Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![The scale used for measuring the acidity or basicity of a solution is known as the pH scale. Typically you will see values ranging from 0 to 14, however it is possible to produce highly acidic solutions with a lower pH or a highly basic solution with a
higher pH. A neutral solution has an equivalent concentration of hydronium and hydroxide ions, which has a pH of 7 at 25 °C. A pH less than 7 indicates that a solution is an acid, and a pH greater than / Indicates that a solution is a base.
Click on the image below to explore this simulation, which demonstrates the pH scale. The pH of the solution is related to the H₂O¹ ion concentration by the equation
pH = -log H₂O¹]
When you click the simulation link, you may be asked whether to run, open, or save the file. Choose to run or open it
Part D
A
PHET=
In this simulation, allowing you to produce solutions at at 25°C, you should see three modes: Macro, Micro, and Custom. In Macro and Micro, you are provided with a calibrated beaker along with an inlet and an outlet tap. You can choose different
solutions from the dropdown list above the beaker in the simulation in Macro mode, the pII scale displayed on the left side of the beaker indicates the pII of the solution. In Micro mode, the graphic to the left gives the concentration, or number of
moles, of H₂O¹, OH, and H₂O.
Express your answer numerically to two decimal places.
▸ View Available Hint(s)
POH
Show Transcribed Text
■V
pH
5.80
In the simulation, open the Custom made. The beaker will be filled to the 0.50 L mark with a neutral solution. Set the pH to 3.15 by using the green arrows adjacent to the pH value indicated on the probe in the solution. Once you adjust the pH
note the corresponding OH ion concentration in Mas given in the graphic on the left side of the simulation. Make sure to select the option "Concentration (mol/L) above the graphic. Select on the Logarithmic scale below the graphic.
Find the pOH of the solution.
| ΑΣΦ +
C
L-4054L
?
G
Ć](https://content.bartleby.com/qna-images/question/781810ad-2ef2-46a9-ab70-3ca45e7bfd53/49ecfa56-52fb-4ccc-bc3f-077139dd9229/1pmeln7_processed.jpeg)
Transcribed Image Text:The scale used for measuring the acidity or basicity of a solution is known as the pH scale. Typically you will see values ranging from 0 to 14, however it is possible to produce highly acidic solutions with a lower pH or a highly basic solution with a
higher pH. A neutral solution has an equivalent concentration of hydronium and hydroxide ions, which has a pH of 7 at 25 °C. A pH less than 7 indicates that a solution is an acid, and a pH greater than / Indicates that a solution is a base.
Click on the image below to explore this simulation, which demonstrates the pH scale. The pH of the solution is related to the H₂O¹ ion concentration by the equation
pH = -log H₂O¹]
When you click the simulation link, you may be asked whether to run, open, or save the file. Choose to run or open it
Part D
A
PHET=
In this simulation, allowing you to produce solutions at at 25°C, you should see three modes: Macro, Micro, and Custom. In Macro and Micro, you are provided with a calibrated beaker along with an inlet and an outlet tap. You can choose different
solutions from the dropdown list above the beaker in the simulation in Macro mode, the pII scale displayed on the left side of the beaker indicates the pII of the solution. In Micro mode, the graphic to the left gives the concentration, or number of
moles, of H₂O¹, OH, and H₂O.
Express your answer numerically to two decimal places.
▸ View Available Hint(s)
POH
Show Transcribed Text
■V
pH
5.80
In the simulation, open the Custom made. The beaker will be filled to the 0.50 L mark with a neutral solution. Set the pH to 3.15 by using the green arrows adjacent to the pH value indicated on the probe in the solution. Once you adjust the pH
note the corresponding OH ion concentration in Mas given in the graphic on the left side of the simulation. Make sure to select the option "Concentration (mol/L) above the graphic. Select on the Logarithmic scale below the graphic.
Find the pOH of the solution.
| ΑΣΦ +
C
L-4054L
?
G
Ć
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- Chemistry of Solütions 202-NYB-05 2. Pre-lab question: Calculate the.volume of NaOH 0.50 M needed to obtain a 1:1 acid:acetate ratio from 50 mL of acetic acid 0.20 M. Note that you need to neutralize only half of the acetic acid.arrow_forwardNonearrow_forwardWrite the Henderson-Hasselbalch equation for a propanoic acid solution (CH₂CH₂CO₂H, pKa [HA] pH = = 4.352 || pH = 4.874 Answer Bank [A] + log Using the equation to calculate the quotient [A¯]/[HA] at three different pH values. [A-] [HA] [A-] [HA] - o = pka pH = 4.874).arrow_forward
- Please don't provide handwritten solution ....arrow_forwardClick on the My Solution section and explore the simulation to familiarize yourself with the controls. Then, reset the experiment by clicking the orange button with the circular arrow before continuing. 1. Adjust the H30* slider until the pH reaches 2.00. Record the [H30*] and [OH] for the solution in Table 5. 2. Calculate the pOH for the solution, and enter it into Table 5. 3. Repeat for pHs of 5.00, 7.00, 9.00, and 12.00. Table 5. Concentrations of hydronium ion, hydroxide ion, and pOH at various pH values. Table view List view [H30*] (M) [OH¯] (M) pOH pH 2.00 pH 5.00 pH 7.00 pH 9.00 pH 12.00arrow_forwardUsing the graph, identify the half way and equivalence point. Base: NaOH Acid: unknown 11arrow_forward
- Please do it neat and clean correctly please... Posting third time please help me with correct solution pleasearrow_forward1. The [H30"], in M, of 10.00 mL of 0.100 M NAOH after adding 10.00 mL of indicator solution. To enter exponential values, use the format 1.0e-5. Answer: 2. The [H30"], in M, of 10.00 mL of 0.100 M HCl after adding 10.00 mL of the indicator solution. To enter exponential values, use the format 1.0e-5. Answer:arrow_forwardClassify the solutions as acidic or basic. Drag the appropriate items to their respective bins. Reset Help [OH-] =1.9 × 10–9 M [OH-] = 2.9 x 10-2 M [OH-] = 6.5 x 1o-12 M| %3D Acidic solution Basic solutionarrow_forward
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