Buffer Preparation: There are several ways to prepare a buffer solution ofa specific pH. One method is mentioned in the manual. The other way is mentioned below but not in a correct order. Once the pH is adjusted to the desired pH, dilute the solution to the final desired volume. 1. Measure the pH of the solution using a pH meter. 2. 3. Adjust the plH to the desired value using a strong base or acil like NaOH or HCl. 4. Prepare a solution with an acid and its conjugate base by dissolving them in about so% of the volume of water required to obtain the final solution volume. What is the correcet order of preparing the buffer solution: 04.2.3.1 O1,3-4,1 04,1,2,1 Oa,3,14

Please answer the 3 boxes for ph

During a titration, it is found that 59.5 mL of a solution of NaOH is needed to neutralize a solution that contains 1.69 g HCL. What is the concentration of the NaOH solution?  a.) 0.3535m b.) 0. 6869m c.) 0. 7790m d.) 0. 6051m e.) 1.055m

The pH after adding 20.0 mL of 1.0 M NaOH to 25.0 mL of 1.0 M HCl is a. 0.95 b. 0.11 c. 0.70 d. 13.0

If I add an acid to a buffer solution, how will the buffer behave compared to pure water? Will the pH go up or down and will the change be large or small?

Hello can you help me answer question 2,3.a, and 3.b please? Thank you!

You are given a 0.25 M solution of an unknown weak base. Use 1/10th of dilution to find unknown weak base The diluted solution has a pH= 11.2. a) Write out an equation shows the reaction of base + waterb) What is the Ka and KB of weak base

The following are steps that you might need to perform in order to prepare a buffer. Choose the answer that puts the steps in the correct order. A. Add enough water to reach the final volume needed. B. Mass out the solid buffer salt. C. Take the pH of the buffer. D. Add -60% of the total volume of water. E. Add acid or base to reach the desired pH. Select one: O B, D, C, E, A O B, A, C, E ⒸB, D, C, E, Cx B, D, A, C, E

2. The pH of a 2.14 M solution of a weak base Bis measured to be 10.82 Determine K, of the base Determine K, of the weak bases's conjugate acid, HB* Determine [H*] in a 2.00 M solution of the chloride salt, HBCI Determine the pH of a 2.00 M solution of the chloride salt, HBCI

Need good explanation for question 4