a) According to the statement you started with an initial volume of 15 ml and a final reading 32 ml so:
32 - 15 = 17 ml of NaOH used or 0.017 L
we know that the concentration of the acetic acid is 0.5 M, you can calculate the number of moles of NaOH
Molarity = moles / volume
moles = molarity * volume
moles of NaOH = 0.5 * 0.017 = 0.0085 moles of NaOH used
b)according to the reaction
NaOH + CH3COOH == CH3COONa + H2O, we require 1 mole of NaOH to neutralize 1 mole of CH3COOH so
we have 0.0085 moles of acetic acid in the solution
the concentration in the acetic acid solution 25 ml will be
volume = 0.025 L
Molarity = moles of acetic acid / volume = 0.0085 moles / 0.025 L = 0.34 M of acetic acid
c) phenolphtalein is an indicator that will turn pink under basic conditions, it will become colorless under acidic conditions.
When exposed to the environment your solution will get some CO2 diluted (coming from air), the reaction will be like:
CO2 + H2O === H2CO3 , this will dissociate like
H2CO3 === H+ + HCO3
The protons will neutralize the OH- ions coming from the NaOH, this will create a slightly acid condition.
In the titration below acetic acid (CH CooH)i (a) What is the volume of NaOH used to neutralize t...
A titration of 25.00 mL of an acetic acid solution with 0.1220 M NaOH solution starts at a burette reading for NaOH of 0.17 mL. The phenolphthalein indicator turns light pink in the acid solution for over 30 seconds at a burette reading of 36.32 mL. The volume of NaOH used to neutralize the acid is _______ mL.
What information then do you need? This is Chem 2 and not Org Chem. Titration of Vinegar Lab Report 1 /25 pts) Name: Part 1: Data and Calculations mass KHC.H.O. - 4.0744 g Molecular Weight potassium hydrogen phthalate KHC.H. - [1 pt) #moles KHP = [0.5 pts) Volume of solution = 250 ml_ L10.5 pts] Concentration of KHP = Mop = _M (1 pt) Volume of KHP Solution to be titrated mL = [1 pt) #mols of KHP to be...
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...
how to find volume of NaOH, molar concentration of NaOH, and molar concentration of acid soultion? (14pts) Part A. Standardization of a Sodium Hydroxide Solution Table view Table 4. Calculations for standardization of sodium hyroxide List view Trial 1 Trial 2 Trial 3 [1] Tared mass of KHCH04 (9) 0.333 0.320 0.383 [2] Burette reading of NaOH, initial (mL) (3) Burette reading of NaOH, final (mL) 3.79 4.97 3.58 19.17 20.04 21.97 [4] Volume of NaOH, dispensed (mL) 15.38 15.07...
Trial 1 Acetic acid / L solution 2.402g/L Volume of acetic acid (mL) 30 mL Initial buret volume (mL) 0.2 mL Final buret volume at end point (mL) 18.2 mL Total volume of NaOH titrated (mol) 18.0 mL Moles of NaOH titrated (mol) Molarity of acetic acid (mol/L) Molar mass of acetic acid Average volume of NaOH titrated mL Average molar concentration of acid Average molar mass of acetic acid
45 THE TITRATION OF VIR EXPERIMENT 8 REPORT SHEET Name Section Date Attach your completed Post-Lab Questions to this Report Sheet to hand in next week. INTRODUCTION By titrating vinegar with a standardized solution of sodium hydroxide, the experimental % acetic acid in the vinegar was determined and compared to the manufacturer's reported value. DATA 5% acetic acid on vinegar Trial 1 Trial 2 Trial 3 Volume of Vinegar Used (mL) Mass S Vinegar Reported on Bottle Concentration of NaOH...
millimoles of NaOH titrant Chemical Equilibria: K, of a Weak Monoprotic Acid Report Form Name: Partner's Name: (if any) Lab Section MWITTHM-TH (Circle) Data and Calculations 1. Measurement of pH and titration of acetic acid solution Concentration of standardized NaOH titrant 0.1054 Mass concentration of acetic acid 2.40 - mol/L Trial 3 Measured pH of the acetic acid solution Mass of acetic acid solution taken for titration Trial 1 3.09 20.16 0 11.4 Trial 2 3.32 30.06 Initial buret reading...
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...
n titration of 50.00(±0.01) mL an acetic acid solution with a 0.1000 (±0.0004) molar NaOH solution (as the titrant), the initial and final (end point) buret readings are as follows: Initial buret reading: 0.07 (±0.01) mL Final buret reading: 5.72 (±0.01) mL Calculate the concentration of acetic acid and the percent relative uncertainty related to it. Report ONLY the percent relative uncertainty in the provided box with correct number of significant figures.
Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC8H404, MW = 204.23 g/mol. Acetic acid, HC2H302, MW = 60.05 g/mol Part 1: Standardization of NaOH Assume 0.951 g of KHP is weighed and transferred to a 250 mL Erlenmeyer flask. Approximately 50 ml water is added to dissolve the KHP. Note that the exact volume of water is not important because you only need to know the exact number of moles of KHP that will react with...