. What is the molarity of HCl?
- Determine the amount of solute in the following solution: 1 mL of 5 M HCl (hydrochloric acid).
- A 0.1501 M solution of hydrochloric acid is used to titrate 30.02 mL of a calcium hydroxide solution to determine its concentration. If 140.21 mL of hydrochloric acid is required, what is the concentration (in molarity) of the calcium hydroxide solution?
- A 35.0 ml sample of 37% HCl solution has a density of 1.18 g/ml. The sample is diluted to a volume of 0.125 L. What is the molarity of the final solution?
- Solution prepared adding 50 mL HCl and 20 mL HNO_3 to 300 mL water. More water added until final volume is 1.00 L. Calculate [H^+], [OH^-], and pH for solution. 38 % HCl by mass and density of 1.19 g / mL. 70 % HNO_3 by mass and density of 1.42 g / mL.
- How much concentrated hydrochloric acid solution (36.0% HCl by mass, d = 1.18g/mL), in milliliters, is required to produce 11.5 L of 0.268 M HCl?
- How much concentrated hydrochloric acid solution (36.0% HCl by mass, d= 1.18g/mL), in milliliters, is required to produce 12.0 L of 0.258 M HCl?
- An aqueous solution is found to have a density of 1.04 g/mL. If the solution was prepared by dissolving 45.0 grams in enough water to make 1.00 liter of solution, what is the concentration of the solution expressed as %(w/v)?
- How many grams of HCl are in 50.0 mL of a 0.65 M HCl solution?
- How many grams of HCl are in 125 mL of a 1.7 M HCl solution?
- How many grams of CaCl2 are present in a 55.0 mL aqueous solution that has a 15.0 percent by mass concentration? Assume the density of the solution is 1.00 g/mL.
- How many grams of CaCl2 are present in a 65.0 mL aqueous solution that has a 15.0 percent by mass concentration? Assume the density of the solution is 1.00 g/mL.
- How many grams of CaCl2 are present in a 75.0 mL aqueous solution that has a 35.0 percent by mass concentration? Assume the density of the solution is 1.00 g/mL.
- How much concentrated 12 M hydrochloric acid is needed to prepare 100 mL of a 2.0 M solution?
- How much concentrated 12 M hydrochloric acid is needed to prepare 100.0 mL of a 2.0 M solution?
- What volume of 12.0 M hydrochloric acid must be used to prepare 250 mL of a 1.22 x 10-1 M solution?
- What volume of concentrated 12M hydrochloric acid (HCl) is required to make 250 ml of 1M HCl solution? Use the formula V1xC1=V2xC2 to calculate the answer.
- Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20 g/mL. Part A How much concentrated solution would you take to prepare 2.70 L of 0.43
- What is the Mass/Volume percent concentration of a solution that contains 5.02 grams of sodium chloride in 100 milliliters of solution and has a mass of 103 grams?
- The mass of a beaker is 5.333 g. After 5.00 mL of a concentrated hydrochloric acid solution is pipetted into the beaker, the combined mass of the beaker and the hydrochloric acid sample is 11.229 g. What is the measured density of the hydrochloric acid so
Explore our homework questions and answers library
Browse
by subject