What is ph when 4.0 ml of 2.0 m barium hydroxide is added to 10.0 ml of 1.00 m nitric acid? 13.63 0.37 0.85 13.15

Answer : The pH of the solution will be 13.63.

Solution:

Moles of hydroxide ions in barium hydroxide solution

Number of moles = (concentration)(volume in liters) ...(1)(1L=1000mL)

2.0 M barium hydroxide in solution

Number of moles of in 2.0 M solution moles

If One mole of barium hydroxide gives two moles of hydroxide in solution then 0.008 moles will give:

Number of moles of   moles

Moles of ions in nitric acid

In 1.00 M nitric acid solution

Moles of nitric acid in 1.0 M solution moles

If one mole of nitric acid will give one moles of ion.

Then 0.010 moles of nitric acid in solution will give :

Number of moles of   moles

Since , the reaction will be neutralization reaction, equal number of moles of will neutralize equal number of moles of

So,0.010 moles of will neutralize 0.010 moles of in the solution

Remaining moles of moles

Concentration of resulting solution

Resulting volume of the solution : 0.004 + 0.010 liters

Calculating by using equation (1).

The pH of the solution will be 13.633.

lol for the pointsss