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Titration
Terms
Calculations
Buffers
Indicators
100

Equipment used to add the titrant in slow increments

Burette

100

This is an acid that does not fully dissociate.

What is a weak acid?

100

pH of a 0.01M HCl solution

2

100
This is what a buffer is made of.
What is a weak acid/base and its conjugate?
100
The purpose of indicators.
What is to determine when pH passes a given point?
200

The equivalence point.

What is The point in a titration at which the reaction between titrant and unknown has just been completed.

200

What is a BL Base?

A substance that receives a proton

200

pH of a 0.01M NaOH

12

200
You would add this to a solution of ammonia to make it a buffer.
What is ammonium?
200

Do all indicators produce the same color change?

No

300
This is titrated to a weak acid to give an equivalance point pH greater than 7.
What is a strong base?
300

Solutions that resist changes in pH when a strong acid or base is added

Buffer solution

300

pH of 0.005M HF Ka = 1.43x10-5

3.57

300
This base would be used to form a buffer with HBr.
What is What is Br-?
300

Do all indicators change color at the same pH?

No

400
This amount of 5M HCl is needed to fully titrate 1.000L of 1M NaOH.
What is 200ml?
400

This term that is used to describe a substance that is able to donate a hydrogen cation.

What is a Bronsted-Lowry acid?

400

pH of 0.005M NH3 Kb = 1.43x10-5

10.43

400
This is the pH of 50.00 mL buffer solution which is 2.00M in HCl2H3O2 and 2M in NaC2H3O2. Ka of acetic acid=1.8x10-5.
What is What is 4.74? pH = -log(1.85×10-5) + log(2.00 / 2.00) pH = -log(1.85×10-5) + 0 pH = 4.74
400

When did the lab indicator turn pink

When pH got above 7

500
Titration reveals that 12.5mL of 3.0M HCl is required to neutralize a 25.0mL solution of NaOH showing this is the molarity of the NaOH solution.
What is 1.5M
500
This is the difference between amphiprotic and ampiteric.
What is amphiprotic can donate and accept a proton while ampiteric can act either as a base or an acid?
500

Name this equation: pH=pKa + log([base]/[acid])

Henderson Hasselbach

500
This is the pH for a solution of 1 mol ammonium and 1 mol ammonia when 36.5g of HCl is added . Ka of ammonium=5.9x10-10
What is What is 4.61? 5.9×10-10 = x2/1 [H+] = 2.4x10-5 pH = -log(2.4×10-5) pH = 4.61
500

Indicator used in the lab experiment

Phenolphtalein