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Strong acid/base Titration
Weak acid/ strong base titration
pH/ pOH
Ka/ Kb
100

There is a titration of 20.00 mL of 0.500 M HCl with 0.500 M NaOH. 

What is the initial pH?

0.30

100

85.0 mL of nitrous acid (HNO2) required 60.0 mL of 0.200 M NaOH to reach the equivalence point of a titration. Ka for nitrous acid = 4.6 * 10-4. What was the concentration of the HNO2 in the starting solution?

0.141 M

100

What is the pH of a 0.050 M solution of HI

What is a pH of 1.3

100

What is pKa

What is the measure of acid strength

200

There is a titration of 20.00 mL of 0.500 M HCl with 0.500 M NaOH. 

What is the pH after the addition of 10.00 mL of 0.500 M NaOH?

0.78

200

60.0 mL of 0.200 M nitrous acid (HNO2) required 60.0 mL of 0.200 M NaOH to reach the equivalence point of a titration. Ka for nitrous acid = 4.6 * 10-4. What was the pH of the solution after the addition of 30.0 mL of NaOH?

3.34

200

What is the pOH of the solution if the [H3O] concentration is 4.2 * 10^-3 M?

What is a pOH of 11.623

200

What is pKb

What is the measure of base strength

300

60.0 mL of 0.200 M nitrous acid (HNO2) required 60.0 mL of 0.200 M NaOH to reach the equivalence point of a titration. Ka for nitrous acid = 4.6 * 10-4. What was the pH of the solution after the addition of 85.0 mL of NaOH?



12.538

300

The pOH of the solution is 4.5. Calculate the pH of the solution

What is a pH of 9.5

300

If the Ka of an acid is 1.8 * 10^-5, calculate the pKa and pKb values of the acid

What is a pKa of 4.745 and a pKb of 9.255

400

You are given 25.0 mL of 0.100 M HCHO3 to be titrated with 0.100 M NaOH. 

Ka = 1.8 * 10-4 

pKa = 3.74

OH + HCHO2 ←→ H2O + CHO2


  1. Find the equivalence point

  2. Find initial pH

1. 25 mL -> 0.025 L

2. 2.37

400

Free Points

YAY!

400

The pH of a 0.0516 M solution of nitrous acid, HNO2, is 2.34. What is the Ka?

4.05 * 10^-4

500

You are given 25.0 mL of 0.100 M HCHO3 to be titrated with 0.100 M NaOH. 

Ka = 1.8 * 10-4 

pKa = 3.74

OH + HCHO2 ←→ H2O + CHO2


Find the pH at equivalence point

8.22

500

What is the pH of a solution consisting of 0.150 M HNO2 and 0.200 M NaNO2



3.46

500

The pH of a solution of a household ammonia, a 0.950 M solution of NH3 is 11.612. What is the Kb for NH3?

1.8 * 10^-5