Determine the pH of the following solutions.
1) 0.600 M HCl
2) 0.052 moles of H2SO4 dissolved in 4.2 L of water.
3)5.6 grams HNO3 dissolved in 450 ml of water.
4) 2.5 grams of NaOH dissolved in 500 mL of water.
5) adding 2 grams NaH dissolved in 0.56 L of water.
6) 20 mL of 0.27 M HNO3 is diluted to 500 mL.
All of these are the pH values for strong or weak acids. What is it you don't understand. Be specic.
You have to determine the pH of these solutions. These are acid-base questions.
I know that. What is your problem in understanding these. Be specific. I need to know what you don't understand so I'll know where to start explaining.
I think I understand 1) and 2) but I do not understand how to calculate the pH when it is dissolved and diluted.
To determine the pH of a solution, you need to know the concentration of the hydrogen ions (H+) in the solution. There are different methods to calculate it depending on the information given. I will guide you step by step for each of the solutions:
1) 0.600 M HCl:
Since HCl is a strong acid, it completely dissociates in water, leading to the formation of H+ ions and Cl- ions. In this case, the concentration of H+ is the same as the initial concentration of HCl, so the H+ concentration is 0.600 M. To find the pH, you can use the formula: pH = -log[H+].
2) 0.052 moles of H2SO4 dissolved in 4.2 L of water:
H2SO4 is a strong acid that dissociates into 2 H+ ions and 1 SO4^2- ion. First, calculate the new concentration of H+ ions by dividing the moles of H2SO4 by the volume of the solution in liters (0.052 moles / 4.2 L). Then, use the formula pH = -log[H+] to find the pH.
3) 5.6 grams HNO3 dissolved in 450 mL of water:
To calculate the concentration in moles per liter, you need to convert grams to moles. In this case, divide the mass of HNO3 by its molar mass. Then, divide the obtained moles by the volume of the solution in liters (450 ml = 0.45 L). Finally, use the formula pH = -log[H+] to find the pH.
4) 2.5 grams of NaOH dissolved in 500 mL of water:
Again, you need to calculate the concentration in moles per liter. Convert grams to moles by dividing the mass of NaOH by its molar mass. Then, divide the obtained moles by the volume of the solution in liters (500 ml = 0.5 L). NaOH is a strong base that completely dissociates into Na+ and OH- ions. From this, you can calculate the concentration of OH- ions. Finally, use the formula pOH = -log[OH-], and then pH = 14 - pOH to find the pH.
5) Adding 2 grams NaH dissolved in 0.56 L of water:
First, convert grams of NaH to moles by dividing the mass by its molar mass. Then, divide the obtained moles by the volume of the solution in liters (0.56 L). NaH is a strong base that completely dissociates into Na+ and H- ions. From this, you can calculate the concentration of H- ions. Finally, use the formula pH = -log[H+] to find the pH.
6) 20 mL of 0.27 M HNO3 is diluted to 500 mL:
First, calculate the moles of HNO3 in the original solution by multiplying the concentration by the volume in liters (20 ml = 0.02 L). Then, calculate the new concentration of HNO3 after dilution by dividing the moles of HNO3 by the final volume of the solution in liters (500 ml = 0.5 L). Finally, use the formula pH = -log[H+] to find the pH.
Remember, in cases where a weak acid or base is involved, you may need to consider additional calculations based on equilibrium constants and dissociation equations.