Calculate the equivalence point volume for titration of 38.5 mL of 0.17M HClO4 with a sample...
15. Calculate the equivalence point volume for titration of 39.5 mL of 0.15 M HCIO4 with a sample of 0.35 M NaOH. ml
A 23.00 ?mL sample of an unknown HClO4 solution requires titration with 20.12 mL of 0.2000 M NaOH to reach the equivalence point. The neutralization reaction is: HClO4(aq)+NaOH(aq)?H2O(l)+NaClO4(aq) What is the concentration of the unknown HClO4 solution? express your answer using four Sig figs.
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...
Determine the volume in mL of 0.45 M HClO4(aq) needed to reach the half-equivalence (stoichiometric) point in the titration of 35.2 mL of 0.31 M CH3CH2NH2(aq). Enter your answer with one decimal place. The Kb of ethylamine is 6.5 x 10-4.
Determine the pH during the titration of 22.7 mL of 0.134 M HClO4
by 0.134 M NaOH at the following points
Determine the pH during the titration of 22.7 mL of 0.134 M HCIO, by 0.134 M NaOH at the following points: (a) Before the addition of any NaOH (b) After the addition of 11.4 mL of NaOH (c) At the equivalence point (d) After adding 28.6 mL of NaOH
A Weak Acid - Strong Base Titration Report Sheet Date: Name: Volume of CH3COOH (ml): Sample Code: { 10.00 mL Temperature: _22.0_ Initial Volume of NaOH (mL): 0.00 Molarity of NaOH (from label): _0.1013__ RUN 1 From LabQuest Titration Curve From 1st Derivative From Printed Titration Curve Instructor's Approval of LabQuest Data Volume of NaOH at Equivalence Pt (mL) 12.00mL 12.65mL Average Volume of NaOH at Equivalence Pt Include printed graphs of titration curve and 1st Derivation with Report Sheet...
What is the pH at the equivalence point in the titration of a
29.4 mL sample of a 0.403 M aqueous acetic acid solution with a
0.386 M aqueous sodium hydroxide solution?
What is the pH at the equivalence point in the titration of a 29.4 mL sample of a 0.403 M aqueous acetic acid solution with a 0.386 M aqueous sodium hydroxide solution?
Find the pH of the equivalence point and the volume (mL) of 0.0372 M NaOH needed to reach the equivalence point in the titration of 42.2 mL of 0.0520 M CH3COOH. (K_a of CH_3COOH = 1.8 times 10^-5)
Calculate the hypothetical pH AT THE EQUIVALENCE POINT for the titration of 50.00 mL of 0.0800 M Formic Acid (HCOOH, Ka=1.80x104) with 0.1000M NAOH at 25°C.
Calculate the pH at the equivalence point for the titration of 1.0 M ethylamine, C2H5NH2, by 1.0 M perchloric acid, HClO4. (pKb for C2H5NH2 = 3.25)