Without doing detailed calculations, and assuming that the volumes of the solution and water are additive, what happens to the final solution obtained as a result of evaporating 500.0 mL water from 2500.0 mL of 0.800 M sucrose. increase in moles O increase in concentration O decrease in moles O decrease in concentration

Without doing detailed calculations, and assuming that the volumes of the solution and water are additive, what happens to the final solution obtained as a result of evaporating 500.0 mL water from 2500.0 mL of 0.800 M sucrose. increase in moles O increase in concentration O decrease in moles O decrease in concentration

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

1. Determine the molarity of a NaOH solution if 0.8427 g of KHP: 15.57 mL of NaOH. are required to standardize
Consider the solubilities of a particular solute at two different temperatures. Temperature (°C) Solubility (g/100 g H,O) 20.0 45.9 30.0 68.7 Suppose a saturated solution of this solute was made using 70.0 g H,0 at 20.0 °C. How much more solute can be added if the temperature is increased to 30.0 °C? mass: g
A 52.0 mL aliquot of a 1.30 M solution is diluted to a total volume of 218 mL. A 109 mL portion of that solution is diluted by adding 161, mL of water. What is the final concentration? Assume the, volumes are additive. concentration:
Which of the following could cause errors in measurement of the percent chloride? Group of answer choices A. Hydrated precipitate and heat B. Incomplete precipitation and hydrated precipitate C.Light exposure D. Hydrated precipitate and light exposure E. Incomplete precipitation and heat F. Hydrated precipitate G. Incomplete precipitation H. Incomplete precipitation and light exposure I. Heat and light exposure J . Heat
A solution is made by dissolving 3.56 mol of sodium chloride in 250. mL of distilled water. The amount concentration of the solution is A) 0.0142 mol/L. B) 70.2 mol/L. O C) 0.0702 mol/L. D) 14.2 mol/L.
Aa.91.
If 0.0578 mol CaCl, is dissolved in water to make a 0.780 M solution, what is the volume of the solution? mL V =
Solid aluminum nitrate is slowly added to 150 mL of a 0.0699 M potassium hydroxide solution. The concentration of aluminum ion required to just initiate precipitation is M.the expert working on my last question, doesnt have to anymore, its been answered thanks.
To determine the concentration of a NaOH (39.997 g/mol) solution, 1.42 g of C8H5KO4 (a commonly used standard, 204.22 g/mol) was used. The volume of NaOH solution needed to reach the endpoint was 33.54 mL. What was the concentration (in molarity) of the NaOH solution? The mole:mole ratio for NaOH and KHP neutralization is 1:1. Report your answer to the thousandths place and do not include units.
Please see attached photo and answer question in photo, for #41. Thanks!
A student is preparing 0.5 L of a 0.1 M magnesium chloride solution. The student uses the following steps to get started. Step 1: Gather a graduated cylinder, balance, and stirring rod. Step 2: Calculate the number of moles of magnesium chloride needed. Step 3: Add enough water to reach the 0.5 L mark of magnesium chloride solution and stir until dissolved. Step 4: Label the solution 0.1 M MgCl2. The process as described is incomplete. What would fix the process so that it is accurate? A The student made a mistake in Step 1 by getting a graduated cylinder. The student should have gotten a beaker. B The student made a mistake in Step 2 by only calculating the moles of magnesium chloride. The grams should also be calculated to make the solution. C The student made a mistake in Step 3 by adding enough water to reach 0.5 L mark of solution. Exactly 0.5 L of water should have been added. D The student make…
: What is the molarity and normality of a solution which is prepared by dissolving 75.0 g of Ba(OH)2 in water and diluting it to 0.500 L. The molar mass of Ba(OH)2 is 171 g/mol.