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Data/Observations: Volume of (NH4)2SO4 used: 50.0 initial pH of (NH4)2SO la-8le Equivalence vol. of NaOH: 21.00l...
Need help with 3 and 4 on calculations. some info is on top of the page...
Need help with 3 and 4 on calculations. some info is on top of
the page
Data Sheet for Lab #10 Name: Partner: Data/Observations: Volume of (NH), SO, used: Suomi initial pH of (NH4)2SO4 6.79 Equivalence vol. of NaOH: 20.00 pH at half-equivalence: 10,63 Balanced Chemical Equation: 1. Write the balanced equation for the reaction of ammonium sulfate and sodium hydroxide. (NH4)2SO4(s)? 2 N.0H(1) Nasa, () + 2NH3(-) + 2H2O 2. Write the balanced equation showing the ammonium ion acting...
How would the pH for a weak acid at the half-equivalence point and volume of NaOH...
How would the pH for a weak acid at the half-equivalence point and volume of NaOH used as the titrant to reach the equivalence point, change if the i) NaOH concentration was increased ii) Acid concentration was increased
Since you know the molarity of the NaOH titrant and the volume added to the equivalence...
Since you know the molarity of the NaOH titrant and the volume added to the equivalence point, as well as the volume of acid used (10.00 mL) and the mole:mole ratio of acid and base, determine the molarity of the known and unknown acids. (You did this calculation in a 1211L, General Chemistry I, experiment.) molarHy of NoOH-O.118 Volume odd volume used - 10 Ratio Acetic Acid Molarity 27.1 (2 pts.) Unknown Acid Molarity (2 pts.) Show calculations for the...
Equivalence Point for Titration #1: 24.96 mL Equivalence Point for Titration #2: 25.40 mL Equivalence Point...
Equivalence Point for Titration #1: 24.96
mL
Equivalence Point for Titration #2: 25.40
mL
Equivalence Point for Titration #3: 25.20
mL
Midpoint pH for Titration #3: 9.80
QUESTIONS:
4) Set up the calculation required to determine
the concentration of the NaOH solution via titration of a given
amount of KHP. Include all numbers except the given mass of
KHP.
5) Set up the calculation required to determine
the concentration of the unknown strong acid via titration with a
known volume...
STR Data Standard solution: NaOH concentration 025M volume of initial NaOH buret reading final NaOhH buret readingG TUTHL volume of NaOH used Concentration of HCI Calculations(Show all work and r...
STR Data Standard solution: NaOH concentration 025M volume of initial NaOH buret reading final NaOhH buret readingG TUTHL volume of NaOH used Concentration of HCI Calculations(Show all work and remember your units and significant figures) Determine the Molarity (concentration) of HCl using the data you collected and the titration formula. (The concentration of the NaOH used was 0.25M) Record your answer on your data form. Questions 1. State the purpose of this experiment The ouredse of thrs expetmeot bn of...
6. Using the literature accepted K value where needed, calculate the expected pH of the titra...
6. Using the literature accepted K value where needed, calculate the expected pH of the titra (a) initially, before any NaOH(aq) has been added (5 marka) ard, calculate the expected pH of the titration inixture [1,07 = 1 (7.413x10-6.0.1030 mol/l) = 8.738810-4 pH = -log 8.73880-4 = 3.058 (b) when 18.00 mL of NaOH(aq) has been added (8 marks) Chemistry 1051 Laboratory Experiment (e when 45.00 mL of NaOH(aq) has been added (3 marks) (d) at the equivalence point (5...
Titration: Acids and Bases 2. How can you determine which acid is diprotic? 3. using the...
Titration: Acids and Bases
2. How can you determine which acid is diprotic?
3. using the answers to questions one and two, which acid is
diprotic?
4. Which base has more hydroxide ions per molecule?
Acid Volume Base Base Initial Volume (mL) Base Final Volume (mL) Volume of Base Used (mL) Acid: Base Ratio Acid 1 20 mL Base 1 50 mL 34.5 15.5 4:3 Acid 2 20 mL Base 1 Acid 1 20 mL Base 2 Acid 2 20...
I’m so confused on how to do any of this. Name Date General Chemistry I Lab CHE 1211 Data: Concentration of NaOH Trial Titration (to be used as practice) Initial burete eading4.0 ml Final burette...
