Use the solubility graph to answer the following question. If 45 g of potassium nitrate is placed in 100 ml of water at 40 °C, how much salt would have to be added or removed in order to saturate the solution? Solubility Curves Solubility (g/L of solvent) 10 g 15 g 25 g 30 g 20 g 1400 1300 1200 1100 1000 900 800 700 600 500 400 300 200 100 O KI -HCI SO₂ NaNO₂ -KNO₂ NHẠCH KCI -KCIO3 -NaCl NH₂ 0 10 20 30 40 50 60 70 80 90 100 Temperature (°C)

Use the solubility graph to answer the following question. If 45 g of potassium nitrate is placed in 100 ml of water at 40 °C, how much salt would have to be added or removed in order to saturate the solution? Solubility Curves Solubility (g/L of solvent) 10 g 15 g 25 g 30 g 20 g 1400 1300 1200 1100 1000 900 800 700 600 500 400 300 200 100 O KI -HCI SO₂ NaNO₂ -KNO₂ NHẠCH KCI -KCIO3 -NaCl NH₂ 0 10 20 30 40 50 60 70 80 90 100 Temperature (°C)

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 55QAP

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Similar questions

. Why does the amount of excess solid solute present in a solution not affect the amount of solute that ultimately dissolves in a given amount of solvent?
Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?
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. What is the special name given to the equilibrium constant for the dissolving of an ionic solute in water?
What kinds of solute particles are present in a solution of an ionic compound? Of a molecular compound?
Classify each of the following solutions as saturated, unsaturated, or supersaturated based on the following observations made after adding a small piece of solid solute to the solution. a. The added solute rapidly dissolves. b. The added solute falls to the bottom of the container where it remains without any decrease in size. c. The added solute falls to the bottom of the container where it decreases in size for several hours and thereafter its size remains constant. d. The added solute causes the production of a large amount of solid white crystals.
Consider a 1.50-g mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture in water, 0.500 M silver nitrate is added dropwise until precipitate formation is complete. The mass of the white precipitate formed is 0.641 g. a. Calculate the mass percent of magnesium chloride in the mixture. b. Determine the minimum volume of silver nitrate that must have been added to ensure complete formation of the precipitate.
Addition of water to concentrated sulfuric acid is dangerous because it generates enough heat to boil the water, causing it to spatter out of the container. For this reason, chemists remember to add acid to water. In a dilution experiment, we calculate the amount of the more concentrated solution that must be measured out. If we place this concentrated solution (Figure 4.7) in the volumetric flask first, then dilute with water, we violate the caution Add acid to water. Describe a safer variation on the method shown in Figure 4.7 that allows the quantitative dilution of concentrated sulfuric acid. Figure 4.7 Preparing a dilute solution from a concentrated solution. (a) Draw the concentrated solution into a pipet to a level just above the calibration mark. (b) Allow the liquid to settle down to the calibration line. Touch the tip of the pipet to the side of the container to remove any extra liquid. (c) Transfer this solution to a volumetric flask. Again touch the pipet to the wall of the flask to ensure complete transfer, but do not blow out the pipet because it is calibrated for a small amount of liquid to remain in the tip. (d) Dilute to the mark with solvent. Frequently, especially with concentrated acids, it is best to have some solvent present in the volumetric flask before you add the concentrated sample.
What happens if you add a very small amount of solid salt (NaCl) to each beaker described below? Include a statement comparing the amount of solid eventually found in the beaker with the amount you added: a a beaker containing saturated NaCl solution, b a beaker with unsaturated NaCl solution, c a beaker containing supersaturated NaCl solution. A saturated sodium chloride solution.