What is the pH of a 1.5x10-3M solution of NaOH, a strong base

The answer to your question is pH = 11.18

Explanation:

Data

pH = x

Concentration = 1.5 x 10⁻³ M

Formula

pOH = -log[OH]

pH +pOH = 14

Process

1.- Calculate the pOH of the solution

pOH = -log[1.5 x 10⁻³]

pOH = 2.82

2.- Calculate the pH of the solution

pH + pOH = 14

solve for pH

pH = 14 - pOH

pH = 14 - 2.82

pH = 11.18

The pH of the solution is 11.18

Explanation:

Step 1: Data given

Concentration NaOH solution = 1.5 * 10^-3 M

Step 2: Calculate pOH

pH = log[H+]

pOH = -log [OH-]

pOH = -log (1.5*10^-3)

pOH = 2.82

Step 3: Calculate pH

pH + pOH = 14

pH = 14 - pOH

pH = 14 -2.82

pH = 11.18

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.

i do not get it   at all