Textbook Question
Calculate the pH of each of the following strong acid solutions: (b) 1.52 g of HNO3 in 575 mL of solution
Ch.16 - Acid-Base Equilibria
Chapter 16, Problem 44
Calculate the pH of each of the following strong acid solutions: (a) 0.0167 M HNO3 (b) 15.00 mL of 1.00 M HCl diluted to 0.500 L (c) a mixture formed by adding 50.0 mL of 0.020 M HCl to 125 mL of 0.010 M HI.
Verified step by step guidance1
For part (a), recognize that HNO3 is a strong acid, which means it completely dissociates in water. The concentration of H+ ions is equal to the concentration of the acid. Therefore, [H+] = 0.0167 M. Use the formula for pH: \( \text{pH} = -\log[H^+] \) to find the pH.
For part (b), first calculate the number of moles of HCl before dilution using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \). Here, \( \text{moles of HCl} = 1.00 \text{ M} \times 0.01500 \text{ L} \). Then, find the new concentration after dilution by dividing the moles of HCl by the new volume (0.500 L). Finally, calculate the pH using \( \text{pH} = -\log[H^+] \).
For part (c), calculate the moles of HCl and HI separately. For HCl: \( \text{moles} = 0.020 \text{ M} \times 0.0500 \text{ L} \). For HI: \( \text{moles} = 0.010 \text{ M} \times 0.125 \text{ L} \).
Add the moles of HCl and HI together to get the total moles of H+ ions in the solution. Then, calculate the total volume of the solution by adding the volumes of HCl and HI: \( 0.0500 \text{ L} + 0.125 \text{ L} \).
Determine the concentration of H+ ions in the mixture by dividing the total moles of H+ by the total volume of the solution. Finally, calculate the pH using \( \text{pH} = -\log[H^+] \).
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 HNO3 and HCl, 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 strong acids, this simplifies the calculation since the pH can be directly derived from the molarity of the acid.
Recommended video:
Guided course
02:39
pH of Strong Acids and Bases
Dilution and Concentration
When a solution is diluted, the number of moles of solute remains constant, but the volume increases, resulting in a lower concentration. The dilution can be calculated using the formula C1V1 = C2V2, where C1 and V1 are the initial concentration and volume, and C2 and V2 are the final concentration and volume. This concept is crucial for determining the pH of diluted strong acid solutions.
Recommended video:
Guided course
00:58Dilution Equation
Mixing Solutions and Total Volume
When mixing two solutions, the total concentration of hydrogen ions must be calculated based on the volumes and concentrations of each solution. The total volume after mixing affects the final concentration of H+. The combined concentration can be found using the formula: [H+] = (C1V1 + C2V2) / (V1 + V2), which is essential for accurately calculating the pH of the resulting mixture.
Recommended video:
Guided course
02:35Constant-Volume Calorimetry