The pH of a basic solution is 8.65. What is [OH⁻]?

Calculate the pH of a solution when3.78grams of HCl was placed in 150.25 mL of water. HCl is a strong acid.

Strong acids and strong bases ionize 100% in aqueous solution.- HCl is a strong acid. In solution we write it as H+(aq) + Cl -(aq).- HF is a weak acid. In solution we write it as HF(aq).- KOH is a strong base. In solution we write it as K+(aq) + OH -(aq).- NH3 is a weak base. In solution we write it as NH3(aq).Exception: Since Ca(OH)2 is only slightly soluble we write it as Ca(OH)2(s).Below is a list of the 6 strong acids and 6 strong bases you should know. All other acids and bases are considered weak. Strong Acids Strong Bases HCl, HBr, HI LiOH, NaOH, KOH HNO3 Ca(OH)2 (slightly soluble) HClO4 Ba(OH)2 H2SO4 Sr(OH)2 Question 1)What is the hydronium ion concentration in an aqueous hydrobromic acid solution that has a pOH of 10.200?[H3O+] =  M

Determine the OH− in a solution with a pH of 3.7.

The concentration of hydroxide ion in an aqueous solution at 25°C is 7.3 × 10⁻⁴ M. What is the concentration of the hydronium ion?

2. An aqueous solution has a pH of 3.75. What is the hydronium ion concentration of the solution? Is the solution acidic or basic?

Determine the pH of an aqueous solution where [OH] = 6.0 x 10 10 M.

The autoionization constant for water at 35 °C is 2.2 × 10−14. Use this information to answer the following questions. a)What is the [H3O+] and pH of neutral water at 35 °C? b)Determine if the following solutions are acidic, neutral, or basic at 35 °C. Explain your answer. i)[H3O+] = 9.8 × 10−6 M ii)pH = 6.95 iii)[OH−] = 5.1 × 10−7 M iv)pOH = 9.24