Acids Lesson 12 Calculating Ka From pH. 1.The pH of 0.100 M H 2 C 2 O 4 is 1.28. Calculate the Ka for the weak acid.

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Presentation transcript:

Acids Lesson 12 Calculating Ka From pH

1.The pH of M H 2 C 2 O 4 is Calculate the Ka for the weak acid.

H 2 C 2 O 4 ⇄ H + +HC 2 O 4 - I C E

1.The pH of M H 2 C 2 O 4 is Calculate the Ka for the weak acid. H 2 C 2 O 4 ⇄ H + +HC 2 O 4 - I C E pH=1.28

1.The pH of M H 2 C 2 O 4 is Calculate the Ka for the weak acid. H 2 C 2 O 4 ⇄ H + +HC 2 O 4 - I C E pH=1.28 [H + ]=

1.The pH of M H 2 C 2 O 4 is Calculate the Ka for the weak acid. H 2 C 2 O 4 ⇄ H + +HC 2 O 4 - I C E pH=1.28 [H + ]= [H + ]= M

1.The pH of M H 2 C 2 O 4 is Calculate the Ka for the weak acid. H 2 C 2 O 4 ⇄ H + +HC 2 O 4 - I C E pH=1.28 [H + ]= [H + ]= M

1.The pH of M H 2 C 2 O 4 is Calculate the Ka for the weak acid. H 2 C 2 O 4 ⇄ H + +HC 2 O 4 - I C E pH=1.28 [H + ]= [H + ]= M

1.The pH of M H 2 C 2 O 4 is Calculate the Ka for the weak acid. H 2 C 2 O 4 ⇄ H + +HC 2 O 4 - I C E pH=1.28 [H + ]= [H + ]= M Ka=[H + ][HC 2 O 4 - ] [H 2 C 2 O 4 ]

1.The pH of M H 2 C 2 O 4 is Calculate the Ka for the weak acid. H 2 C 2 O 4 ⇄ H + +HC 2 O 4 - I C E pH=1.28 [H + ]= [H + ]= M Ka=[H + ][HC 2 O 4 - ] =( ) 2 [H 2 C 2 O 4 ]

1.The pH of M H 2 C 2 O 4 is Calculate the Ka for the weak acid. H 2 C 2 O 4 ⇄ H + +HC 2 O 4 - I C E pH=1.28 [H + ]= [H + ]= M Ka=[H + ][HC 2 O 4 - ] =( ) 2 = 5.8 x [H 2 C 2 O 4 ]

2.If the pH of 0.40 M NH 25 o C is , calculate the Kb.

NH 3 + H 2 O ⇄ NH 4 + +OH - I C E

2.If the pH of 0.40 M NH 25 o C is , calculate the Kb. NH 3 + H 2 O ⇄ NH 4 + +OH - I C E pH=11.427

2.If the pH of 0.40 M NH 25 o C is , calculate the Kb. NH 3 + H 2 O ⇄ NH 4 + +OH - I C E pH= pOH=2.573

2.If the pH of 0.40 M NH 25 o C is , calculate the Kb. NH 3 + H 2 O ⇄ NH 4 + +OH - I C E pH= pOH=2.573 [OH - ]=

2.If the pH of 0.40 M NH 25 o C is , calculate the Kb. NH 3 + H 2 O ⇄ NH 4 + +OH - I C E pH= pOH=2.573 [OH - ]= [OH - ]= M

2.If the pH of 0.40 M NH 25 o C is , calculate the Kb. NH 3 + H 2 O ⇄ NH 4 + +OH - I C E pH= pOH=2.573 [OH - ]= [H + ]= M

2.If the pH of 0.40 M NH 25 o C is , calculate the Kb. NH 3 + H 2 O ⇄ NH 4 + +OH - I C E pH= pOH=2.573 [OH - ]= [OH - ]= M

2.If the pH of 0.40 M NH 25 o C is , calculate the Kb. NH 3 + H 2 O ⇄ NH 4 + +OH - I C E pH= pOH=2.573 [OH - ]= [OH - ]= M Kb=[NH 4 + ][OH - ] [NH 3 ]

2.If the pH of 0.40 M NH 25 o C is , calculate the Kb. NH 3 + H 2 O ⇄ NH 4 + +OH - I C E pH= pOH=2.573 [OH - ]= [OH - ]= M Kb=[NH 4 + ][OH - ] =( ) 2 [NH 3 ]

2.If the pH of 0.40 M NH 25 o C is , calculate the Kb. NH 3 + H 2 O ⇄ NH 4 + +OH - I C E pH= pOH=2.573 [OH - ]= [OH - ]= M Kb=[NH 4 + ][OH - ] =( ) 2 = 1.8 x [NH 3 ]

3.The pH of a 1.0 M triprotic weak acid is Calculate the Ka and identify the acid. Ka=7.3 x Boric acid

4.The pH of 0.20 M NaCN is , calculate the Kb for CN -.

CN - + H 2 O ⇄ HCN+OH -

4.The pH of 0.20 M NaCN is , calculate the Kb for CN -. CN - + H 2 O ⇄ HCN+OH - I0.2000

4.The pH of 0.20 M NaCN is , calculate the Kb for CN -. CN - + H 2 O ⇄ HCN+OH - I C

4.The pH of 0.20 M NaCN is , calculate the Kb for CN -. CN - + H 2 O ⇄ HCN+OH - I C E

4.The pH of 0.20 M NaCN is , calculate the Kb for CN -. CN - + H 2 O ⇄ HCN+OH - I C E [OH - ] = M

4.The pH of 0.20 M NaCN is , calculate the Kb for CN -. CN - + H 2 O ⇄ HCN+OH - I C E [OH - ] = M Kb=[HCN][OH - ] = [CN - ]

4.The pH of 0.20 M NaCN is , calculate the Kb for CN -. CN - + H 2 O ⇄ HCN+OH - I C E [OH - ] = M Kb=[HCN][OH - ] =( ) 2 = 4.1 x [CN - ]

5.Calculate the pH of M H 3 BO 3 H 3 BO 3 ⇄ H + +H 2 BO 3 - I0.020 M00 CxxxCxxx E xxx 0 small ka x 2 =3.8 x x=[H + ]=2.76 x M pH=-Log[2.76 x ] pH= sig figs due to molarity and Ka

6.Calculate the pH of a solution made by mixing mL of M HCl with 100 mL of water. HCl→H + +Cl - 1(0.050 M)0.025 M0.025 M 2 pH=1.60