Pure water has a density of 1.00 g/ml at 297 K. Calculate the molar concentration of pure water...
Question:
Pure water has a density of {eq}1.00\ g/ml {/eq} at {eq}297\ K {/eq}. Calculate the molar concentration of pure water at this temperature.
Molar Concentration:
Molar concentration is defined as the no. of moles of solute in 1 litre of the solution. Here, there is no soute, only water. So, it is solute as well as solvent. Thus volume of water is taken as volume of the solution.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerVolume of solution=1 L
Volume of water =1L.
Mass of water =1000 gm ...................................................(Given:mass of 1ml water...
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
Molarity vs Molality | Comparison, Formula & Examples
from
Chapter 8 / Lesson 5
32K
What is molarity? What is molality? Compare molarity vs molality by viewing molality and molarity formulas, how to calculate molarity and molality, and examples.
Related to this Question
- Pure water has approximately what molar concentration?
- What is the molar concentration of B in water given that the mass of B in a 100 cm3 is 2.11g, a molar mass of 234.01 g/mol^-1 and a density of 1.01g/cm^-3 when mixed with water?
- Pure water is approximately what molar concentration? a) 0.55 Molar b) 5.5 Molar c) 55 Molar d) 550 Molar
- What is the molar volume of pure water at 22 degrees Celsius?
- Calculate the mole fraction of solute when 355 g of CO2 is in 0.409 L of water (density of water is 1.00 g/mL).
- The solubility of MgCl2 at 25 degrees C is approximately 8.0 g MgCl2/100 g water. Assuming the solution has a density of 1.00 g/cm3, calculate the concentration of MgCl2 in a saturated solution in moles/liter and then calculate Ksp for MgCl2.
- Calculate the concentration, % m/m, of a solution containing 26.0 g solute and 726.0 g water.
- Calculate the freezing point of a water solution at a 1.45 m concentration.
- Calculate the freezing point of a water solution at a 2.5 m concentration.
- Calculate the freezing point of a water solution at a 0.85 m concentration.
- Calculate the freezing point of each water solution at each concentration. (a) -0.80 M (b) -1.50 M (c) -4.6 M (d) -2.15 M
- Calculate the freezing point of a water solution at a 4.8 m concentration.
- Calculate the concentration (% m/m) of a solution containing 26.0 grams of solute and 726.0 grams of water.
- You make a solution using a solute (5g) in water (total volume 100ml). The molar mass of the solute is 110 g/mol. What is the molarity? What is the concentration reported as % by mass?
- The density of a 23.0% by mass ethylene glycol solution in water is 1.04 g/mL. Find the molarity of the solution.
- Find the temperature at which the molarity of pure water is equal to its molality.
- What is the molarity of a solution is dissolved in 81.5 g of ethylene glycol in 1.36 L of water density of water is 1.00 g/mL?
- What is the molarity of NaCl when 100g of this compound is dissolved in 500mL of water such that the density of the final solution is 1.16g/mL?Assume the density of pure water is 1g/ml.
- At 25 degrees C, the density of a 60.0% (m/m) solution of sucrose, C_{12}H_{22}O_{11}, in water is 1.29 g/mL. What is the molarity of this solution?
- What is the molal (m) concentration of a 0.115 M solution of KCl (MW= 74.55 g/mol) whose density is 0.94 g/mL?
- Calculate the freezing point of a solution that contains 8.90 g of KBr in 115 mL of water.
- Calculate the freezing point of a solution that contains 2.06 g of KBr in 188 mL of water.
- Calculate the molality of a solution of 50 mL of ethanol, C2H5OH (density = 0.789 g/mL), which is dissolved in 0.25 L of water (density = 1.00 g/mL).
- Find the boiling point of 0.250 M glucose in water (assume the density of water is 1.00 g/mL).
- An aqueous solution is 0.387 M in HCl. If the density of the solution is 1.23 g/mL, what is the concentration expressed in molality?
- Calculate the molarity and molality of an NH3 solution made up of 30.0 g of NH3 in 70.0 g of water. The density of the solution is 0.982 g/mL.
- A solution of H2SO4(aq) with a molal concentration of 1.94 m has a density of 1.119 g/mL. Calculate the molar concentration of this solution.
