Determine the pH of each solution. a. 0.048 M HI b. 0.0895 M HClO 4 c. a solution that is 0.045 M in HClO 4 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)

Step 1: Understand the nature of the acids involved. HI and HClO 4 are strong acids, meaning they dissociate completely in water. This means the concentration of H + ions in the solution is equal to the concentration of the acid.. Step 2: Calculate the pH for each solution using the formula: \( \text{pH} = -\log[\text{H}^+] \). For part (a), use the concentration of HI, which is 0.048 M.. Step 3: For part (b), use the concentration of HClO 4 , which is 0.0895 M, to find the pH using the same formula.. Step 4: For part (c), since both HClO 4 and HCl are strong acids, add their concentrations to find the total [H + ] and then calculate the pH.. Step 5: For part (d), convert the percentage concentration of HCl to molarity. Use the formula: \( \text{Molarity} = \frac{\text{mass percent} \times \text{density} \times 10}{\text{molar mass of HCl}} \). Then, calculate the pH using the molarity obtained.

Determine the pH of each solution. a. 0.048 M HI b. 0.0895 M HClO 4 c. a solution that is 0.045 M in HClO 4 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)

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

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)

Step 1: Understand the nature of the acids involved. HI and HClO 4 are strong acids, meaning they dissociate completely in water. This means the concentration of H + ions in the solution is equal to the concentration of the acid. Step 2: Calculate the pH for each solution using the formula: \( \text{pH} = -\log[\text{H}^+] \). For part (a), use the concentration of HI, which is 0.048 M. Step 3: For part (b), use the concentration of HClO 4 , which is 0.0895 M, to find the pH using the same formula. Step 4: For part (c), since both HClO 4 and HCl are strong acids, add their concentrations to find the total [H + ] and then calculate the pH. Step 5: For part (d), convert the percentage concentration of HCl to molarity. Use the formula: \( \text{Molarity} = \frac{\text{mass percent} \times \text{density} \times 10}{\text{molar mass of HCl}} \). Then, calculate the pH using the molarity obtained.

Ch.16 - Acids and Bases

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Tro 4th Edition

Ch.16 - Acids and Bases

Problem 58

Chapter 16, Problem 58

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)

Verified step by step guidance

Step 1: Understand the nature of the acids involved. HI and HClO₄ are strong acids, meaning they dissociate completely in water. This means the concentration of H⁺ ions in the solution is equal to the concentration of the acid.

Step 2: Calculate the pH for each solution using the formula: \( \text{pH} = -\log[\text{H}^+] \). For part (a), use the concentration of HI, which is 0.048 M.

Step 3: For part (b), use the concentration of HClO₄, which is 0.0895 M, to find the pH using the same formula.

Step 4: For part (c), since both HClO₄ and HCl are strong acids, add their concentrations to find the total [H⁺] and then calculate the pH.

Step 5: For part (d), convert the percentage concentration of HCl to molarity. Use the formula: \( \text{Molarity} = \frac{\text{mass percent} \times \text{density} \times 10}{\text{molar mass of HCl}} \). Then, calculate the pH using the molarity obtained.

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Key Concepts

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

Strong Acids and pH Calculation

Strong acids, such as HI and HClO4, completely dissociate in water, meaning that the concentration of hydrogen ions (H+) in solution is equal to the concentration of the acid. The pH of a solution is calculated using the formula pH = -log[H+]. For example, a 0.048 M HI solution will have a pH of -log(0.048), which can be computed directly.

Mixed Acid Solutions

When dealing with mixed acid solutions, such as the one containing both HClO4 and HCl, the total concentration of H+ ions is the sum of the contributions from each acid. Since both are strong acids, their concentrations can be added directly to find the total H+ concentration, which is then used to calculate the overall pH of the solution.

Mass Percent Concentration to Molarity Conversion

To determine the pH of a solution given in mass percent, such as 1.09% HCl, it is necessary to convert this to molarity. This involves calculating the mass of HCl in a given volume of solution, using the density to find the volume, and then converting the mass to moles using the molar mass of HCl. The resulting molarity can then be used to find the pH.