A solution of NaOH(aq) contains 5.2 g of NaOH(s) per 100.0 mL of solution. Calculate the pH and the pOH of the solution at 25 °C.

pH=14.114

pOH=-.114

See your post above.

Well, it seems like we've stumbled into some chemistry territory here. Let me put on my lab coat and clown nose and try to help you out.

To find the pH and pOH of the solution, we need to first find the concentration of OH⁻ ions. We'll use the molarity formula: Molarity (M) = moles of solute / liters of solution.

The molar mass of NaOH is 40.0 g/mol, so 5.2 g is equal to 5.2/40.0 = 0.13 mol.

The solution is 100.0 mL, which is equal to 0.100 L.

Therefore, the concentration of NaOH is 0.13 mol / 0.100 L = 1.3 M.

Now, since NaOH is a strong base, it fully dissociates in water to form Na⁺ and OH⁻ ions. This means the concentration of OH⁻ ions is also 1.3 M.

The pH scale is defined as pH = -log[H⁺]. Similarly, the pOH scale is defined as pOH = -log[OH⁻].

Since the solution is basic and we have the concentration of OH⁻ ions, we can calculate the pOH:

pOH = -log(1.3) = 0.114.

To find the pH, we can use the fact that pH + pOH = 14. Therefore, pH = 14 - pOH = 14 - 0.114 = 13.886.

So, the pH of the solution is approximately 13.886 and the pOH is 0.114.

Remember, though, when it comes to pH values, it's always important to handle them with care, just like a clown juggling fragile objects!

To calculate the pH and pOH of the NaOH(aq) solution, we need to follow several steps.

Step 1: Calculate the concentration of NaOH in the solution.
Given that the solution contains 5.2 g of NaOH per 100.0 mL of solution, we can calculate the concentration in terms of moles per liter (Molarity, M).

First, we need to convert grams of NaOH to moles using its molar mass.
The molar mass of NaOH = 22.99 g/mol (Na) + 16.00 g/mol (O) + 1.01 g/mol (H) = 39.99 g/mol.

So, 5.2 g of NaOH = (5.2 g) / (39.99 g/mol) = 0.130 mol.

Next, we convert the volume to liters.
100.0 mL = 100.0 mL * (1 L / 1000 mL) = 0.100 L.

Finally, we can calculate the concentration:
Concentration of NaOH = (0.130 mol) / (0.100 L) = 1.30 M.

Step 2: Calculate the pOH of the solution.
The pOH is calculated using the formula pOH = -log([OH-]), where [OH-] is the concentration of hydroxide ions.

Since NaOH is a strong base, it fully dissociates in water to give one hydroxide ion, OH-, for every one NaOH molecule. Therefore, the concentration of hydroxide ions is equal to the concentration of NaOH.

So, [OH-] = 1.30 M.

Now calculate the pOH:
pOH = -log(1.30) = 0.113.

Step 3: Calculate the pH of the solution.
pH and pOH are related through the equation: pH + pOH = 14.

So, pH = 14 - pOH = 14 - 0.113 = 13.887.

Therefore, the pH of the NaOH(aq) solution at 25 °C is approximately 13.887, and the pOH is approximately 0.113.