The purpose of the lab was to find the equilibrium constant of the rxn of acetic acid and ethanol to yield ethyl acetate and water. Hydrochloric acid is used as a catalyst. We have to determine the equilibrium concentrations of all the species (water included) present at equilibrium. In test tubes, different concentrations of the equilibrium system were prepared then titrated with NaOH to determine the total acid content of the system at equilibrium. From this you will be able to determine the concentration of all species at equilibrium and the equilibrium constant.
To determine the total concentration of acid at equilibrium, which is equal to the concentration of HCl and acetic acid. First of all you need to determine the concentration of the catalyst HCl, that is present at equilibrium. The first table is data from the titration of 5.00mL and 6 M HCl by NaOH. I'm lost on how to find the number of moles of HCl. I used the C1*V1=C2*V2, to find the molarity of NaOH, and dimensional analysis to find the moles of HCl but I don't think I did it right.
The second table is the titration of a soultion by NaOH. The contents of the solution were 5.00mL 6M HCl, 2.00mL ethanol, and 3.00mL of glacical acetic acid. I'm lost on how to find the molarity of NaOH, the moles of NaOH, the moles of acid at equivalence point, and average moles of acetic acid at equilibrium.
Please help me with this. :)
The purpose of the lab was to find the equilibrium constant of the rxn of acetic...
I'm having trouble with the calculations for my chemistry lab: Determination of an Acid Dissociation Constant, Ka Half-Neutralization Molarity of acetic acid: 2 M Molarity of NaOH: 1 M Volume of acetic acid: 25 mL NaOH Solution Final Buret Reading: 6.23 mL Initial Buret Reading: 0.01 mL Volume added: 6.22 mL Total Volume of Solution: 250 mL pH: 3.85 Caculating Ka Initial number of moles HAn: ? OH-: ? Number of moles at equilibrium: HAn: ? An-: ? Equilibrium concentrations,...
I'm doing a titration lab tomorrow and I am not sure what the
formulas are to calculate the moles of NaOH, the moles of
HCl, and the molarity of HCl.
The objective of this laboratory is to determine the molarity of
a hydrochloric acid solution using a known concentration of sodium
hydroxide as the titrant.
volume of HCl in flask: 25.00 mL
the net ionic equation for the reaction is:
H+(aq) + OH-(aq) --> H2O(l)
I don't have the data...
I'm not sure about how I'm supposed to find NaOH
concentration from a strong acid and strong base titration. I'm
thinking that 2.5×10^-8 mol per L that I calculated would make the
moles of NaOH 2.5x10^-8 mol since it's a one to one
ratio.
Hydrochloric acid titration: Confirming the concentration of NaOH Concentration of HCl solution from the stock bottle: _ 0.OSM! Initial pH of HCl solution: 1.66 pH Volume NaOH (mL) Concentration of NaOH (M) Non Phenolphthalein (end point)...
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...
Lab Report: Titration of Vinegar Experimental Data Trial 1 Trial 2 Initial Buret Reading Trial 3 OML OML OML Final Buret Reading 40 6 ML 40-3 ML 41-7 ML Volume of NaOH used 40.0ML 4 7 40.3 ML Molarity of NaOH used Volume of vinegar used 5ML SML 5ML Data Analysis 1. Write the balanced equation for the neutralization reaction between aqueous sodium hydroxide and acetic acid. The Molarity of Acetic Acid in Vinegar Trial 1 Trial 2 Trial 3...
How do I calculate the ionization
constant for acetic acid from the measured pH of the acedic acid
samples?
Data and Calculations 1. Measurement of pH and fitration of acetfic acid solution Concentration of standardized NaOH titrant Mass concentration of acetic acid-aao Trial 3 Trial 2 Trial 1 Measured pht of the acetic acid solution Mass of acetic acid solution taken for titration. Initial buret reading of NaOH titrant Final buret reading of NaOH titrant Net volume of NaOH Millimoles...
moles of oxalix acid
moles/molarity of NaOH
average molarity
volume/molarity of hcl used
average molarity
NAME SECTION DATA SHEET LOCKER A CTOR Write a balanced equation for the reaction between H.CO. and NaOH: 90.33/mol 0.878 0836 TRIAL NUMBER a. Mass of oxalic acid used (g) b. Final Buret reading (ml.] c. Initial Buret reading (ml] d. Volume of NaOH used (b-c) Moles of oxalic acid used f. Moles of NaOH used (2 xe) g. Molarity of NaOH (f/d/1000) Average Molarity...
The table filled is the lab run.
Please can you use the three informations provided above to answer
the empty table
Take Density of vinegar = 1.005g/mol
concentration of NaOH = 0.1205M
Experiment #7. Titration of Vinegar Goals 1. To determine the mass percent of acetic acid in a solution via titration. 2. To master the technique of titration. Introduction Vinegar is a common household item that is found in a number of products from salad dressing to cleaners. Vinegar...
A student is trying to determine the concentration of an acetic acid (HC2H302) solution. They place 5.00 mL of it in a flask and titrate it with a 0.150 M NaOH solution. At the endpoint of the titration, they find that they have used 19.27 mL of the NaOH solution. Based on this information answer the following questions. a) How many moles of NaOH are used to reach the endpoint? moles NaOH b) How many moles of acetic acid were...
Experiment Lab Team Members Finding Equilibrium Constants: The Solubility of Borax Report Sheet Part A: Titration of Room Temperature Borax: K Molarity of Standard HCl solution: 004 u Temperature of room temperature borate mixture (T): T, in 20.0c T, in к Trial Trial 2 Trial 3 if donel Final buret reading HCI, ml. Initial buret reading HCl, mL Volume of HCl used in Titration, ml. Moles HCI Moles Borate Molarity of Borate Molarity of Na Average of Borax: Part B:...