Determine [H30+], [OH-], and pH.

A solution that is 0.655% HNO3 by mass (assume a density of 1.01 g/ mL for the solution).

Well, water isn't the only thing that's acidic around here! We've got ourselves a feisty solution of HNO3. Let's break it down, shall we?

First, we need to determine the molarity of the solution. To do that, we'll need to know the molar mass of HNO3.

HNO3 has a molar mass of approximately 63 g/mol. So, let's calculate the number of moles of HNO3 in our solution:

0.655% of the solution by mass is HNO3. Considering the density of 1.01 g/mL, we can calculate the mass of HNO3 present in one milliliter of the solution:

0.655% * 1.01 g/mL = 0.0066255 g/mL

Now, let's convert grams to moles using the molar mass:

0.0066255 g/mL * (1 mol/63 g) = 1.0519 x 10^-4 mol/mL

Since the density of water is approximately 1 g/mL, we can assume that the volume of the solution in milliliters is equal to its mass in grams. So, we have:

1.0519 x 10^-4 mol/mL * 1000 mL = 0.10519 mol

Now, let's move on to the hydronium ion concentration, [H3O+]. In a strong acid like HNO3, all the acid molecules dissociate to release H3O+ ions. Since the molarity of our solution is the same as the hydronium ion concentration, we can conclude that [H3O+] = 0.10519 M.

As for the hydroxide ion concentration, OH-, in our acidic solution, it is extremely low since this is a strong acid. We can safely assume it's negligible.

Now, to find the pH, we'll use the equation:

pH = -log[H3O+]

pH = -log(0.10519)

And after doing some math, the pH of this solution is approximately 0.979.

Even though this solution has a low pH, don't let it get under your skin! Just embrace the acidic side of life, my friend.

To determine the [H3O+], [OH-], and pH of the solution, we need to consider the dissociation of HNO3 in water.

Step 1: Calculate the molarity of HNO3 in the solution.
To determine the molarity, we need to know the molecular weight of HNO3. The molecular weight of HNO3 is 63 g/mol (1H + 1N + 3O).

Given that the solution is 0.655% HNO3 by mass, we can assume we have 0.655 g of HNO3 in a 100 g solution (since 0.655% is equivalent to 0.655 g/100 g).

Now, we can calculate the number of moles of HNO3:
moles of HNO3 = mass of HNO3 / molecular weight of HNO3
= 0.655 g / 63 g/mol
≈ 0.0104 mol

Next, we need to find the volume of the solution (in liters) to calculate the molarity:
volume of the solution = mass of the solution / density of the solution
= 100 g / 1.01 g/mL
= 99.01 mL
≈ 0.0990 L

Now, we can calculate the molarity of the HNO3 solution:
molarity (M) = moles of solute / volume of solution (in liters)
= 0.0104 mol / 0.0990 L
≈ 0.105 M

Step 2: Determine the [H3O+], [OH-], and pH.

In the dissociation of HNO3, it completely ionizes to form H3O+ and NO3- ions.

Since HNO3 is a strong acid, we can assume that it fully dissociates in water, meaning that the concentration of HNO3 (0.105 M) is equal to the concentration of H3O+ ions.

Therefore, [H3O+] = 0.105 M

To calculate [OH-], we can use the equation:
[H3O+] × [OH-] = 1.0 × 10^-14

Plugging in the value of [H3O+] = 0.105 M, we can solve for [OH-]:
0.105 M × [OH-] = 1.0 × 10^-14
[OH-] = (1.0 × 10^-14) / 0.105 M
≈ 9.52 × 10^-14 M

To calculate the pH, we can use the equation:
pH = -log[H3O+]

Plugging in the value of [H3O+] = 0.105 M, we can solve for pH:
pH = -log(0.105)
≈ 0.98

Therefore, the [H3O+] is approximately 0.105 M, [OH-] is approximately 9.52 × 10^-14 M, and the pH is approximately 0.98.

To determine [H3O+], [OH-], and pH of a solution, we first need to understand the concept of acidity and alkalinity.

Acidity is determined by the concentration of hydrogen ions (H+) in a solution, while alkalinity is determined by the concentration of hydroxide ions (OH-) in a solution. The concentration of H+ ions in a solution is quantified by pH, which is a measure of the acidity or alkalinity of a solution on a logarithmic scale ranging from 0 to 14.

In order to calculate [H3O+], [OH-], and pH, we need to know the concentration of HNO3 in the given solution, as well as the dissociation reaction of HNO3 in water.

The dissociation reaction of HNO3 in water is as follows:
HNO3 + H2O -> H3O+ + NO3-

The equation tells us that one molecule of HNO3 produces one H3O+ ion and one NO3- ion.

Let's start the calculation.

Step 1: Convert the given percentage of HNO3 to grams.
Assuming a total mass of 100g for the solution, the mass of HNO3 is:
0.655% of 100g = 0.655g

Step 2: Calculate the number of moles of HNO3.
To calculate the number of moles, we need to know the molar mass of HNO3, which is:
H = 1.007g/mol
N = 14.007g/mol
O = 16.00g/mol

Adding these values, we get:
Molar mass of HNO3 = (1 x 1.007) + (1 x 14.007) + (3 x 16.00) = 63.012 g/mol

Number of moles of HNO3 = Mass of HNO3 / Molar mass of HNO3
= 0.655g / 63.012 g/mol

Step 3: Calculate the molarity of HNO3.
Since we know the volume of the solution, we can calculate the molarity using the equation:

Molarity (M) = Number of moles / Volume in liters

First, we need to convert the density of the solution from grams per milliliter to grams per liter.
Density of the solution = 1.01 g/mL

To convert to g/L, we multiply by 1000:
Density of the solution = 1.01 g/mL x 1000 mL/L = 1010 g/L

Next, we need to calculate the volume (V) of the solution in liters.
To do this, we divide the mass of the solution by its density:
Volume (V) = Mass of solution / Density of solution
= 100g / 1010 g/L
= 0.099 L

Now we can calculate the molarity of HNO3:
Molarity (M) = Number of moles / Volume in liters
= (0.655g / 63.012 g/mol) / 0.099 L

Step 4: Calculate [H3O+], [OH-], and pH using the molarity of HNO3.

Since HNO3 is a strong acid, it fully dissociates, resulting in equal amounts of H3O+ and NO3- ions. Therefore, the concentration of H3O+ ions would be the same as the molarity of HNO3.

[H3O+] = Molarity of HNO3

Now, since the solution is neutral (neither acidic nor alkaline), the concentration of [OH-] is equal to the concentration of [H3O+]. Therefore, [OH-] = [H3O+].

Finally, we can calculate the pH using the formula: pH = -log10([H3O+]).

Plug in the value of [H3O+] from step 4 into the pH formula to get the pH of the solution.

Take a 1000 mL sample.

1000 mL x (1.01 g/mL) x 0.00655 x (1/molar mass HNO3) = Molarity of the HNO3 solution.

Since HNO3 is a strong acid (it ionizes 100%) then
(H3O^+) = (HNO3) and pH = -log(H3O^+)
Since pH + pOH = pKw = 14, you can get pOH from that and OH comes from pOH = -log(OH^-)