WebbOne "rule of thumb" that I learned is if your x ends up being larger than 5% of your starting value you need to solve the quadratic. Let's say that you started with an initial concentration of 5*10-8 M NH4Cl and you solve this problem using the method shown. You will find x = 5.27*10-9 x is (5.27*10-9/5*10-8)*100% = 10.5% of starting value Webb16 mars 2024 · To calculate the pH of a solution: Measure the concentration of hydrogen ion in the solution. Alternatively, you can measure the activity of the same species. We …
Answered: 2. 100.0 mL of a 0.0875 M weak base… bartleby
WebbAfter 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid. Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M NH3 (Kb = 1.8 105) with 0.100 M HCl. WebbWhat is the pH of the solution formed when 0.060 moles NaOH is... Expert Help. Study Resources. Log in Join. Science. Chemistry. 15. What is the pH of the solution formed when 0.060 moles NaOH is ... The pH of the solution formed when 0.060 moles of NaOH is added to 1.0 L of 0.050 M HCl is 12.00. ... assaasdf
The pH of a 10^-10 molar HCl solution is approximately
Webbinitial pH, before the addition of strong base. In dealing with strong acids and bases, assume that they dissociate completely in water. [H+] = [HCl] In this example, we have a 0.1 M solution of HCl, so the [H+] = 0.1 M - log (0.1) = 1 … WebbSolution for Calculate the pH change that results when 12 mL of 2.1 M HCl is added to 560. mL of each of the following solutions. a solution that is 0.10 M ... A solution is made up of 273 mL of 0.164 M HNO3 and 0.800 M HCl. The resulting pH of the solution is 0.39. How many mL of HCl are used to make up the solution? Assume volumes are additive. WebbAnswer: You need to bear in mind: 1. pH = -log[H+] 2. HCl is a strong acid, completely dissociated in water. Therefore, a concentration of HCl = 2*10^-8 M 3. H2O dissociates … lakshman jhula scene