For each strong acid solution, determine [H 3 O + ], [OH – ], and pH. d. a solution that is 0.655% HNO 3 by mass (assume a density of 1.01 g/mL for the solution)

Hey everyone, we're asked what is the ph concentration of hydrogen ions and the concentration of hydroxide ions for a 0.732% per clark acid by mass of a strong acid solution with a density of 1.2 g per meal leader since we have a strong acid, we know that this is going to dissociate completely and we can go ahead and assume that we have 100 g of solution. This will also make it easier for us to convert from percentage Instagram's first. Taking our 0.732%, we can convert this into grams of solution per g of solution. We then want to use the density for our dimensional analysis. So we have 1.02 g of solution per one mil liter of solution. Now, using the molar mass of per clark acid, we know that we have 100.46 g of per clark acid Per one mole of per caloric acid. Next we want to convert our milliliters of solution into liters of solution for our denominator. So we know we have 10 to third milliliters of solution for one liter of solution. So when we calculate this out and cancel out all of our units, we end up with a polarity of 0. moller a perk Lorik acid, which is going to be the concentration of our hydro ni um ions. Now let's go ahead and write out our reaction. So we have our per caloric acid and this is going to react with our water. Since it is a strong acid, it will completely dissociate to those hydro ni um ions and those per chlorine ions. Now let's go ahead and calculate our ph we know that our ph is the negative log of our hydro ni um ion concentration. So, plugging that in, we get the negative log of 0.07432, which will get us to a ph of 1.129. And lastly, we want to calculate the concentration of our hydroxide ions and we're going to use our KW, which is one times 10 to the negative 14 And divide that by the concentration of hydrogen ions which was 0. Molar. This will get us to a concentration of 1.35 times 10 to the - Mueller. And these are going to be our final answers Now, I hope this made sense. And let us know if you have any questions

Ch.17 - Acids and Bases

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Tro 6th Edition

Ch.17 - Acids and Bases

Problem 61d

Chapter 17, Problem 61d

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. d. a solution that is 0.655% HNO₃ by mass (assume a density of 1.01 g/mL for the solution)

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Convert the percentage concentration of HNO₃ to a molarity. Start by assuming you have 100 g of the solution, which means you have 0.655 g of HNO₃.

Calculate the number of moles of HNO₃ using its molar mass (63.01 g/mol).

Determine the volume of the solution in liters using the given density (1.01 g/mL).

Calculate the molarity of the HNO₃ solution by dividing the moles of HNO₃ by the volume of the solution in liters.

Since HNO₃ is a strong acid, it dissociates completely in water. Therefore, [H₃O⁺] is equal to the molarity of the HNO₃ solution. Use this to find [OH⁻] using the water dissociation constant (K_w = 1.0 x 10⁻¹⁴) and calculate the pH using the formula pH = -log[H₃O⁺].

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Strong Acids and Ionization

Strong acids, like HNO3, completely dissociate in water, meaning that all the acid molecules break apart into ions. For HNO3, this results in a concentration of hydronium ions [H3O+] equal to the concentration of the acid. Understanding this complete ionization is crucial for calculating the concentrations of [H3O+] and [OH-] in the solution.

pH Calculation

The pH of a solution is a measure of its acidity, defined as the negative logarithm of the hydronium ion concentration: pH = -log[H3O+]. For strong acids, where [H3O+] can be directly determined from the acid concentration, calculating pH becomes straightforward. This concept is essential for determining the acidity of the solution in question.

Concentration and Density

To find the molarity of the HNO3 solution, we need to convert the mass percentage to moles per liter using the solution's density. The mass percentage indicates how many grams of solute are present in a certain mass of solution, and the density allows us to convert this mass into volume. This step is critical for accurately determining the concentrations of [H3O+] and [OH-].