Homework Answers
(1) May be pH meter sensor is not working properly. It needs to be properly clean. Any chemical deposition on the sensor may change the readings.
(2) Glass vials might not be cleaned properly. Before you, somebody might have handled acids in it.
(3) Water is contaminated. Most of the groundwater is acidic. Water might not properly be distilled or deionised.
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we did a lab where we measured the pH of different diluted solutions of HCL and...
We did a lab in which we discovered how increasing the length of a nichrome wire...
We did a lab in which we discovered how increasing the length of a nichrome wire affects the amount of current and found that there was an inverse relationship. We used an ammeter, one battery, and measured varied lengths of nichrome wire from 5-100 cm. What are some possible sources of random or systemic experimental error in this experiment?
IV. Comparing Buffering Capacity A. pH of Pure Water i. Measure out 30.0 mL DI H2O...
IV. Comparing Buffering Capacity A. pH of Pure Water i. Measure out 30.0 mL DI H2O into a beaker. 1. Calculate the expected pH of pure water. pH ________ 2. Measured pH of pure water. pH ___3.88______ 3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error? % error __________ B. pH of Water and Strong Acid i. Measure out 30.0 mL DI H2O and 2.0...
Experiment VII: Buffers Lab Report ( 49 pts) I. Determination of the K, of acetic acid...
Experiment VII: Buffers Lab Report ( 49 pts) I. Determination of the K, of acetic acid 1. Measured pH of the solution PH 2.40 < Calculate the [H3O*) at equilibrium for this solution. (include units) Tog [HT] = 10-2.40 H 0% 0.004 m. 3. Calculate the [CH,C00] at equilibrium for this solution. (include units) [CH.CO01 0.004 m 4. What is the [CH3COOH) at equilibrium for this solution? (include units) 700. [CH.COOH): 0.00lem 5. Based on these values, what the acid...
unknown solutions A and B are 0.1 M solutions of either HCI or NaOH. According to your pH measurement, which is which...
unknown solutions A and B are 0.1 M solutions of
either HCI or NaOH. According to your pH measurement, which is
which
10% Bleach Question: 1. Unknown solutions A and B are 0.1 M solutions of either HCl or NaOH. According to your pH measurements, which is which? 1 2. The pH of pure water is 7. Comment on how closely your measured pH values from each measurement method compared to the expected value. Which method was more appropriate for...
1) Find the Difference between measured pH and calculated theoretical pH of solutions 1-6 for [HC2H3O2]...
1) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6 for
[HC2H3O2] (M) and
[C2H3O2−] (M)
2) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6.
3) In this experiment, we define the buffer capacity of a buffer
as the number of drops of either 3.0 M HCl or 3.0 M NaOH needed
before the pH of the solution changes by more than 0.5 pH units.
For example, if the pH of...
REPOSTING: observing pH changes in Water and Buffer solutions. the amount added of HCl and NaOH...
REPOSTING: observing pH changes in Water and Buffer
solutions.
the amount added of HCl and NaOH are both 25mL.
the buffer solution is made of 2grams of NaC2H3O2 and
4 mL of 6M HC2H3O2 in a 50 mL solution (46mL of water). the
solution will contain 2.4x10^-2 mol each of NaC2H3O2 a d
HC2H3O2.
question:
how to answer it (I'm not sure I'm doing it right and
want an expert to double check):
I need help calculating the theoretical and...
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 this experiment you will be measuring pH for several different solutions. A pH probe will...
In this experiment you will be measuring pH for several
different solutions. A pH probe will be used rather than pH paper
as it will be more accurate.
You will be testing the pH of six solutions: deionized water,
0.1 M HCl, 0.1 M HCH3COO, 0.1 M NaCH3COO, 0.1
M NaOH, and a buffer made by mixing equal parts of
HCH3COO and NaCH3COO.
You will measure the pH of each solution three times:
Neat - just the solution
After the...
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....
Properties of Buffers Lab. I need help with problems 7 & 8. They’re pretty similar, but...
Properties of Buffers Lab.
I need help with problems 7 & 8. They’re pretty similar,
but I’m confused on whether I’m doing them right.
I need to calculate the moles of HCl and NaOH and then somehow
insert them into the log fraction in the Henderson Hasselbach
formula, is that right?
Procedure (values are needed in procedure):
Measured values during lab that I’ll be comparing #6/7/8
to:
Questions I need help with:
Part B Procedures: 1. Weigh about 3.5g of...
Experiment VII: Buffers Lab Report ( 49 pts) I. Determination of the K, of acetic acid 1. Measured pH of the solution PH 2.40 < Calculate the [H3O*) at equilibrium for this solution. (include units) Tog [HT] = 10-2.40 H 0% 0.004 m. 3. Calculate the [CH,C00] at equilibrium for this solution. (include units) [CH.CO01 0.004 m 4. What is the [CH3COOH) at equilibrium for this solution? (include units) 700. [CH.COOH): 0.00lem 5. Based on these values, what the acid...
unknown solutions A and B are 0.1 M solutions of
either HCI or NaOH. According to your pH measurement, which is
which
10% Bleach Question: 1. Unknown solutions A and B are 0.1 M solutions of either HCl or NaOH. According to your pH measurements, which is which? 1 2. The pH of pure water is 7. Comment on how closely your measured pH values from each measurement method compared to the expected value. Which method was more appropriate for...
1) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6 for
[HC2H3O2] (M) and
[C2H3O2−] (M)
2) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6.
3) In this experiment, we define the buffer capacity of a buffer
as the number of drops of either 3.0 M HCl or 3.0 M NaOH needed
before the pH of the solution changes by more than 0.5 pH units.
For example, if the pH of...
REPOSTING: observing pH changes in Water and Buffer
solutions.
the amount added of HCl and NaOH are both 25mL.
the buffer solution is made of 2grams of NaC2H3O2 and
4 mL of 6M HC2H3O2 in a 50 mL solution (46mL of water). the
solution will contain 2.4x10^-2 mol each of NaC2H3O2 a d
HC2H3O2.
question:
how to answer it (I'm not sure I'm doing it right and
want an expert to double check):
I need help calculating the theoretical and...
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 this experiment you will be measuring pH for several
different solutions. A pH probe will be used rather than pH paper
as it will be more accurate.
You will be testing the pH of six solutions: deionized water,
0.1 M HCl, 0.1 M HCH3COO, 0.1 M NaCH3COO, 0.1
M NaOH, and a buffer made by mixing equal parts of
HCH3COO and NaCH3COO.
You will measure the pH of each solution three times:
Neat - just the solution
After the...
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....
Properties of Buffers Lab.
I need help with problems 7 & 8. They’re pretty similar,
but I’m confused on whether I’m doing them right.
I need to calculate the moles of HCl and NaOH and then somehow
insert them into the log fraction in the Henderson Hasselbach
formula, is that right?
Procedure (values are needed in procedure):
Measured values during lab that I’ll be comparing #6/7/8
to:
Questions I need help with:
Part B Procedures: 1. Weigh about 3.5g of...
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