For each strong acid solution, determine [H 3 O + ], [OH – ], and pH. b. 0.015 M HNO 3

Step 1: Recognize that HNO 3 is a strong acid, which means it completely dissociates in water. Therefore, the concentration of H 3 O + ions will be equal to the initial concentration of the acid, which is 0.015 M.. Step 2: Use the relationship between the concentrations of H 3 O + and OH - ions in water, given by the ion product of water: K w = [H 3 O + ][OH - ] = 1.0 x 10 -14 at 25°C.. Step 3: Calculate the concentration of OH - ions using the formula: [OH - ] = K w / [H 3 O + ]. Substitute the known values to find [OH - ].. Step 4: Determine the pH of the solution using the formula: pH = -log[H 3 O + ]. Substitute the concentration of H 3 O + to find the pH.. Step 5: Review your calculations to ensure that the values for [H 3 O + ], [OH - ], and pH are consistent with the properties of a strong acid solution.

For each strong acid solution, determine [H 3 O + ], [OH – ], and pH. b. 0.015 M HNO 3

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.16 - Acids and Bases

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Ch.16 - Acids and Bases

Problem 57b

Chapter 16, Problem 57b

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. b. 0.015 M HNO₃

Verified step by step guidance

Step 1: Recognize that HNO3 is a strong acid, which means it completely dissociates in water. Therefore, the concentration of H3O+ ions will be equal to the initial concentration of the acid, which is 0.015 M.

Step 2: Use the relationship between the concentrations of H3O+ and OH- ions in water, given by the ion product of water: Kw = [H3O+][OH-] = 1.0 x 10-14 at 25°C.

Step 3: Calculate the concentration of OH- ions using the formula: [OH-] = Kw / [H3O+]. Substitute the known values to find [OH-].

Step 4: Determine the pH of the solution using the formula: pH = -log[H3O+]. Substitute the concentration of H3O+ to find the pH.

Step 5: Review your calculations to ensure that the values for [H3O+], [OH-], and pH are consistent with the properties of a strong acid solution.

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Key Concepts

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

Strong Acids

Strong acids, such as HNO3 (nitric acid), completely dissociate in water, meaning that all the acid molecules break apart into their constituent ions. This results in a high concentration of hydronium ions ([H3O+]) in solution, which is crucial for calculating pH and hydroxide ion concentration ([OH-]).

pH Calculation

The pH of a solution is a measure of its acidity, calculated using the formula pH = -log[H3O+]. For strong acids, the concentration of hydronium ions is equal to the molarity of the acid solution, allowing for straightforward pH calculations. A lower pH value indicates a more acidic solution.

Water Ion Product

The water ion product (Kw) is the equilibrium constant for the self-ionization of water, defined as Kw = [H3O+][OH-] = 1.0 x 10^-14 at 25°C. This relationship allows for the determination of hydroxide ion concentration ([OH-]) from the known hydronium ion concentration, using the equation [OH-] = Kw / [H3O+].

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Textbook Question

Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH of an acid solution should carry as many digits to the right of the decimal place as the number of significant figures in the concentration of the solution. [H₃O⁺] = 0.044 M [H₃O⁺] = 0.045 M [H₃O⁺] = 0.046 M

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Textbook Question

Determine the concentration of H₃O⁺ to the correct number of significant figures in a solution with each pH. Describe how these calculations show the relationship between the number of digits to the right of the decimal place in pH and the number of significant figures in concentration. pH = 2.50 pH = 2.51 pH = 2.52

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Textbook Question

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. a. 0.25 M HCl

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. c. a solution that is 0.052 M in HBr and 0.020 M in HNO₃

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Textbook Question

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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Textbook Question

Determine the pH of each solution. a. 0.048 M HI b. 0.0895 M HClO₄ c. a solution that is 0.045 M in HClO₄ and 0.048 M in HCl d. a solution that is 1.09% HCl by mass (assume a density of 1.01 g/mL for the solution)

For each strong acid solution, determine [H3O+], [OH–], and pH. b. 0.015 M HNO3

Verified Solution

Key Concepts

Strong Acids

pH Calculation

Water Ion Product

For each strong acid solution, determine [H₃O⁺], [OH^–], and pH. b. 0.015 M HNO₃