15. Calculate the equivalence point volume for titration of 39.5 mL of 0.15 M HCIO4 with...
Calculate the equivalence point volume for titration of 38.5 mL of 0.17M HClO4 with a sample of 0.35M NaOH.
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...
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)
In a titration of 20 mL of 0.20 M HX with a NaOH solution the equivalence point volume of base is 30 mL. If the PH is 3.74 @ 15 mL of base what is the pH @ 10 mL of added base?
52. Consider the titration of 20.0 ml of 0.45 M HOCI (Ka = 1.3x10-5) with 0.15 M Ca(OH)2. a. What is the volume of 0.15 M Ca(OH)2 required to reach the equivalence point. b. What is the pH of the solution at the point which is half-way to the equivalence point? c . C. What is the pH of the solution after addition of a total of 20.0 ml of 0.15 M Ca(OH)2? d. What is the pH of the...
Calculate the pH at the equivalence volume for the titration of 25.0 mL of 0.350 M acetic acid with 0.350 M sodium hydroxide. The K a for acetic acid is 1.8 * 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.
What is the equivalence volume for a titration of 13.6 mL of 1.59 M monoprotic acid (HA) with 9.51 M NaOH? (Answer in units of mL, but do not write mL in the box)
Acid-Base Titration: A 0.15 M solution of NaOH is used to titrate 200.0 mL of 0.15 M HCN. What is the pH at the equivalence point? Ka = 4.9 x 10-10. Please include steps/work so I can see and understand how this problem is solved.
Find the pH of the equivalence point and the volume (mL) of 0.0346 M KOH needed to reach the equivalence point in the titration of 23.4 mL of 0.0390 M HNO2. Find the pH of the two equivalence points and the volume (mL) of 0.0652 M KOH needed to reach them in the titration of 17.3 mL of 0.130 M H2CO3.