A sample of mineral water contains 5.24 * 10^-2 of NaCl in 2.88 L. If the density of the water is 1.00 g/mL, how many ppm of NaCl is this equal to?

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A sample of mineral water contains 5.24 * 10^-2 of NaCl in 2.88 L. If the...
A 1.00 L sample of water contains 0.0048 g of SH ions. Determine the concentration (in ppm) of SH ions? The density of the solution is 1.00 g/mL. and What is the weight percent of a caffeine solution prepared by dissolving 6.35 g of caffeine, C8H10N4O2, in 75.0 g of benzene, C6H6?
please help ASAP water has fluoride ion added in many parts of U.S.A water sample contains 0.70 ppm F- a. what mass of F- is contained in one liter of this water? density is 1.00 g/mL b. what mass of CaF2 will result if all the water is evaporated from a 1.0 L sample of 0.70 ppm fluoridated water?
An aqueous NaCl solution contains 1.343x10* ppm NaCl. The density of water is 1.000g/ml. The density of the solution is 1.08 g/mL. The molar mass of NaCl is 58.44g/mol. Keep the correct number of significant figures. a) What is the molality of NaCl? b) What is the molarity of NaCl? c) What is the (mass/volume)% is unit of (kg/L)%? d) What is mass percent? e) What is mole fraction of NaCl?
Hard water normally contains mineral ions, such as Ca2+ and Mg2+ ions, from minerals that dissolved in the ground water. For water of low hardness, the concentration of Ca2+ ions is usually expressed as ppm CaCO3 in the water sample. Parts per million (ppm) is defined as one part of solute mass per 1,000,000 parts of solution mass, as shown in the following equation. Please note, the unit of denominator and numerator needs to be the same. Since ppm expresses...
Question 1. A 2.700×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.3 mL . The density of water at 20.0∘C is 0.9982 g/mL. a.)Calculate the molality of the salt solution. B.) Calculate the mole fraction of salt in this solution. C.) Calculate the concentration of...
A 2.400×10−2 M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.4 mL . The density of water at 20.0∘C is 0.9982 g/mL. a. Calculate the molality of the salt solution. b. Calculate the mole fraction of salt in this solution. c. Calculate the concentration of...
A 2.300×10−2 M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.4 mL . The density of water at 20.0∘C is 0.9982 g/mL. Express your answer(s) to four significant figures and include the appropriate units. Part A) Calculate the molality of the salt solution. Part B)...
PEIT A What mass of salt (NaCl) should you add to 1.90 L of water in an ice cream maker to make a solution that freezes at-11.4 C ? Assume complete dissociation of the NaCl and density of 1.00 g/mL for water. VAE ? m(NaCl) Request Answer Submit
PEIT A What mass of salt (NaCl) should you add to 1.90 L of water in an ice cream maker to make a solution that freezes at-11.4 C ? Assume complete dissociation...
Please I need help with number 54 and 61 please
An aqueous NaCl solution is made using 112 g of NaCl diluted to a total solution volume of 1.00 L. Calculate the molarity, molality, and mass percent of the solution. (Assume a density of 1 08 g/mL for the solution.) An aqueous KNO_3 solution is made using 72.5 g of KNO_3 diluted to a total solution volume of 2.00 L. Calculate the molarity, molality, and mass percent of the solution....
Water in a jar contains 250. ppm lead. How many grams of lead will be taken by a person who drinks 200. mL of water from the jar? Assume density of water to be 1.00 g/mL.