- Calculate the molarity of a solution that consists of 25.0 grams of NH3 in 75.0 grams of water. The density of the solution is 0.952 g/mL.
- Determine the molality and molarity of a solution prepared by dissolving 75.0 g of Ba(NO3)2(s) into 374.00 g of water at 250 degrees Celsius. (water density = 0.99707 g/mL3)
- The density of water is about 1.0 g/mL at room temperature. Briefly explain how the density of an aqueous solution at room temperature can be significantly less than 1.0 g/mL. Give an example of such a solution.
- What is the ppm of NaCl when 100g of this compound is dissolved in 500mL of water such that the density of the final solution is 1.16g/mL?Assume the density of pure water is 1g/ml.
- You are asked to calibrate a 25.00-mL volumetric pipet. You determine the temperature of your distilled water is exactly 20.0 degrees Celsius. You carefully determine the mass of a clean, dry beaker and find it is 60.0826 grams. You pull water up to the m
- A solution containing 121.8g of Zn(NO3)2 per liter has a density of 1.107 g/mL. Calculate its molal concentration.
- The density of a 22.0 % by mass ethylene glycol (C_2H_6O_2) solution in water is 1.03 g / ml . (a) Find the molarity of the solution.
- Calculate the freezing point of an aqueous solution formed by dissolving 4.22 g of KCl in 25.00 mL of water. The Kf for water is -1.86 C/m. Assume the density of water is 1 g/mL.
- If 45.8 grams of MgO are dissolved in 205 grams of water, what is the concentration of the solution in percent by mass?
- The density of a 20.0% by mass ethylene glycol (C_2H_6O_2) solutionin water is 1.03 g/mL. Find the molarity of the solution.
- Calculate the concentration of the solution in mass percent: 32.3 mg KNO3 in 2.44 g of H2O.
- Calculate the concentration of the solution in a mass percent: 122 g KCl in 628 g H_2O.
- The density at 20 degrees Celsius of a 0.258 m solution of glucose in water is 1.0173 g/ml, and the molar mass of glucose is 180.2 g/mol. What is the molarity of the solution?
- At 25 C, the lowest conductivity observed for distilled water (density = 0.997 g/ml) is 58 10 9 S/cm. This conductivity must be attributed to the equilibrium concentration of H + and O H . Determine the degree of dissociation, , and the d
- Calculate the theoretical boiling point of a solution prepared by dissolving 50.0 g of MgCl2 in 500 mL of water.
- You dissolved 450.0 g of sugar (C12H22O11) in 150 mL of water. The density of water is 1.00 g/mL. a. Calculate the molarity of the solution. b. Calculate the molality of the solution.
- If (MM + 180.2) grams of a substance is dissolved in 500 mL of water, what is the molality of the resulting solution? Assume the density of water is 1 g/mL.
- Calculate the concentration, in percent by mass, of a refrigerant brine solution which is 4.03 M in NaCl with a density of 1.116 g mL-1.
- The density at 20 degrees C of a 0.258 m solution of glucose in water is 1.0173 g/mL, and the molar mass of glucose is 180.2 g/mol. What is the molarity of the solution?
- Calculate the freezing point and boiling point: An ethylene glycol solution contains 20.2 g of ethylene glycol (C_2H_6O_2) in 86.4 mL of water. (Assume a density of 1.00 g/mL for water.)
- 3) You are asked to calibrate a 25.00 mL volumetric pipet. You determine that the temperature of your distilled water is 24.5 degrees Celsius. You carefully determined the mass of a clean dry beaker a
- A solution is prepared by adding 1.43 moles of KCI to 889 grams of water. What is the molal concentration of KCI?
- You are given the temperature of Y which is 20 degrees Celsius, the temp of water which is 40 degrees celsius. There is 100 mL of compound Y poured into a flask containing 50 mL of water. Assume that compound Y has a density of 1.62 g/mL. The solution's f
- A solution is made by dissolving 96.2 g of HI in 3.75 liters of water at 90^\circ C. Given that the density of water at this temperature is 0.9585 \dfrac{g}{ml}, find the following: a) Molarity b) Molality
- If 12.20 grams of RbCl are dissolved in water to make a solution of 0.223 L, the density is found to be 1.040 g/cm^3. Calculate the molality of the solute.