I’m so confused on how to do any of this.
Name Date General Chemistry I Lab CHE 1211 Data: Concentration of NaOH Trial Titration (to be used as practice) Initial burete eading4.0 ml Final burette reading 20.h m 22.om. Volume of NaOH used Repeat until 2 successful titrations are achieved. Titrations (to be used in calculations) K.Oml 0.bml 35.o mL 22.3 mL 38.5ml ↓ 30.6 mL45.0 mL 49.0 mL 35.5mL50.0 me 22.0mL H. m0 ml 1b.20 m 4.5ml Initial burette...
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...
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....
Need help with 3 and 4 on calculations. some info is on top of
the page
Data Sheet for Lab #10 Name: Partner: Data/Observations: Volume of (NH), SO, used: Suomi initial pH of (NH4)2SO4 6.79 Equivalence vol. of NaOH: 20.00 pH at half-equivalence: 10,63 Balanced Chemical Equation: 1. Write the balanced equation for the reaction of ammonium sulfate and sodium hydroxide. (NH4)2SO4(s)? 2 N.0H(1) Nasa, () + 2NH3(-) + 2H2O 2. Write the balanced equation showing the ammonium ion acting...
Since you know the molarity of the NaOH titrant and the volume added to the equivalence point, as well as the volume of acid used (10.00 mL) and the mole:mole ratio of acid and base, determine the molarity of the known and unknown acids. (You did this calculation in a 1211L, General Chemistry I, experiment.) molarHy of NoOH-O.118 Volume odd volume used - 10 Ratio Acetic Acid Molarity 27.1 (2 pts.) Unknown Acid Molarity (2 pts.) Show calculations for the...
Equivalence Point for Titration #1: 24.96
mL
Equivalence Point for Titration #2: 25.40
mL
Equivalence Point for Titration #3: 25.20
mL
Midpoint pH for Titration #3: 9.80
QUESTIONS:
4) Set up the calculation required to determine
the concentration of the NaOH solution via titration of a given
amount of KHP. Include all numbers except the given mass of
KHP.
5) Set up the calculation required to determine
the concentration of the unknown strong acid via titration with a
known volume...
STR Data Standard solution: NaOH concentration 025M volume of initial NaOH buret reading final NaOhH buret readingG TUTHL volume of NaOH used Concentration of HCI Calculations(Show all work and remember your units and significant figures) Determine the Molarity (concentration) of HCl using the data you collected and the titration formula. (The concentration of the NaOH used was 0.25M) Record your answer on your data form. Questions 1. State the purpose of this experiment The ouredse of thrs expetmeot bn of...
6. Using the literature accepted K value where needed, calculate the expected pH of the titra (a) initially, before any NaOH(aq) has been added (5 marka) ard, calculate the expected pH of the titration inixture [1,07 = 1 (7.413x10-6.0.1030 mol/l) = 8.738810-4 pH = -log 8.73880-4 = 3.058 (b) when 18.00 mL of NaOH(aq) has been added (8 marks) Chemistry 1051 Laboratory Experiment (e when 45.00 mL of NaOH(aq) has been added (3 marks) (d) at the equivalence point (5...
Titration: Acids and Bases
2. How can you determine which acid is diprotic?
3. using the answers to questions one and two, which acid is
diprotic?
4. Which base has more hydroxide ions per molecule?
Acid Volume Base Base Initial Volume (mL) Base Final Volume (mL) Volume of Base Used (mL) Acid: Base Ratio Acid 1 20 mL Base 1 50 mL 34.5 15.5 4:3 Acid 2 20 mL Base 1 Acid 1 20 mL Base 2 Acid 2 20...
I’m so confused on how to do any of this.
Name Date General Chemistry I Lab CHE 1211 Data: Concentration of NaOH Trial Titration (to be used as practice) Initial burete eading4.0 ml Final burette reading 20.h m 22.om. Volume of NaOH used Repeat until 2 successful titrations are achieved. Titrations (to be used in calculations) K.Oml 0.bml 35.o mL 22.3 mL 38.5ml ↓ 30.6 mL45.0 mL 49.0 mL 35.5mL50.0 me 22.0mL H. m0 ml 1b.20 m 4.5ml Initial burette...
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....
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