You are given 30 Calculate the values of both pH and pOH of the following solutions: pOH pH 0.020M HNO3 2. 00050M KOH 3. A blood sample 7.2x10-8M of H 4. 4.251M Acetic acid 5. 0.00035M NaOH

Please explain in detail thank you!

h To add an 0 atom in basic solution, add 2 OH" to the side that needs the O atom, and also add an H20 to the other side. (OH has one more O than HOH). How many H20 molecules should be added to the left side? How many OH ions should be added to the right? H20 + CIO3 - CI" + OH Number of H50 molecules = 1 Number of OH ions =2

What is the pH of a solution that is 0.80M benzoic acid and 0.20 M sodium benzoate ? Ka HC6H5O2 = 6.3x10^-5  -> 3.1 -> 3.6  -> 4.2  -> 4.8  -> 6.3

A chemist titrates 150.0 mL of a 0.6575M hydrobromic acid (HBr) Solution with 0.4987M KOH Solution at 25 °C. Calculate the pH at equivalence. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH =

A 13.8 mL solution of 0.100 mol L-1 HOCl is titrated using 0.150 mol L-1 NaOH. What is the pH of the solution after 4.45 mL of the NaOH solution is added? Express your answer to 2 decimal places.

Which of the options below correctly describes what happens when a small amount of strong base is added to a buffer solution consisting of the weak acid HA its conjugate base A-? Oa. The concentration of H* increases and the pOH decreases. Ob. The concentration of H* increases and the pOH remains the same. Oc. The concentration of Ht decreases and the pOH decreases. Od. The concentration of H* remains the same and the pOH remains the same. Oe. The concentration of H* remains the same and the pOH increases.

Calculate the pH when 25.0 mL of 0.150 M HNO₃ is mixed with 40.0 mL of 0.250 M LiOH.

The pOH of a 0.0310 M solution of HCI is 1 2 3 5 6 C 7 8 +/- x 100 LO 4-

10. help please use sig figs