Which of the following are errors that can occur when measuring
the pH with a glass combination electrode?
Homework Answers
Glass combination electrodes have higher sensitivity for H+ over other ions
The internal AgAgCl reference electrode will have a fixed potential
Therefore, the errors are possible due to
Uncertainty in the pH of the standard buffers used to calibrate the instrument
Sodium error at high pH
Junction potential
Add Answer to:
Which of the following are errors that can occur when measuring
the pH with a glass...
The alkaline error observed when the pH of alkaline solutions is measured occurs because: A. alkaline...
The alkaline error observed when the pH of alkaline solutions is measured occurs because: A. alkaline solutions can damage the glass electrode. B. the membrane of the glass electrode can respond to other cations besides H+. C. not enough time was allowed for the electrode to equilibrate with the solution. D. the glass electrode was saturated with H+ cations. E. the junction potential increases the uncertainty.
Which of the following are NOT potential error sources associated with pH measurement using a glass...
Which of the following are NOT potential error sources associated with pH measurement using a glass electrode? Heavy metal ions Junction potential Alkaline error Acid error
This is from a Study of Buffer Solutions and pH of Salt Solutions Lab. I calculated...
This is from a Study of Buffer Solutions and pH of Salt
Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value
larger than the standard value?
Procedure:
10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
I know some of the measured pH values are a little off due to error in...
I
know some of the measured pH values are a little off due to error
in the lab, but I need help filling out the “Ion Hydrolyzed” table
and then the “Net Ionic Equation” part. I remember doing net ionic
equations in General Chemistry I, bit don’t see how it applies
here.
Thanks, in advance! (i will rate!)
Learning Objectives: 1. To test the acidic and basic properties of ionic compounds. 2. To create a buffer solution and calculate its...
In the lab, a student determines the density of a metal object by measuring its mass...
In the lab, a student determines the density of a metal object by measuring its mass on a balance and its volume by displacement in a graduated cylinder. The data collected by the student is shown. mass of object: 44.701 g volume of water in cylinder before object submersed: 29.47 ml volume of water + object in cylinder: 35.33 mL Calculate the density of the object. d= g/mL Based on the recorded volume data, and assuming that the student used...
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Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and...
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and react with water to produce hydronium ions or hydroxide ions that contribute to the pH of the salt solution. Since strong acids and strong bases completely ionize in solution, the reverse reaction essentially does not occur, meaning that the resulting conjugate base of a strong acid or conjugate acid of a strong base do NOT act as acids or bases. Ions that are conjugate...
I need help with the problem in the last photo.. I thought I’d post my lab...
I need help with the problem in the last photo.. I thought I’d
post my lab explanation and data if that helps you get a better
understanding, but it’s just the question at the end. I know I need
to use the Henderson Hasselbach equation.. so... 4.70 = pKa + log(
[acetate-ion] / [acetic-ion] ) and solve for pKa, then Ka.. but how
do I find the concentrations to put in the log fraction?
Thanks, in advance!
Learning Objectives: 1....
is a solution that resists changes in pH when a small amount of acid or base...
is a solution that resists changes in pH when a small amount of acid or base is added to best buffer solutions are prepared from weak acids and their conjugate base added as a sodium of potassium salt. Most biological systems must maintain a very narrow range of pH; therefore, buffers allow the biological solution to function correctly. Blood is a good example of a biological system that must maintain a pH in a very narrow range from 7.3 to...
There are some issues that will be occur when applied ICS related to Auditor: The management may over rely on the strength of the ICS and therefore relax their supervision which may leave room for err...
There are some issues that will be occur when applied ICS related to Auditor: The management may over rely on the strength of the ICS and therefore relax their supervision which may leave room for errors and frauds thus exposing the auditor to potential civil liabilities. ICS may reduce the auditor’s vigilance and observations with an unfavorable effect on the quality of the audit. ICS may be abused by the internal auditors through collusion with the management and this may...
The alkaline error observed when the pH of alkaline solutions is measured occurs because: A. alkaline solutions can damage the glass electrode. B. the membrane of the glass electrode can respond to other cations besides H+. C. not enough time was allowed for the electrode to equilibrate with the solution. D. the glass electrode was saturated with H+ cations. E. the junction potential increases the uncertainty.
This is from a Study of Buffer Solutions and pH of Salt
Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value
larger than the standard value?
Procedure:
10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
I
know some of the measured pH values are a little off due to error
in the lab, but I need help filling out the “Ion Hydrolyzed” table
and then the “Net Ionic Equation” part. I remember doing net ionic
equations in General Chemistry I, bit don’t see how it applies
here.
Thanks, in advance! (i will rate!)
Learning Objectives: 1. To test the acidic and basic properties of ionic compounds. 2. To create a buffer solution and calculate its...
In the lab, a student determines the density of a metal object by measuring its mass on a balance and its volume by displacement in a graduated cylinder. The data collected by the student is shown. mass of object: 44.701 g volume of water in cylinder before object submersed: 29.47 ml volume of water + object in cylinder: 35.33 mL Calculate the density of the object. d= g/mL Based on the recorded volume data, and assuming that the student used...
Video Assessment Questions 1. What possible errors can occur at Norchem Drug Testing? 2. Which type of error is of greater concern to Norchem Drug Testing? 3. Norchem Drug Testing tries to ensure that the probability of a false positive is near zero. What type of probability is this? In the context of hypothesis testing, what would we call this probability? 4. Give a scenario other than drug testing that is designed to keep the probability of making a Type...
I need help with the problem in the last photo.. I thought I’d
post my lab explanation and data if that helps you get a better
understanding, but it’s just the question at the end. I know I need
to use the Henderson Hasselbach equation.. so... 4.70 = pKa + log(
[acetate-ion] / [acetic-ion] ) and solve for pKa, then Ka.. but how
do I find the concentrations to put in the log fraction?
Thanks, in advance!
Learning Objectives: 1....
is a solution that resists changes in pH when a small amount of acid or base is added to best buffer solutions are prepared from weak acids and their conjugate base added as a sodium of potassium salt. Most biological systems must maintain a very narrow range of pH; therefore, buffers allow the biological solution to function correctly. Blood is a good example of a biological system that must maintain a pH in a very narrow range from 7.3 to...
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