A buffer consists of 0.120 m hno2 and 0.150 m nano2 at 25°c.

a. what is the ph of the buffer?

b. what is the ph after the addition of 1.00 ml of 11.6 m hcl to 1.00 l of the buffer solution?

A) pH of the buffer is 3.44

B) pH of the buffer solution is 3.37

Explanation:

Relation between K_{a} and pK_{a} is as follows.

.

The relation between pH and  pK_{a} is as follows.

pH of the buffer is 3.44.

b)

mol of HCl added = 11.6M *0.001 L = 0.0116 mol

In the given reaction, will react with to form

No. of moles of

And, no. of moles of

                                              = 0.12 mol

after the reaction :  

No. of moles of = moles present initially - moles added

                                         = (0.15 - 0.0116) mol

                                         = 0.1384 mol

Moles of = moles present initially + moles added

                = (0.12 + 0.0116)

                = 0.1316 mol

As,

Since, volume is both in numerator and denominator, we can use mol instead of concentration.

= 3.347+ log {0.1384/0.1316}

           = 3.369

           ≅ 3.37

pH after the addition of 1.00 mL of 11.6 M HCl to 1.00 L of the buffer solution is 3.37

hi,

the capital city of australia is canberra.

i just learnt this recently but i need to look through my notes again