Question

In the Electrolytes and Nonelectrolytes lab you measured the conductance of 0.02 M solutions of KNO3,...

In the Electrolytes and Nonelectrolytes lab you measured the conductance of 0.02 M solutions of KNO3, NaCl, and NaOH. You diluted these solutions to 0.10 M and measured the conductance again. How did the conductivity change after the solution was diluted?

Homework Answers

Answer #1

are strong electrolytes. Their initial concentration was 0.02 M, The final concentration of the solutions are 0.1 M. Thus, the concentration of the electrolytes has increased.

The conductance of a solution is due to the presence of ions in the solution. The greater the number of ions, more is the conductance. As on dilution, more ions are produced, so conductance should also increase on dilution. Here, since the concentration is being increased, it's conductance decreases.

The specific conductivity falls with dilution, because, the number of current carrying particles per ml decreases with dilution or decrease in concentration. Here, since the concentration is being increased, it's conductivity increases.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Water Conductance Lab (Redone) **Known Brine Solution is (0.100 M) NaCl Part 1: Conductance of Known...
Water Conductance Lab (Redone) **Known Brine Solution is (0.100 M) NaCl Part 1: Conductance of Known Solutions Brine Solutions Conductivity Temperature (with thermometer) #1 (100 ppm) 0.01 µS 25°C #2 (500 ppm) 0.07 µS 25°C #3 (1,000 ppm) 0.14 µS 25°C #4 (5,000 ppm) 0.66 µS 25°C #5 (10,000 ppm) 1.26 µS 25°C Part 2: Conductance of Unknown Solutions (100 mL each) Unknown Brine Solutions Conductivity Temperature (with thermometer) Unknown #1 9.99 µS 25°C Unknown #2 5.08 µS 25°C Unknown...
Consider the conductances of the following 0.025 M solutions. How many strong electrolytes (SE), weak electrolytes...
Consider the conductances of the following 0.025 M solutions. How many strong electrolytes (SE), weak electrolytes (WE) and nonelectrolytes (NE) are there Conductance (mS) SE/WE/NE A 0.4 B 7.2 C 0.0 D 0.2 E 2.6 F 0.6 G 0.7
Two aqueous solutions - 0.1 M NaCl and 0.1 M KNO3 - have the same freezing...
Two aqueous solutions - 0.1 M NaCl and 0.1 M KNO3 - have the same freezing point. Explain how this observation is consistent with what is known about colligative properties.
In Lab Exercise 8 you measured the electrical resistance of a number of solutions in order...
In Lab Exercise 8 you measured the electrical resistance of a number of solutions in order to determine whether a particular substance is ionic or covalent. Suppose you measure the resistance of a solution of NaCl, and the resistance was 2600 ohms. What resistance would you expect to measure for a solution of CH3OH dissolved in water? Select one: a. 1200 ohms b. More than 10,000 ohms c. 1800 ohms d. 2600 ohms e. 2700 ohms
In a similar conductometric titration, 7.00 mL of an unknown M of NaOH was titrated with...
In a similar conductometric titration, 7.00 mL of an unknown M of NaOH was titrated with 0.115 M HCL. The equivalence point volume was 12.5 mL of HCl. [NaOH (aq) + HCl (aq) --> NaCl (aq) + H2O (l)] (b). Classify the reactants in terms of electrolytes. (c). Classify the products in terms of electrolytes. (d). As the reaction progresses, will the conductivity go up or down? (As products are made and reactants used up, will you have more or...
Please send me the correct solutions. Your lab needs a 8 liter stock solution of sodium...
Please send me the correct solutions. Your lab needs a 8 liter stock solution of sodium chloride concentrated enough to make 79 L of 189.9 mM sodium chloride (FW = 58.45). The concentration of the stock solution you need to make is ____ M. You will need to measure out ____ grams of NaCl in order to make this stock solution.
A 0.860 M solution of NaOH is used to titrate the following solutions to the equivalence...
A 0.860 M solution of NaOH is used to titrate the following solutions to the equivalence point. How many milliliters of NaOH do you need when titrating against a concentration for Acetic Acid is 0.900 M. After determining the mL of NaOH, calculate the pH for both a. and b. a. 50.0 mL of 0.0750 M HCl b. 40.0 mL of CH3COOH How many millilters of NaOH do you need when titrating aginst
In lab you are asked to titrate 50.00 mL of 1.000 M HCl with 1.000 M...
In lab you are asked to titrate 50.00 mL of 1.000 M HCl with 1.000 M NaOH. Predict what the pH will be after adding 60.00 mL of NaOH.
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you 100 mL of 6.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. You have in front of you: 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT