Calculate the ph of 1.0 l of the original buffer upon addition of 0.010 mol of solid naoh to the original buffer solution.

This is an incomplete question, here is a complete question.

Consider a buffer solution that is 0.50 M in NH₃ and 0.20 M in NH₄Cl. For ammonia, pKb = 4.75.

Calculate the pH of 1.0 L of the original buffer upon addition of 0.010 mol of solid NaOH to the original buffer solution.

Answer : The pH of solution is, 9.68

Explanation : Given,

Concentration of NH₃ (base) = 0.50 M

Concentration of NH₄Cl (salt) = 0.20 M

Concentration of NaOH =

After addition of NaOH:

Concentration of NH₃ (base) = 0.50 + 0.01 = 0.51 M

Concentration of NH₄Cl (salt) = 0.20 - 0.01 = 0.19 M

First we have to calculate the value of pOH.

Using Henderson Hesselbach equation :

Now put all the given values in this expression, we get:

Now we have to calculate the pH.

Therefore, the pH of solution is, 9.68

answer: option (b) is the correct answer.

explanation:

a covalent bond is formed by sharing of electrons. whereas polarity arises due to difference in electronegativity of two atoms.

therefore, more is the electronegativity of an atom which combines with the titanium, more readily it will induce a partial positive and negative charge.

thus, out of the given options fluorine is most electronegative and has an incomplete octet. therefore, it will readily combine with titanium to share the electrons and complete its octet.  

2b2t

explanation:

2b2t