Determine the pH of a solution created by mixing 95.0 mL of 0.200 M nitric acid, HNO3, with 320.0 mL of 0.078 M potassium hydroxide, KOH.

Explanation:

We have to start with the reaction between nitric acid and potassium hydroxide:

With this in mind, we can calculate the number of moles of each compound if we use the molarity equation: (this means that we have to find the Litters dividing by 1000)

Now, we can calculate the moles:

If we have a molar ratio 1:1 (1 mol of reacts with 1 mol of ). So, if we have we will need . So, we have to calculate the amount of KOH that remains in the solution, so:

If we have an excess of KOH, this compound will be the cause of the pH value. Therefore we have to calculate the concentration. We already know the moles we have to calculate the volume. The total volume:

With this value, we can calculate the concentration of KOH:

We have to keep in mind that this compound is a base, so we have to calculate the pOH value first and then the pH:

If we remember that: 14 = pH + pOH we can find the pH value:

I hope it helps!

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :