Titration Basics
What is the purpose of a titration experiment?
To determine the concentration of an unknown solution
What equipment is used to hold the titrant?
buret
What does the sharp increase in pH indicate on a titration curve?
equivalence point
What is the formula used to find the molarity of the analyte?
#H+ MaVa = MbVb #OH-
Why does the titrant needs to be slowly added?
to prevent overshoot
What term describes the point at which moles of acid equal moles of base?
An erlenmeyer flask is commonly used to hold what?
analyte
What is the pH of the equivalence point of a strong acid and strong base titration?
7
f 25.0 mL of 0.100 M NaOH is required to neutralize 50.0 mL of HCl, what is the molarity of HCl?
0.05 M
What equation is to be used at the half-equivalence point?
Henderson Hasselbalch Equation
What is the name of the solution with known concentration in a titration?
titrant
A student swirls after adding few drops of titrant. The color change does not disappear. What is happening?
Full equivalence / end point.
half-equivalence point
A 25.0 mL sample of monoprotic acid requires 32.0 mL of 0.100 M NaOH to reach equivalence. What is the molarity of the acid?
0.128 M
A titration starts at pH of 1 and ending at a pH of 9, what is the titrant?
weak base
How many equivalence points does H2SO4 have if a titration is performed?
2
A titration ended up being a vibrant pink color. what did the student end up doing?
overshooting
what is the pH of the equivalence point where strong acid is added to weak base during titration?
<7
It takes 20 mL of a 0.30 M HCl solution to neutralize 300 mL of NaOH solution. What is the concentration of the NaOH solution?
0.021M
Why are indicators used?
To mark the end/equivalence point
How will polyprotic acids affect titration?
overestimation.
Why does the pH change very slowly at the half equivalence point?
After reaching full equivalence point during a strong acid-strong base titration, the student adds another 20 mL of 0.1M NaOH. What will be the new pH of the solution?
12.2