KClO4 is salt of Strong base (KOH) and Strong acid (HClO4)
Both acid and base are strong
So, the salt KClO4 is neutral
So, its pH would be 7.00
Answer: 7.00
the pH and [s2-1 in a 0.21 M H2S solution. Assume Ka,-1.0x10-7. Ka,-1.0x10-19. Calculate pH [s2-] Calculate the pH of a 3.9x10 M solution of H2SO4 Need Help? Read it
the pH and [s2-1 in a 0.21 M H2S solution. Assume Ka,-1.0x10-7. Ka,-1.0x10-19. Calculate pH [s2-] Calculate the pH of a 3.9x10 M solution of H2SO4 Need Help? Read it
7. (a) Define pH (b) Calculate the pH of 0.030 M Ba(OH)2 solution (c) Calculate the pH of a solution containing 0.085 M nitrous acid alone and a solution containing 0.085 M nitrous acid and 0.10 M potassium nitrite (KNO2). K, for HNO2 = 4.5 x 10-
7) Calculate the pH of a 0.215 M NaCN solution. (5pts)
Calculate pH of 0.2 M solution of Tartaric acid. Calculate the volume of 1 M solution of NaOH required to neutralize 20 mL of 0.2 M tartaric acid solution (final pH should be 7). (pKa's of Tartaric acid are 3.0 and 4.4). 3.
1. Calculate the pH of a 0.543 M aqueous solution of codeine (C18H21O3N, Kb = 8.9×10-7). pH = 2. Calculate the pH of a 0.1250 M aqueous solution of piperidine (C5H11N, Kb = 1.3×10-3). pH = 3. Calculate the pH of a 0.0774 M aqueous solution of the weak base triethylamine ((C2H5)3N, Kb = 5.20×10-4). pH =
Calculate the pH and [S2-] in a 0.15 M H2S solution. Assume Ka, 1.0 x 10-7, Ka2 = 1.0 x 10-19. pH s2-1 Need Help? Read It Supporting Materials ■ Supplemental Data Periodic Table Constants & Factors 7. -6.25 points ZumChemP8 7.E.098. Calculate the pH of a 3.4x 10-3 M solution of H2SO4
7.(6 pts) Calculate the pH, [OH], and pOHl of a 0.0035 M HCl aqueous solution: 8. (6 pts) What are the [Hs0'1, (OH], and poH in a solution with a pH of 3.82? 9. (6 pts) What are the [H:0'], [OH], and pH in a solution with a pOH of 11.75? pH = pOH= , [OH'] = POH ' [OH'] = 10. (6 pts) Calculate the [H30, [OH1, and pH a 0.040 M Ba(OH)2 solution. [OH-11- pH=
7. (6 pts) Calculate the OH- concentration and pH of a 0.02 M ammonia solution.
7. Calculate the pH of a 2.7 M hydrofluoric acid solution. HF has a Ka = 6.6 x 104, Answer= PH=1.37 Need to know the steps
A 50.0 mL solution of 0.140 M KOH is titrated with 0.280 M HC1. Calculate the pH of the solution after the addition of each of the given amounts of HCI 0.00 mL pH = 11.84 5.00 mL pH = 12.5 mL pH = 12.74 19.0 mL pH = 12.38 24.0 mL pH = 11.56 25.0 mL pH = 7 31.0mL pH = 1.7
A 50.0 mL solution of 0.140 M KOH is titrated with 0.280 M HC1. Calculate the...