Electrolytes 5 of 9 If a solute produces ions when dissolved, it is called an electrolyte because the resulting ions in solution will allow the solution to conduct electricity. A solute that completely dissociates into ions is a stronger electrolyte than one that only partially dissociates into ions. If a solute remains as a molecule when dissolved, it is called a nonelectrolyte.In this tutorial, you will practice identifying substances as strong electrolytes, weak electrolytes, or nonelectrolytes. Part A Each of the following reactions shows a solute dissolved in water. Classify each solute as a strong electrolyte, a weak electrolyte, or a nonelectrolyte. 1. X(s)–→X(aq) 2. CD(aq) =C* (aq) + D (aq) 3. YZ(s)>Y*(aq) +Z (aq) 4. PQ(aq)P' (aq) + Q (aq) 5. R(i)R(aq) Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help xCD]Yz]PaR Strong electrolyte Weak electrolyte Nonelectrolyte Submit

Electrolytes 5 of 9 If a solute produces ions when dissolved, it is called an electrolyte because the resulting ions in solution will allow the solution to conduct electricity. A solute that completely dissociates into ions is a stronger electrolyte than one that only partially dissociates into ions. If a solute remains as a molecule when dissolved, it is called a nonelectrolyte.In this tutorial, you will practice identifying substances as strong electrolytes, weak electrolytes, or nonelectrolytes. Part A Each of the following reactions shows a solute dissolved in water. Classify each solute as a strong electrolyte, a weak electrolyte, or a nonelectrolyte. 1. X(s)–→X(aq) 2. CD(aq) =C* (aq) + D (aq) 3. YZ(s)>Y*(aq) +Z (aq) 4. PQ(aq)P' (aq) + Q (aq) 5. R(i)R(aq) Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help xCD]Yz]PaR Strong electrolyte Weak electrolyte Nonelectrolyte Submit

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...

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Imagine a small amount of each compound in the table below is dissolved in water. Pick the sketch that best shows what the solution would look like, at the atomic level. The large number of faint red and white molecules in the background of each sketch represent the water solvent. Also, the colors of the solute atoms may not mean the same element in each sketch. For example, solute oxygen atoms could be colored yellow in the first sketch but blue in the second. Chlorine atoms could be colored blue in the first sketch but yellow in the second. And so on. Note for advanced students: the sizes of the atoms and any bond angles may not be accurate.
3. Write the balanced complete molecular, complete ionic and net ionic chemical equations including phase labels for the neutralization of solid potassium hydroxide with aqueous sulfuric acid. Include phase labels.
The solution was prepared by adding 150 g of sodium hydroxide to 150 g of water, giving a total weight of 300 g. Density of the solution is 1.53 g/mL What is the molarity of the solution? 2. Pause the Student Protocol video at 1 minute 39 seconds. Now use your molarity in the dilution equation to calculate the number of mL you will need to dilute to make 500 mL of a 0.10 M sodium hydroxide solution.
Suppose a mixture is made by mixing together 10 drops of a water solution of a halogen, 10 drops of a water solution of the potassium salt of the halogen and 10 drops of hexane. Upon shaking, the hexane layer takes on a distinct purple color. Which of the following pairs could not represent the halogen and halogen salt that were mixed? a) I2, KI b) Cl2, KI c) Cl2, KBr d) I2, KCl
A chemist starts with 25.0 mL of a 0.20 M NaCl solution and dilutes it to 500 mL. What is the concentration of NaCl in the new solution? 0.060 M 0.080 M 0.020 M 0.040 M What is the molarity of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL? 0.267 M 6.67 M 0.150 M 0.200 M Consider the following sample data or measurement. 167, 180, 188, 177, 181, 185, 189 Is 167 an outlier at 90% confidence interval?
Magnesium oxide is sometimes used as an antacid to help with indigestion and stomach upset caused by excess stomach acid (hydrochloric acid). Write two balanced chemical equations to explain how this works. One should be a synthesis and the other a neutralization.
Write ONLY the balanced "NET" ionic equations for each of the reactions. If no net, write NR. barium chloride + silver nitrate barium chloride + lead(II) nitrate barium chloride + copper(II) sulfate barium chloride + calcium nitrate barium chloride + barium chloride potassium bromide + silver nitrate potassium bromide + lead(II) nitrate potassium bromide + copper(II) sulfate potassium bromide + calcium nitrate potassium bromide + barium chloride Magnesium sulfate + silver nitrate Magnesium sulfate + lead(II) nitrate Magnesium sulfate + copper(II) sulfate Magnesium sulfate + calcium nitrate Magnesium sulfate + barium chloride sodium carbonate + silver nitrate sodium carbonate + lead(II) nitrate sodium carbonate + copper(II) sulfate sodium carbonate + calcium nitrate sodium carbonate + barium chloride sodium chromate + silver nitrate sodium chromate + lead(II) sulfate sodium chromate + copper(II) sulfate sodium chromate + calcium nitrate sodium chromate + barium…
Imagine a small amount of each compound in the table below is dissolved in water. Pick the sketch that best shows what the solution would look like, at the atomic level. The large number of faint red and white molecules in the background of each sketch represent the water solvent. Also, the colors of the solute atoms may not mean the same element in each sketch. For example, solute oxygen atoms could be colored yellow in the first sketch but blue in the second. Chlorine atoms could be colored blue in the first sketch but yellow in the second. And so on. Note for advanced students: the sizes of the atoms and any bond angles may not be accurate. pick a sketch compound NaNO, OCI₂ Submit (Drag the slider to choose an image) (Drag the slider to choose an image)
7. Classify each as a soluble ionic compound (SI), insoluble ionic compound (II), strong acid (SA), weak acid (WA), strong base (SB), or molecular non-acid/non-base (M). Then assign each as a Strong, Weak, or Nonelectrolyte: Mg(OH)2 HI NaNO3 HCIO4 СоBr, PbBr2 Cal2 HF H;SO3 NHẠNO3 II N
If 23.1 g of NaOH (MM = 40.00 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of NaOH in the resulting solution? What quantity in moles of NaI are in 55.8 grams of NaI ?
CHAPTER 8 - SOLUTIONS Previous Page 18 of 35 Next O If 8.50 g Ca(NO3)2 is dissolved in enough water to make 0.750 L of solution, what is the molar concentration of Ca(NO3)2?
Imagine a small amount of each compound in the table below is dissolved in water. Pick the sketch that best shows what the solution would look like, at the atomic level. The large number of faint red and white molecules in the background of each sketch represent the water solvent. Also, the colors of the solute atoms may not mean the same element in each sketch. For example, solute oxygen atoms could be colored yellow in the first sketch but blue in the second. Chlorine atoms could be colored blue in the first sketch but yellow in the second. And so on. Note for advanced students: the sizes of the atoms and any bond angles may not be accurate. compound BaCl, CO pick a sketch (Drag the slider to choose an image) (Drag the slider to choose an image) X $ Education All Rights Reserved of the 1 Privacy