Question

Calculate pH Using Kw= 1.00X 10^-14 of 0.010 M HCl

Calculate pH Using Ka = 1.75 x 10^-5 of 0.010 M HC₂H₃O₂

Calculate pH 0.0010 M NaOH

Calculate pH Using Kb= 1.77x 10 ^-5 of 0.010 M NH₃

Calculate pH Using Ka = 1.75 x 10 ^-5 of 0.010 M NaC₂H₃O₂

Calculate pH Using Kb = 1.77 x 10 ^-5 of 0.010 M NH₄Cl

Answer 1

Answer : Here u have to acually first write the balanced equation and then by using ICE method you can solve it easily

1] Calculate pH Using Kw= 1.00X 10^-14 of 0.010 M HCl

here HCl ------------------------------- > H+ + Cl -

Hcl is trong acid will completely dissociate and hence we get H+ concentrtion = 0.010M

Ph = -Log[0.010] = 2

Hence the PH is = 2

2] Calculate pH Using Ka = 1.75 x 10^-5 of 0.010 M HC2H3O2

in case of monotropic we get

Ka = [X]²/ 0.010 -X = 1.75 * 10^-5

neglecting X we get 0.010-X = 0.010

X ² = 0.175 * 10^-6

X = 0.418 * 10^-3M

Hence concentration of H+ = 0.418 * 10^-3

Ph = - log [ 0.418 * 10^-3] = 2.62

Hence Ph = 2.62

3] Calculate pH 0.0010 M NaOH

POH = -log [ 0.0010] = 3

and we know that PH + POH = 14

Hence PH = 14-3 = 11

Hence the Ph value is 11

4] Calculate pH Using Kb= 1.77x 10 ^-5 of 0.010 M NH3

Here NH3 is stong base and hence POH = -Log [ 0.010] = 2

And Hence PH = 14 - 2 = 12

5} Calculate pH Using Ka = 1.75 x 10 ^-5 of 0.010 M NaC2H3O2

If it is mono basic. Now Kb = 10^-14 /1.75 * 10^-5 = 0.57 * 10^-9

Kb = X²/ 0.010 = 0.57 * 10^-9

X2 = 0.057 * 10^-10

X = 0.238 * 10^-5 M

POH = -log 0.238 * 10^-5 = 4.37

Ph = 14-4.37 = 9.63

Hence PH = 9.63

5] Calculate pH Using Kb = 1.77 x 10 ^-5 of 0.010 M NH4Cl

Kb = X² / 0.010 = 1.77 * 10^-5

X2 = 0.177 * 10^-6

X = 0.42 * 10^-3

poh = - log [ 0.42 * 10^-3] = 2.62

Ph = 11.38

Hecne this is all about the questions