What is the [H+] of a solution with a POH of 5.5? *

The answer to your question is [H⁺] = 3.16 x 10⁻⁹ M

Explanation:

Data

[H⁺] = ?

pOH = 5.5

Process

Calculate the pH, after that calculate the [H⁺]

1.- Calculate the pH

   pH + pOH = 14

-Solve for pH

    pH = 14 - pOH

-Substitution

    pH = 14 - 5.5

-Result

    pH = 8.5

2.- Calculate the [H⁺]

Formula

pH = -log[H⁺]

-Substitution

8.5 = -log[H⁺]

-Solve for [H⁺]

[H⁺] = antilog(-8.5)

-Result

[H⁺] = 3.16 x 10⁻⁹ M

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 :

conduction is the transfer of thermal energy (heat in transfer) due to collisions between the molecules in the object. collisions between adjacent atoms and molecules transfer kinetic energy from the warmer to the cooler object. the objects must be in physical contact.