In the lab procedure you are told to calibrate the pH meter using (1) a solution that is pH 4 and (2) a solution that is pH 7 before you measure the pH of any of the solutions that you have made. Imagine that you skip that step, you don’t calibrate the pH meter and instead you simply plug it into the LabQuest, turn it on and measure the pH of your solutions. How would that impact the following of your pH measurements?
a. Would your pH measurements be more or less precise? Why?
b. Would they be more or less accurate? Why? We would like you to think about why you need to calibrate instruments before taking measurements.
Calibration of the instrument is one basic and very important step before any practical or research which contains any equipment
In our case this equipment is ph metre
It is very necessary to calibrate the ph meter or any instrument otherwise we can get a consistent error in the readings and this error will affect our each and every reading
Before answering the below question lets understand what is accuracy and precision
precision-
precision is in simple words reproducibility of a result.
Or in other word precision refers to how close the values are to each other. The more they are close to each other the more they will be precise
accuracy
accuracy is degree to closeness to real value or true value .
So by keeping this in mind if we dont calibrate our ph meter and start the experiment we will get a continuous error in the experiment which will affect the accuracy throughout the experiment but it won't affect the precision since even after some error if we carried out the experiment correctly the value we get should be precise
Hence
A.ph measurents will be same precise if we dont calibrate the instrument i.e. it is unaffected
B. This will be less accurate since it will deviate from true or actual value by a error that is caused by not calibrating the ph meter
I hope this helps if you have any query or want more detailed explanation feel free to ask in the comment section below.
In the lab procedure you are told to calibrate the pH meter using (1) a solution...
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...
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....
what will the ph be for solution Q??
PROCEDURE The pH meter should already be calibrated at pH 4, 7 and 10. If your pH meter appears not to be operating properly, notify your TA and they will recalibrate the meter. Please handle the pH probe carefully; the tip is made of a fragile glass membrane. Be sure to rinse the probe with DI water and blot it dry with a Kimwipe whenever it is transferred from one solution to...
Need help answering all questions. much
appreciated.
The Relative Strengths of Some Acids Results Solution pH from pH Paper pH from Indicators pH from pH Meter 2.8 14 1.99 1.4 1.4. HCL Ha POq HC2H30a Na HQ PO & AL (NO3)3 Zn(NO3)2 NH 4 NO3 1.7 1.7 4.63 2.4. 2.8 5.00 6.67 Questions 1. a. Calculate the concentration of H.O ions in the most acidic solution that you examined. Use your most precise pH measurement, 262 alculate the concentration of...
) The acidity or alkalinity of a solution is described using the pH scale. Basically, pH (which stands for "potential of hydrogen") is a measure of how many H+ ions there are in a solution. As we saw in the previous question, the more H*s there are in a solution, the more acidic it is. The formula for calculating pH is given below: In words, pH equals the negative log base ten of the hydrogen ion concentration. Solution X has...
how
would you calculate the expected pH for solution 7, 8, 9, 10, and
11? (I am confused on how you calculate the dilutions for finding
the expected pH too)
Ka= 1.4x10^-5
pKa= 4.85
Part B - The Effect of Adding Acid or Base to a Buffered Solution Solution 6 16. Prepare a buffer solution by mixing 30.0 mL of 0.10 M HOAc and 40.0 mL of 0.10 M NaOAc. Measure the pH of the resulting solution with the pH...
Procedure: Re-Write this procedure in 3rd person past tense. 1. Fill the burette with sodium hydroxide solution. 2. Using the pipette, measure 10 mL of an unknown acid solution into a clean, dry flask. Add 2-3 drops of phenolphthalein and swirl gently. 3. Place the flask on the retort base on a white paper. 4. Record the pH of the acid using an electronic pH probe before titration begins. 5. Titrate the acid solution with sodium hydroxide solution until the...
Focus on Step A5 of the procedure, where one
partner prepared their sample for visual titration by adding
approximately 100mL of water to the to
sample in the plastic cup or beaker before beginning the
titration.
Note that this step was also repeated in the potentiometric
(pH-meter) titration in Part 2 (Step A7).
In both cases, the addition of more water was an experimental
necessity, to allow the solution to be stirred easily and to ensure
that the pH probe...
You need to measure pH of a solution known to be made from a metal hydroxide, but you don't have a meter or any indicators. You do happen to have some lead (II) nitrate that is soluble, and you remember that lead (II) hydroxide is insoluble. You add some to 1 liter of your unknown solution and a precipitate forms. You add more until the precipitate stops forming and then a bit more just in case. After you filter and...