- Calculate the molality of a solution formed by dissolving 34.8 g of LiI in 500.0 mL of water.
- Calculate the molarity and molality of a solution of 50 grams of ethanol, C2H5OH (density = 0.789 g/mL) which is dissolved in 200 mL of water (density = 1.00 g/mL). Show your complete solution.
- Calculate the molality and molarity of HCl for a solution of 75.2 g of HCl in 140.0 g of water if the density = 1.009 g/mL.
- How to calculate grams of solute in a given volume of solution using the percent concentration?
- Which is the mass of the solute in 400 grams of 20% solution? What is the concentration of this solution knowing that its density is 1.2 g/mL?
- Calculate the boiling point of a solution containing 312g ethylene glycol (C_2H_6O_2) dissolved in 1.75 L of water. Assume a density of 1.00 g/mL for water.
- An ethylene glycol solution is mad using 58.5 g of (C_2H_6O_2) and diluting to a total volume of 500.0 mL. Calculate the freezing and boiling point. Assume a density of 1.09 g / ml for the solution.
- Calculate the boiling point of a solution that contains 8.90 g of KBr in 115 mL of water.
- Calculate the molality of a solution prepared by dissolving 4.75 g of C10H8 in 75.0 mL of C6H6(l) of density 0.879 g/mL.
- Calculate the molality of a solution prepared by dissolving 4.75 g of C_{10}H_8 (s) in 75.0 mL of C_6H_6(l) of density, 0.879 g/mL.
- What is the freezing point of a solution that contains 20.5 g of CO (NH_2)_2 in 260 ml water, H_2O? Assume a density of water of 1.00 \dfrac{g}{mL}.
- Can one calculate solution density from the solute mass and solvent volume?
- What is the freezing point of a solution that contains 23.9 grams of urea in 295 mL of water? Assume a density of water of 1.00 g/mL.
- A 9.50% by mass solution of acetone in water has a density of 0.9849 g/mL at 20 degrees Celsius. What is the molarity of this solution?
- A solution is made by dissolving 97.5 g of HI in 3.75 liters of water at 90 degrees C. Given that the density of water at this temperature is 0.9715 g/ml, find the molarity and molality.
- A sample of seawater has a density of 1.02 kg/L and has the following ion in parts per million by mass, 19,000 Cl^-. how do you find the molar concentration
- What is the freezing point of a solution that contains 21.1 g of urea, CO(NH_2)_2, in 305 mL water, H_2O? Assume a density of water of 1.00 g/mL.
- What is the freezing point of a solution that contains 23.8 g of urea, CO(NH2)2, in 205 mL water, H2O? Assume a density of water of 1.00 g/mL.
- What is the freezing point of a solution that contains 28.9 g of urea, CO(NH2)2, in 295 mL of water, H2O? Assume a density of water of 1.00 g/mL.
- An aqueous solution of Kl has a freezing point of -1.80 degrees C and anosmatic pressure of 26.0 atm at 25.0 degrees C. Assume Kl completely dissociates in water. What is the density of the solution?
- What is the freezing point of a solution that contains 20.2 g of urea CO(NH_2)_2 in 295 mL water? (Assume a density of water of 1.00 g/mL)
- Calculate the molality of a solution formed by adding 2.435 g of methanol (CH3OH) to 100.00 mL of water. The density of water is 0.9982 g/mL.
- If 14.40 grams of RbCl are dissolved in water to make a solution of 0.224 L, the density is found to be 1.047 g/cm3. Calculate the molality of the solute.
- Suppose 115 g of KCl is dissolved in 750 mL of water (density = 1.005 g/mL). What would be the freezing point and boiling point of that solution, assuming the Kf of water is 1.86 C/m and Kb is 0.512 C/m? (Assume that KCl fully dissociates with no pairing
- Calculate the volume (mL) of the solute (CH3)2CO and the volume (L) of the solvent H2O that should be added to prepare 1.36 kg of a solution that is 25.7 g (CH3)2CO per 100 g solution. Given: For Acetone ((CH3)2CO): Molar Mass (g/mol) = 58.05, Density (g
- What is the molality of NaCl when 100g of this compound is dissolved in 500mL of water such that the density of the final solution is 1.16g/mL?Assume the density of pure water is 1g/ml.
