What is the [H3O-] and [OH-] ion concentration respectively in a solution that contains 0.155 M HNO3?   0.200 M, 5x10^-14 M   6.45x10^-14 M, 0.155 M   0.155 M, 6.45x10^-14 M   5x10^-14 M, 0.200 M

If the pH of a solution is 4.5, what is the [H3O+] of the solution? Hint [H3O+] = 10-PH 90.0 M 3.16x104 M 3.16x10-5 M 0.65 M 1.50 M

You find a very dilute solution of a very weak acid. Which of the following is true of the [H+] concentration of that solution? Concentration is 1.0*10-7 M Concentration is larger than 1.0*10^-7 M ○ Concentration is 7 Concentration is smaller than 1.0*10^-7 M

Determine the pH of a solution with [OH-] = 5.88 × 10-3 M.  Your answer should contain 3 decimal places as this corresponds to 3 significant figures when dealing with logs.    pH =

A 0.075 M solution of a base has a pH of 11.40.   What are the hydronium and hydroxide ion concentrations of this solution? [H3O^+] [OH^-]

For each strong base solution, determine [OH^-], [H3O^+], pH, and pOH. c) 1.9 x 10^-4 M KOH d) 5.0 x 10^-4 M Ca(OH)2

What are [H3O+], [OH−], and pOH in a solution with a pH of 3.40? [H3O+] = ___× 10^___ M [OH−] = ___× 10^___ M   I calculated the pH as 10.6, but I do not know where to go from here

What is [OH−] in a solution of 1.25 M NH3 and 0.78 M NH4NO3?

What is the pH of a 1.7 x 10^-3 M HI solution?