- Calculate the freezing point of a solution containing 24.5 grams of CuCl2 in 480 grams of water. (Kf for water = 1.86 C/m)
- A solution is prepared by mixing 5.00 grams of compound Z (molar mass 15.00 g/mol) in 100.0 mL of water. The density of the solution is 1.09 g/mL. Calculate the molarity of the solution.
- Any dilute aqueous solution has a density near 1.00 g/mL. Suppose the solution contains 1 ppm of solute; express the concentration of solute in g/L, mug/L, mug/mL, and mg/L.
- Any dilute aqueous solution has a density near 1.00 g/mL. Suppose the solution contains 2.2 ppm of solute; express the concentration of solute in g/L, ?g/L, ?g/mL, and mg/L.
- Calculate the mass percent of a NaCl solution in which 158 g of NaCl is dissolved in 3.81 L of water at 25 degrees C (density = 0.997 g/mL).
- Assuming that seawater is an aqueous solution of NaCl, what is its molarity? The density of seawater is 1.025 g/mL at 20 degrees Celsius, and the NaCl concentration is 3.50 mass %.
- A 100 g sample of NaCl is dissolved in water to give a final volume of 700mL. The density of the solution at 22 Celsius was determined to be 1.10 g/mL a) Calculate the molarity b) Calculate the mola
- A 4.305 g sample of a nonelectrolyte is dissolved in 105 g of water. The solution freezes at -1.23 degrees C. Calculate the molar mass of the solute. K_f for water = 1.86 C/m.
- Express the concentration of a 0.0260 M aqueous solution of fluoride, F^-, in mass percentage. Assume the density of the solution is 1.00 g/mL. T
- Calculate the solubility of 43g of NaCl containing 100ml of water at temperature of 20^oC.
- Calculate the mass of solute that must be dissolved in 50.00 mL of deionized water to prepare each of the solutions listed (0.5 m methanol, 0.5 m NaCl, 0.5 m CaCl_2).
- If 32.3 g of KCl are dissolved in 192 g of water, what is the concentration of the solution in percent by mass? A. 5.94% KCl B. 8.55% KCl C. 14.4% KCl D. 16.8% KCl
- A solution containing 80.5 grams of C6H8O6 dissolved in 210 grams of water has a density of 1.22 g/mL at 55 degrees Celsius. Express the concentration of C6H8O6 in each of the following: a. mass percentage b. mole fraction c. molality d. molarity
- A 95.0 wt% solution of ethanol, C2H5OH, in water has a density of 0.804 g/mL. Find the mass of 1.00 L of this solution and the number of grams of ethanol per liter. What is the molar concentration of ethanol in this solution?
- Calculate the mass of solute present in 21.7 mL of 0.0125 M \rm KBrO_3
- Given that 1.0 L of water has a mass of 1.0 kg, what is the molarity of pure water to 2 significant figures?
- A solution of 16.1 grams of an unknown solute in 600 mL of water boils at 100.28 ^\circ C. What is the molar mass of the solute?
- Calculate the final concentration if 2.0 L of 0.53 M NaO, 1.4 L of 0.15 M NaCl, and 0.6 L of water are mixed.
- A 15.00 % by mass solution of lactose (C_{12}H_{22}O_{11}, 342.30 g/mol) in water has a density of 1.0602 g/ml at 20 degree C. What is the molarity of this solution? a. 0.03097 m b. 0.4133 m c. 0.4646 m d. 1.590 m e. 3.097 m
- What is the freezing point of a solution that contains 23.0g of urea in 275mL water. Assume a density of water of 1.00 g/mL
- Calculate the mass percent of ethylene glycol (C2H6O2) in a 1.50 M aqueous solution. The density of the solution at 20.0 degrees Celsius is 1.0116 g/mL.
- Calculate the molality of a solution formed by dissolving 42.3 g of LiBr (MW = 86.8 g/mol) in 650.0 mL of water and 25 degrees C (Density of water 0.997 kg/L). A. 0.065 m. B. 0.752 m. C. 0.013 m. D. 3.20 m. E. 0.015 m.
Explore our homework questions and answers library
Browse
by subject